physical chemistry objective

Single Correct Choice Type01.The crystal structure with no element of symmetry is. a) Rhombohedralb) Monoclinicc) Triclinicd) Orthorhombic

02.How many octahedral sites per sphere are there in a cubic closest packed (face-centred cubic) structure?a) 1b) 8c) 6d) 3

03.Which among the following will bring about the coagulation of gold sol quickest and in the least of molar concentration?

a) NaClb) c) d)

04.At the vapour pressure of methyl alcohol is 96 torr. The mole fraction of methyl alcohol in a solution in which the partial vapour pressure of methyl alcohol is 23 torr at is

a) b) c) d)

05.An ionic compound AB crystallises in FCC lattice. The radius ratio of the compound is 0.5. If all the ions along one of the axes passing through face centres are removed, the percentage of the volume occupied by the cations/unit cell is a) 74b) 37c) 27.75d) 6

06.On adding few drops of dil.HCl to freshly precipitated ferric hydroxide, a red coloured colloidal solution is obtained. This phenomenon is known asa) Protective actionb) Coagulationc) Peptisationd) Dialysis

07.Which of the following 1m solutions has highest depression in freezing point?a) aq. Glucose solution

b) aq. which is 50% ionized

c) which is 30% ionizedd) aq. NaCl which is 100% ionised

08.The graph between and log P is a straight line inclined at an angle and log K = 0.699. Then the amount in grams of adsorbate adsorbed per gram of adsorbent when the pressure is 0.2 atm isa) 1b) 2c) 5d) 2.5

01.The lowering of vapour pressure due to the solute in a 3 m aqueous solution at is approximatelya) 14 torrb) 28 torrc) 40 torrd) 7.6 torr

02.Which of the following is an example of associated colloid?

a) b)rubber + benzenec) Soap + waterd) Protein + water

03.An ionic compound AB crystallizes in B.C.C. lattice. If the radius ratio is almost one, the ratio of volumes occupied by cation to that of anion in the unit cell is

a) b) c) d) 1

04.NaF and NaI are dissolved in water to prepare 100ml solution which produces the same osmotic effects as 0.1 molar solution of urea in water at the same temperature. The solution on complete evaporation left a residue of 0.48g. Then the ratio of weights of NaF to NaI added to water isa) 0.14b) 0.28c) 0.46d) 0.75

05.According to adsorption theory of catalysis, the reaction rate increases becausea) In the process of adsorption, the kinetic energy of the molecules increasesb) The activation energy of reaction becomes high due to adsorptionc) Adsorption produces heat which increases the rate of reactiond) The concentration of reactants at the active centres becomes high due to adsorption.

06.An element (Molecular weight = 200) has an atomic radius of . The density of that element is 7 g/cc. The crystal structure of the element isa) Simple cubicb) BCCc) FCCd) HCP.4.Fully charged lead storage battery contains 1.5 L of 5.00 M H2SO4. If 2.5 amp of current is drawn for 965 minutes, then final left concentration of H2SO4 is (Assume volume of battery fluid to be constant.)(A)3.5 M(B)2.00(C)4.25 M(D)4.00 M3.Consider the plots of radial wave function R(n, l) (r) against r for electrons belong to different orbitals.

The number of radial nodes in each of these orbitals respectively is(A) 1, 2, 3 (B) 0, 1, 2 (C) 1, 1, 1 (D) 2, 2, 2

1.An oxide of a metal has the formula M2O3. When 0.16g of the oxide on being reduced to pure metal by hydrogen 54mg of water are formed. Hence the atomic mass of the metal isA) 27B) 159.6C) 79.0D) 55.82.The extent of dissociation of N2O4 is 40% at 270C under a pressure of 760 mm Hg. Hence the density of the equilibrium mixture of N2O4 and NO2 in g/L would beA) 4.85B) 2.67C) 3.82D) 3.183.A certain mass of NH4Cl was boiled with 200mL of 0.6M NaOH until the reaction is completed. After that, the reaction mixture containing excess of NaOH on being titrated, it required 100 mL of 0.4N HCl. Hence the mass of NH4Cl taken to start with [M.M. of NH4Cl = 53.5]A) 2.14 gB) 6.42 gC) 4.28 gD) 8.56 g4.Two moles of an ideal gas expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. the enthalpy change (in kJ) for the process is:A) 11.4B) -11.4C) 0D) 4.88.Which electronic transition in a hydrogen atom, starting from the orbit n = 7, will produce infrared light of wavelength 2170 nm? (Given : RH = 1.09677 107 m-1)A) n = 7 to n = 6B) n = 7 to n = 5C) n = 7 to n = 4D) n = 7 to n = 3

1.Ksp of AgCN is and Ka of HCN is . Hence the solubility of AgCN in a buffer solution of pH equal to 3 in mol/L

A) B) C) D) 2.A mixture of N2(g), H2(g) and NH3(g) is present in a 10L flask at equilibrium as per the equation.

and the equilibrium constant at a particular temperature is 10. In case the molar concentrations of H2 and NH3 are 1.0 and 0.5, the number of moles of N2 present in the flask.A) 0.5B) 5.0C) 6.25D) 0.25

2.In mineral wurtzite, iron oxide is usually non-stoichiometric with approximate formula . What is percentage of cationic sites are occupied by ? (A) 5.2%(B) 30%(C) 19.78%(D) 8.88%3.Which of the following relation is true in respect of adsorption?

(A)

(B)

(C)

(D)

1.KCl crystallizes in the same type of lattice as does NaCl. Given that and . Calculate ratio of the side of unit cell for KCl to that for

(A) (B) (C) (D)

3.A graph of Vs is plotted as shown below. What will be the value of when pressure is

(A) 0.2(B) 0.4(C) 0.6(D) 0.8

8.Mixture of containing 0.02mole of and 0.02mol of was dissolved in water to get 2L of solution of

1L of X + Excess of Y mol of ppt

1L of X + Excess of Z mol of pptNumber of moles of Y and Z are(A) 0.01,0.01(B) 0.02,0.01(C) 0.01,0.02(D) 0.02,0.02

1.A mixture containing 100 g and 100 g is ignited so that water is formed according to the reaction, ; How much water will be formed? A) 113 gB) 50 gC) 25 gD) 200 g

2.A partially dried clay mineral contains 8% water. The original sample contained 12% water and 45% silica. The % of silica in the partially dried sample is nearly:A) 50%B) 49%C) 55%D) 47%

3.The reaction is balanced if:A) X = 5, Y = 2B) X = 2, Y = 5C) X = 4, Y = 10D) X = 5, Y = 5

4.The number of electrons lost or gained during the change, , is:A) 2B) 4C) 6D) 8

45. Hexamethylene diamine, a compound used in making nylon-66 has 24.14% nitrogen. There are two nitrogen atoms per molecule. What is the molecular weight of hexamethylenediamine ?A) 36B) 116C) 292D) 146

46. Li3+ and a proton are accelerated by the same potential, their de-Broglie wavelengths have the ratio (mass of Li 7 & mass of proton 1) A) 1:2B) 1 : 4 C) 1 : 1D) 1: 747. If an electron is travelling at 200 m/s within 1 m/s uncertainty, what is the theoretical uncertainty in its position in m (micrometer)?A) 14.5 mB) 29 mC) 58 mD) 114 m48. What percentage of oxygen is present in the compound CaCO3.3Ca3(PO4)2 ? A) 23.3%B) 45.36% C) 41.94%D) 17.08%49. Suppose two elements X and Y combine to form two compounds XY2 and X2Y3 when 0.05 mole of XY2 weighs 5 g while 3.011 x 1023 molecules of X2Y3 weighs 85 g. The atomic masses of X and Y are respectively :A) 20, 30B) 30, 40 C) 40,30D) 80, 6050. An excited state of H-atom emits a photon of wavelength of and return to ground state, the principal quantum no. of excited state is given by:A) R(R-1)B) R/(R - 1) C) (R-1) D) (R-1)/ R51. It is known that atom contain protons, neutrons and electrons. If the mass of neutron is assumed to half of its original value whereas that of proton is assumed to be twice of its original value then the atomic mass of 6C14 will be : A) sameB) 14.28% lessC) 14.28% more D) 28.56% less52. What is the degeneracy of the level of the hydrogen atom that has the energy -RH hc /9. A) 1B) 4 C) 9D) 16 53. 44g of a sample on complete combustion gives 88 gm CO2 and 36 gm of H2O. The molecular formula of the compound may be:A) C4H6B) C2H6OC) C2H4OD) C3H6O 54.Statement 1 : When 40 g CH3CHO is allowed to react with 10 g of O2 amount of product obtained is governed by mass of O2 Statement -2 : O2 is more reactive

55.Statement 1 : De-Broglie principle can be used to calculate wavelength associated with a moving carStatement 2 : De-Broglie relation is applicable only for submicroscopic bodies

56.Statement 1 : One mole of SO2 contains double the number of molecules present in one mole of O2.Statement - 2 : Molecular weight of SO2 is double that of O2.57.Statement 1 : One of the applications of quantum theory is quantization of energy of orbits in an atom

Statement 2 : Energy of nth orbit of an atom is given by 32.Statement I : - 2p orbitals do not have any spherical nodeStatement II : - The number of spherical nodes in p orbitals is given (n - 2) where n' is principal quntum number 33.Statement I : - Each electron in an atom has two spin quantum numbers.Statement II : -Spin quntum number is not obtained by solving Schrodinger wave equation

34.Statement I : -The 19th electron in K atom enters into 4s orbital and not into 3d - orbitalStatement II : - (n+l) rule is followed for determining the orbital of the lowest energy state.

35.Statement I : - s orbital cannot accommodate more than two electrons.Statement II : - Spin exchange can take place among two electrons occupying an orbital.

2.In 0.1 M aq. H2S solution Kb for is 109 . If [S2] in this solution is 1010, then the dissociation constant for will be (approximately)(A) 1015(B) 1013(C) 1019(D) 10188.n containers having volumes v, 2v, 3v..nv containing gaseous moles n, 4n, 9n,..n3 respectively are connected with stopcock at same temperature. If pressure of first container is P, then the final pressure when all the stopcocks are opened is

(A) (B)

(C) (D)

23.The orbital angular momentum for s-electron is

a) b) c) d) zero

24.The number of electrons with the azimuthal quantum number and in ground state of is respectivelya) 16 and 5b) 12 and 5c) 16 and 4d) 12 and 425.The number of radial nodes of 3s and 2p orbitals are respectively a) 2, 0b) 0, 2c) 1, 2d) 2, 126.Which of the following sets of quantum numbers represent the highest energy of an atom?

a) b)

c) d) 27.Which of the following ion is paramagnetic?

a) b) c) d)

28.If the probability density of 1s orbital is given by and its radial probability by . then

a) r =b) c) d) r =

29.If the nitrogen atom had electronic configuration , it would have energy lower than that of normal ground state configuration because the electrons would be closer to nucleus yet is not observed because it violatesa) Heisenbergs uncertainty principleb) Hunds rulec) Pauli exclusion principle d) Bohr postulate of stationary orbits 30.The maximum number of electrons in an orbital having same spin quantum number will be

a) b) c) d)

31. hasa) 1 radial node and 1 angular nodeb) 2 radial node and 1 angular nodec) 1 radial node and 2 angular noded) 2 radial node and 2 angular node

23.The angle made by angular momentum vector of an electron with z-axis is given as

a) b) c) d) 24.Which of the following orbitals has zero probability of finding the electron in yz plane around the nucleus

a) b) c) d)

25.An ion has the magnetic moment equal to 4.9 BM. What is the value of x a) 3b) 4c) 2d) 5

26.Which has the same number of s-electrons as the d-electrons in ?

a) b) c) Nd) P27.Which of the following graphs corresponds to one node ?

a)

b)

c)

d)

28.The orbital angular momentum of 4f electron is

a) b) c) d)

29. x.y.z values in balanced equation are a) 2,3,8b) 1,3,8c)1,3,4d) 3,1,830.If the weights of N2 & O2 are equal then the ratio of number of atoms in N2 & O2 is a) 1 : 1b) 7 : 8c) 8 : 7d) 2 : 3

31.Heating 10 gr of a mixture of and below 500C gives CO2 the volume of which when reduced to STP is 448 ml. The weight percent of in the mixture isa) 8b) 20c) 80d) 4032.Statement 1 : Bohrs theory is not applicable to ionized hydrogen atom

Statement 2 : is devoid of electron33.Statement 1 : Half filled and fully filled state degenerate orbitals are more stable.Statement 2 : Extra stability is due to the symmetrical distribution of electrons and exchange energy. 34.Statement 1 : d-orbitals are five fold degenerate orbitals. Statement - 2 : A d-orbital can accommodate a maximum number of ten electrons.

35.Statement 1 : Limiting line in the Lyman series has a wave length of .Statement 2 : Wave length of Lyman limiting line is calculated for a jump of electron from

n = to

1.5 g sample contain only and . This sample is dissolved in distilled water and the volume made up to 250 ml. 25 ml of this solution neutralises 20 ml of 0.1 M . The % of in the sample is a) 42.4b) 57.6c) 36.2d) 63.8

2.1 mole of equimolar mixture of ferric oxalate and ferrous oxalate will require a mole of in acidic medium for complete oxidation, a is a) 3.6 moleb) 1.8 mole c) 0.9 mole d) 0.5 mole

3.100ml of a 0.2 M NaOH is exactly neutralised by

a) 100ml of 0.1 M HCl + 100 ml of 0.1 M

b) 100 ml of 0.1 M HCl + 50 ml of 0.1 M

c) 50 ml of 0.1 m HCl + 500 ml of 0.1 M

d) 50 ml of 0.1 M HCl + 100 ml of 0.1 M

4.10 ml of decolourises 15 ml of iodine solution when starch is used as an indicator. The amount in grams of present in the given solutions is a) 0.186b) 2.34c) 8.02d) 3.27 5.7.35 g of a dibasic acid was dissolved in water and diluted to 250 ml. 25 ml of this solution was neutralised by 15 ml of N NaOH solution . The molecular weight of this aid is a) 49b) 31c) 62d) 98

6.The volume of water to be added to 100 of 0.5 to get decinormal concentration

a) b) c) d)

7.Equal volumes of 0.1 M and 0.2 M NaCl are mixed. The concentration of ions in the mixture will be a) 0.1 Mb) 0.05 M c) 0.2 Md) 0.13 M8.320 mg of a sample of magnesium having a coating of its oxide required 20 ml of 0.1 M hydrochloric acid for the removal of the coating. The composition of the sample is a) 5.32% Mg and 68% MgOb) 68% Mg and 32% MgO c) 87.5% Mg and 12.5 % MgO d) 12.5 Mg and 87.5% MgO3.Which is a possible set of quantum numbers for a valence electron in ground state atom of phosphrous (Z = 15)?

n m s n m sA) 2 1 0 +1/2B) 3 0 0 0C) 3 1 +1 +1/2D) 3 2 0 -1/24.If aufbau rule is not used, 19th electron in Sc(Z = 21) will have

A) n = 3 B) n = 3 C) n = 3 D) n = 4 57Statement I : - Eudiometry helps in predicting the empirical / molecular formula Statement II: - In eudiometry, turpentine is used to absorb ozone 58Statement I : - On combustion of hydrocarbon, CO2 and water are formed and the liberated gas can be absorbed by baryta water (Ba(OH)2) Statement II: - Baryta water has high affinity towards carbondioxide and absorbs it

23.A small bubble rises from the bottom of a lake, where the temperature and pressure are and 6.0atm, to the waters surface, where the temperature is and pressure is 1.0atm. Calculate the final volume of the bubble if its initial volume was 2mL.A) 14mLB) 12.72mLC) 11.21mLD) 15mL

24.A certain amount of gas at and a pressure of 0.80atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 2.0atm. How high can you raise the temperature of the gas without bursting the vessel?

A) B) C) D)

25.Dry ice is solid carbon dioxide. A 0.050g sample of dry ice is placed in an evacuated 4.6L vessel at . Calculate the pressure inside the vessel after all the dry ice has been converted to gas.

A) 6.14atmB) 0.614atmC) 0.0614atmD)

26.A mixture of helium and neon gases is collected over water at and 745 mm of Hg. If the partial pressure of helium is 368 mm of Hg, what is the partial pressure of neon? (Vapour pressure of water at = 28.3 mm of Hg)A) 348.7 mm HgB) 377 mm HgC) 384.7 mm HgD) 322.7 mm Hg

27.Nitrogen forms several gaseous oxides. One of them has a density of 1.33 g/L measured at 764 mm of Hg and . The molecular formula of the oxide is.

A) B) C) D)

28.Calculate relative rate of effusion of to through a container containing and in mass ratio

A) B) C) D)

29.4gm of sulphur dioxide gas diffuses from a container in 8min. Mass of helium gas diffusing from the same container over the same time interval isA) 0.5gmB) 1gmC) 2gmD) 4gm

30.Two glass bulbs A and B at same temperature are connected by a very small tube having a stop-cock. Bulb A has a volume of and contained the gas while bulb B was empty. On opening the stop-cock, the pressure fell down to 20%. The volume of the bulb B is

A) B) C) D)

31.Pressure of 1g ideal gas X at 300K is 2atm. When 2g of another gas Y is introduced in the same vessel at same temperature, the pressure become 3atm then correct relationship between molar mass of X and Y is

A) B) C) D) 32.Statement 1: A lighter gas diffuses more rapidly than a heavier gas under the same conditions of temperature and pressure.Statement 2: At a given temperature, the rate of diffusion of a gas is inversely proportional to the density.

33.Statement 1: The pressure of a fixed amount of an ideal gas is proportional to its absolute temperature at constant volume.Statement 2: The product of pressure and volume of a given mass of gas is constant at constant temperature.

34. Statement 1: When temperature of an ideal gas increases from to at constant P, its volume increases by 100L.

Statement 2: at constant P.

35.Statement 1: Daltons law is applicable for the non reacting gases only.

Statement 2: A gaseous mixture containing and does not follow the Daltons law

1.The ratio between the root mean square speed of H2 at 50K and root mean square speed of O2 at 800K is A) 1:2B) 1:1C) 2:1D) 8:1

2.A real gas is supposed to obey the gas equation P(V-b) = RT at STP. If one mole of a gas occupies 25dm3 volume at STP, then its compressibility factor is (b = 2.586 lit mole-1)A) 1.115B) 0.115C) 0.784D) 0.885

3.One mole of N2 gas at 0.8atm. takes 38sec to diffuse through a pinhole, where as one mole of an unknown gas at 1.6atm. takes 57sec to diffuse through the same pinhole. The molecular weight of unknown gas is A) 126B) 64C) 80D) 252

4.4g of argon (M.W = 40) in bulb at temperature of T K had a pressure P atm. When the bulb was placed in a hotter bath at temperature 500 more, 0.8g of gas had to be removed to get original pressure. The value of T is A) 100KB) 400KC) 200KD) 250K

1.At low pressure, vander Waals equation is written on . The compressibility factor is then equal to

A) B) C) D)

2.The gas which can most easily be liquefied is (In brackets the value of vander Waals constant a was given )

A) (= 1.360 atm. mole-2)

B) (= 1.390 atm. mole-2)

C) (= 2.253 atm. mole-2)

D) (= 4.170 atm. mole-2)3)The temperature at which the most probable velocity of oxygen is equal to the RMS velocity of ozone at 500C is A) 323KB) 484.5KC) 215.3KD) 646K

4)The temperature at which the RMS velocity of is half the RMS velocity of He at 300KA) 300KB) 150KC) 600KD) 1200K

5) molecule is twice as heavy as molecule. Hence at the ratio of the average kinetic energy of and is A) 2:1B) 1:2C) 1:1D) 4:1

6)For two gases , A and B with molecular weights and , it is observed that at a temperature T, the average velocity of A is equal to the root mean square velocity of B. Thus the average velocity of A can be made equal to the average velocity of B, if A) TA is lowered and TB is raisedB) TA is made equal to 0.85 times of TB C) Both TA and TB are raised to a higher temperature.D) Both TA and TB are placed at a lower temperature (where TA and TB are temperatures of gases A and B)7)The compressibility factor of a gas is more than unity at STP, then

A) B) C) D)

8)The vander waals constant b for helium is . The diameter of helium atom is

A) B) C) D)

45.An aqueous solution contains 10% ammonia by mass and has density of 0.99 g/cc. Calculate hydrogen ion concentration in solution

(A) (B)

(C) (D) 46.Conjugate base of [Fe(H2O)6]2+ is(A) [Fe(H2O)6]3+(B) [Fe(H2O)5(OH)]+(C) [Fe(H2O)5(OH)]3+(D) [Fe(H2O)5H]3+

47.For the reaction the equilibrium constant at 25C is . If a solution is 0.1 M in KCN and 0.03 M in AgNO3 originally at equilibrium, the concentration of Ag+ is

(A)(B)

(C)(D)

48.In the solution is (A) Lewis acid(B) Lewis base(C) Neutral salt(D) Basic salt

49.2NO Br (g) 2NO (g) + Br2 (g). If nitrosyl bromide is 34% dissociated at 25C and a total pressure of 0.25 atm, Kp for the dissociation at this temperature is

(A) (B)

(C) (D)

50.An equilibrium can be represented by following equation

P (aq) + Q (aq) 2 R (aq) + S (aq)In a certain mixture, the equilibrium concentration of Q is 10 mole per litre. What will be equilibrium concentration of Q if 5 moles of pure Q is dissolved in mixture ?(A) 15 mole/dm3(B) between 10 mole/dm3 and 15 mole/dm3(C) 10 mole/dm3(D) between 5 mole/dm3 and 10 mole/dm3

51.For a hypothetical reaction; A (g) + B (g) C (g) + D (g), a graph between log K and T-1 is straight line as follows, when 0.5 and OA = 10, assuming is independent of temperature. The equilibrium constant at 298 K and 798 K are respectively

(A) K1 = 9.96 109; K2 = 2.76 1010(B) K1 = 3.79 108; K2 = 9.98 109(C) K1 = 7.96 108; K2 = 7.96 109(D) K1 = 9.96 109; K2 = 9.96 109

52.H3PO3 is a dibasic weak acid if its initial concentration is 0.3 M and degree of dissociation is 0.3%. Find pH at this point and Ka is (consider )

(A)(B)

(C) (D)

53.

Correct statements related to given graph is / are(A)At moderate pressures inter molecular repulsive forces are dominant than attractive forces for CO2(B)Only at high pressure repulsive forces are dominant than attractive forces for H2(C)At low pressure attractive forces are dominant over repulsive forces for CH4(D)All of these

54.STATEMENT 1: A substance that can either act as an acid or a base is called ampholyte.

STATEMENT 2: Bisulphide ion and bicarbonate ion are ampholytes.

55.STATEMENT 1: It is difficult to distinguish the strength of the strong acids such as HCl, H2SO4, HNO3, HBr in dilute aqueous solutions.STATEMENT 2: In dilute aqueous solution all strong acids donate a proton to water and are essentially 100% ionised to produce a solution containing H3O+ ions plus the anions of strong acid.

56.STATEMENT 1: For the equilibrium N2O4 (g) 2NO2 (g) the mean molar mass of the equilibrium mixture is always more than 46 and less than 92.STATEMENT 2: Addition of xenon at constant volume to the equilibrium mixture will result in decrease in mean molar mass of mixture.

57.STATEMENT 1: Ice melts at 0C under normal conditions, it would melt at lower temperature under higher pressure.STATEMENT 2: Formation of ice is an exothermic process.1.Solubility of a substance which dissolves with decrease in volume and absorption of heat will be increased by (a) Low temperature and high pressure (b) Low temperature and low pressure (c) High temperature and low pressure (d) High temperature and high pressure2.A nitrogen-hydrogen mixture initially in the molar ratio of 1:3 reached equilibrium to form ammonia when 25% of the material had reacted. If the total pressure of the system was 21 atm, the partial pressure of ammonia at the equilibrium was (a) 4.5 atm(b) 3.0 atm(c) 2.0 atm (d) 1.5 atm

3.In a system A(s) 2B(g) +3C(g). if the concentration of C at equilibrium is increased by a factor of 2, it will cause the equilibrium concentration of B to change to (a) Two times the original value(b) One half of its original value

(c) times its original value(d) times

4.Ice(s) Water (), =+ve. The melting of ice is favoured by (a) Low T and Low P(b) High T and High P (c) Low T and High P(d) Low P and High T

5.For the reaction: the degree of dissociation of HI(g) is related to equilibrium constant by the expression.

(a)(b) (c) (d)

6.For , If , equilibrium pressure of mixture is: (a) 8 atm(b) 16 atm(c) 64 atm(d) 4 atm

7.When chemical equilibrium is attained:

(a) G=0 and (Q) attains the maximum value

(b) and Q=K (where K is equilibrium constant)

(c) G=0 and Q assumes minimum values

(d)= - RT in K

8.One mole of at 300 K is kept in a closed container under one atmosphere. It is heated

to 600K when 20% by mass of decomposes to . The resultant pressure is (a) 1.2 atm(b) 2.4 atm (c) 2.0 atm(d) 1.0 atm 1.For a fixed mass of a gas and at a given temperature, which of the following graphs is not consistent with the Boyles law.

A) B) (C) (D)

2.Two flasks X and Y of volumes 250ml and 300ml respectively at the same temperature are connected by a stop cock of negligible volume. The flask X contains nitrogen gas at a pressure of 660 torr and the flask Y contains neon gas at a pressure of 825torr. If the stop cock is opened to allow the two gases to mix, the partial pressure of neon gas and total pressure of the system will be (A) 300 torr,700torr (B) 400 torr,700torr(C) 450 torr,750torr (D) 300 torr,750torr

3.At temperature for the reaction of with excess of hot graphite to form CO is 9atm. The mole% of CO in the equilibrium mixture of gases is(A)14.3%(B)25%(C)75%(D) 85.7%

4.A gas obeys the equation of state P(V-b)=RT(The parameter b is a constant). The slop for an isochore will be: (A) Negative(B) Zero(C) R/(V-b) (D) R/P47.What will be the pH of a solution formed by mixing 40 cm3 of 0.1 M HCl with 10 cm3 of 0.45 M NaOH ? a) 10b) 8c) 5d) 12

48.2.5 mL of 2/5 M weak monoacidic base is titrated with 2/15 M HCl in water at 25C. The concentration of H+ ion at equivalence point is

a) b) c) d)

49.The compound whose 0.1 M solution is basic is a) ammonium acetateb) ammonium chloridec) ammonium sulphated) sodium acetate50.Which of the following solutions will have pH close to 1.0 ?a) 100 ml of (M/10) HCl + 100 ml of (M/10) NaOHb) 55 ml of (M/10) HCl + 45 ml of (M/10) NaOHc) 10 ml of (M/10) HCl + 90 ml of (M/10) NaOHd) 75 ml of (M/10) HCl + 2.5 ml of (M/10) NaOH

51.Hydrolysis constant of two salts KA and KB of weak acids HA and HB are 10-8 and 10-6. If the dissociation constant of third acid HC is 10-2. The order of acidic strengths of three acids will bea) HA >HB > HC b) HB > HA > HCc) HC > HA > HBd) HA = HB = HC

52.The pH of 10-10 M H2SO4 will be almost a) 6b) 7c) 6d) 0

57.STATEMENT1: When CH3 COONa is dissolved in water, the hydrolysis of ion takes place.STATEMENT 2:.The ion which is derived (in the salt) from weak acid, undergoes hydrolysis.58.STATEMENT 1 : H3BO3 is protic acid.STATEMENT 2: Borax is salt of H3BO3 and NaOH, its aqueous solution is alkaline in nature.

59.STATEMENT 1: Benzoic acid is weaker acid than acetic acid STATEMENT 2: Greater is the value of Ka, more is the acidic character.60.STATEMENT 1: Sodium chloride (NaCl) does not undergo hydrolysisSTATEMENT 2: Salts of strong acids and bases are not hydrolysed.

1.Calculate the pH of solution made by mixing 50ml of 0.2M & 75 ml of 0.1 M a) 4.2629b) 9.7324c) 8.3 d) 4.74

2.The equilibrium constant for reaction What is

a) b) c) d)

3.2.5 ml of M weak mono acidic base is titrated with M HCl in water at . The concentration of ion at equivalence point is

a) b) c) d)

4.The in 0.2M solution of .To this solution format is added so as to adjust the conc. of to one mole per liter. What will be the PH of solution a) 10.8b) 4.19c) 6.25 d) 7

1.Calcium lactate is a salt of weak acid i.e. lactic acid having general formula. Aqueous solution of salt has 0.3M concentration. POH of solution is 5.60. If 90% of the salt is dissociated them what will be the value of Pka?

(A) (B) (C) (D) none of these

2. Amount of in an antacid tablet is to be determined by dissolving the tablet in water and titrating the resulting solution with HCl. Which indicator is most suitable in this titration? AcidKa

(A) Methyl orange (B) Bromothymol blue

(C) Phenolphthalein (D) Alizarin yellow

3.0.2g sample of benzoic acid is titrated with 0.12M solution. What volume of solution is required to reach equivalence point? (Molar mass of benzoic acid = 122)(A)6.82 ml(B) 13.6 ml(C) 17.6 ml (D) 35.2 ml

4.Ka for formic acid and acetic acids are respectively. The relative strength of acids having same concentration is (A) 2 : 1(B) 2:3:1 (C) 1:2:1(D) 4.36:1

47.A solution is a mixture of 0.05 M KCl and 0.05 M Nal. The concentration of in the solution when just starts to precipitate is equal to :

A) B) C) D)

48.To separate and identify the ions in a mixture that may contain and use the reagents , and . They should be added in the order :

A) B) C) D)

49.Slaked lime, is used extensively in sewage treatment. What is the maximum pH that can be established in A) 1.66B) 12.35C) 7.0D) 14.050.One litre of N/2 HCl solution was heated in a beaker. When volume was reduced to 600 mL, 3.25g of HCl was given out. The new normality of solution is :A) 6.85B) 0.685C) 0.1043D) 6.50

51. The density of liquid (mol. wt. = 70) is 1.2 g . If 2 mL of liquid contains 35 drops, the number of molecules of liquid in one drop are :

A) B) C) D) 52. 3 g of an oxide of a metal is converted completely to 5g chloride. Equivalent weight of metal isA) 33.25B) 3.325 C) 12D) 20

57.STATEMENT -1: In acidic medium is not precipitated by .

STATEMENT 2: Common ion effect reduces the concentration of to a minimum level

58.STATEMENT -1: Salting out action of sodium soap in presence of NaCl is based on common ion effect

STATEMENT -2:Salting out action of soap is based on the fact that as the concentration of increases, the RCOONa shows precipitation because

59.STATEMENT -1: One equivalent of has 1 equivalent of K, Cr and O each.STATEMENT -2: Equivalent and milli equivalent reacts in equal number to give same eq. or meq of product.60.STATEMENT -1: On increasing the temperature the milli-moles of solute, milli- equivalent of solute, molality, mole fraction of solute and % by weight does not change.STATEMENT -2: Each of these involves only weights of solute and solvent.

1.Aspirin , at body temperature, 370C, Ka is . If two aspirin tablets, each having a mass of 325mg are dissolved in a full stomach whose volume is 1L & whose pH is 2, what percent of a aspirin is in the form of molecules? (a) 5% (b) 95.9%(c) 99.7%(d) 99.2%

2. If are the solubilites of AgCl in , 0.01M , in 0.01M NaCl & in 0.05M respectively at certain temperature, the correct order of sdubilities is

(a) (b)(c) (d)

3. The maximum pH at which the 0.1M solution does not precipitates is equal to ( of = )(a) 11(b) 1.96(c) 9.04(d) 10.04 4.A weak acid HA after treatment with 12ml of 0.1M strong base has a pH of 5. At the end point the volume of same base required is 26.6 ml. The Ka of acid is

(a) (b) (c) (d)

5.Two buffers of pH 4.0 & 6.0 respectively are prepared from adding weak acid HA & its salt NaA. Both the buffers are 0.5M in HA. What would be the pH of the solution obtained by mixing equal volumes of two buffers? ( KHA=)(a) 5.0(b) 6.30(c) 5.70(d) 4.30

6.What is the pH of saturated solution of ? (a) 6.1(b) 7.3 (c) 8.42(d) 7.90

7.What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01M ZnCl2 and saturated with 1.0M H2S? (Given: KSp)(a) 0 (b) 1(c) 2 (d) 4

8.An acidbase indicator has KH In .The acid form of the indicator is red & the basic form is blue. The change inrequired to change the indicator form 75% red to 75% blue is

(a) (b) (c) (d) In determination of molecular weight with the help of depression in freezing point, in which of the following aq solutions, abnormal mol. mass will deviate most from its original mol, mass value (assume 100% dissociation in all cases)(A)0.1 m-NaCl(B)0.05 mKI(C)0.75m-MgSO4(D)0.1 m - NH4Clwhere h is degree of hydrolysisLiquid A can give binary ideal solution S1 and S2 with liquid B and liquid C separately. Molecules of liq. B and liq. C can combine to give another gaseous product BC in vapour phase only. They do not react in liquid phase.Now S1 and S2 are mixed. In vapour phase before combination of B and C, partial pressure of A is P. After combination ________.(A)P will remain same, because A is not taking part in combination(B)P will decrease, because total number of moles in vapour phase will decreases(C)P will increase because total number of moles in vapour phase will decrease(D)P will remain same, because number of moles in vapour phase will not change.Activities of components forming ideal solutions are equal to their respective(A)number of moles(B)molar concentrations(C)partial pressure(D)mole fractionsA liquid mixture is composed of 1 mole of benzene and 1 mole of toluene. If pressure over the mixture is reduced, at what pressure does the first vapour form ?

( and )(A)67 mm(B)134 mm(C)760 mm(D)process does not depend on pressure

Two solutions (both 5% by wt) of non-volatile solutes A and B are prepared. Molar mass ratio MA : MB = 1 : 3. If these solutions are mixed to prepare two new solutions S1 and S2, the mixing ratio being 2 : 3 and 3 : 2 by volume for S1 and S2 respectively, then ratio will be(A)7/9(B)7/11(C)5/7(D)9/11A volatile solute AB is dissolved in water, in which mole fraction of water is 5/6. If 50% of molecules of AB get dissociated into A and B and remaining 50% get dimerised into (AB)2. Then relative lowering in vapour pressure will(A)increase by 20%(B)increase by 25%(C)remain same because mass of solute is unchanged(D)remain same because no of solute particles will not changeFor an ideal solution, Rault's Law is obeyed exactly at (A)fixed concentrations and at fixed temperature(B)all concentrations and at all temperature(C)all concentrations at fixed temperature(D)fixed concentrations and at all temperature

A binary solution is prepared with 1 mole of liquid A() and 1 mole of liq. . If pressure over the mixture is reduced, then the pressure at which last trace of liquid will disappear, will be (A)75 mm(B)66.67 mm(C)150 mm(D)133.33 mmAvailable solutions are 1L of 0.1 M NaCl and 2L of 0.2 M CaCl2. Using only these two solutions what maximum volume of a solution can be prepared having [Cl] = 0.34 M exactly. Both electrolytes are strong(A)2.5 L(B)2.4 L(C)2.3 L(D)2.8 L

Consider equimolal aqueous solutions of NaHSO4 and NaCl with Tb and Tb as their respective boiling point elevations. The value of , will be (A)1(B)1.5(C)3.5(D)2/3A solute 'S' undergoes a reversible trimerization when dissolved a certain solvent. The boiling point elevation of its 0.1 molal solution was found to be identical to the boiling point elevation in case of a 0.08 molal solution in the same solvent of a solute which neither undergoes association nor dissociation. To what percent had the solute 'S' undergone trimerization ?(A)30%(B)40%(C)50%(D)60%vRatio between boiling point elevations of aq. solutions of 0.1 M-NaA and 0.1 M-NaCl 100% dissociation in both cases) is 21/20. NaA is a salt of weak acid HA. Then dissociation constant of weak acid HA will be (A)1.1 10-12(B)8.1 10-13(C)10-11(D)9 10-12

1) A sample of liquid H2O of mass 18.0 g is injected into an evacuated 7.6L flask maintained at 27.00C. If vapour pressure of H2O at 270C is 24.63 mm Hg. What weight percentage of the water will be vapourised when the system comes to equilibrium? Assume water vapour behaves as an ideal gas. The volume occupied by the liquid water is negligible compared to the volume of the container:

A)1%B)10%C)18%D)20%

2) At 880C benzene has a vapour pressure of 900 torr and toluene has a vapour pressure of 360 torr. What is the mole fraction of benzene in the mixture with toluene that will boil at 880C at 1 atm pressure, benzene toluene form an ideal solution?

A)0.416B)0.588C)0.688D)0.740

3) If P0 and PS are the vapour pressures of the solvent and solution respectively, n1 and n2 are the mole fractions of the solvent and solute respectively, then

A)B)C)D)

4) The vapour pressure of water depends upon

A)Surface area of containerB)Volume of container

C)Temperature D)All of the above

45.Two volatile liquids A and B form an ideal binary solution and variation of vapour pressure versus mole fraction is described in the following diagram. Which of the following statements regarding A, B and the solution of A and B is incorrect?

A) Vapour pressure of A in pure state is greater than that of B in pure state at same temperature.B) Vapour pressure of solution at P is 480 mm of Hg.C) Mole fraction of B at P is 0.60.D) At point P, the mole fraction of A in the vapour phase, which is in equilibrium with the solution, is 0.60.

46.Consider two liquids A and B having pure vapour pressure and forming an ideal solution. The plot of ( when and are the mole fraction of A in liquid and vapour phase respectively) is linear with slope and intercepts respectively

A) and B) and

C) and D) and 47.Identify the false statement.A) the volume of solution cant be less than the sum of volumes of the pure solvent and solute used to prepare the solution (binary solution of two liquids).

B) At constant T and P, will be necessarily negative for the ideal solution

C) An ideal binary solution cant form an azeotropic mixture.D) In binary solutions ideality is more of an exception rather than a rule.

48.Equal weights of two non-volatile non-electrolytic solids 1 and 2 were dissolved in two different vessels A and B respectively, each containing 100 mL water, The vessels were maintained at constant temperature as shown in the following figure. At equilibrium, vessels A and B were found to contain 80 mL and 120 mL of water respectively. Which of the following is true?

A) The weight of solute in vessel A is greater than the weight of solute in the vessel BB) The weight of solute in vessel A is lesser than the weight of solute in the vessel BC) Molecular weight of 1 > molecular weight of 2D) Molecular weight of 1 < molecular weight of 2

49. The equilibrium constant for the reaction represented by the equation above is greater than 1.0. Which of the following gives the correct relative strengths of the acids and bases in the reaction? AcidsBases

A)

B)

C)

D)

50.In beaker A, an ice cube of pure is to be placed in pure liquid . In beaker B, an

ice cube of pure is to be placed in pure liquid . Which of the following is the correct statement?A) Ice cube will sink in both the beakers A and BB) Ice cube will float in both the beakers A and BC) Ice cube will sink in beaker A but float over in BD) Ice cube will sink in beaker B but float over in A

51.The correct order of bond angles is :

A) B)

C) D)

52.Nodal planes of -bond(s) in are located in :A) all are in molecular plane

B) two in molecular plane and one in a plane perpendicular to molecular plane which contains -bondC) one in molecular plane and two in plane perpendicular to molecular plane which

contains -bondsD) two in molecular plane and one in a plane perpendicular to molecular plane which

bisects -bonds at right angle

53.Among the following, the molecule with 2nd highest dipole moment is:

A) B) C) D)

54.Assertion : Adding a non-volatile solute to a volatile solvent increases the boiling point.Reason : Addition of non-volatile solute results in lowering of vapour pressure.55.Assertion : When dry air is passed continuously through an aqueous solution of a non-volatile solute, vapour pressure of solution decreases gradually.Reason : Some air is absorbed in the solution.

56.Assertion : Connecting a flask at vacuum to another flask containing solid (s)

in equilibrium with its dissociation products (g) and HCl (g)

decreases the amount of solid . Both the flasks are at same temperature.

Reason: for the decomposition process decreases in the above process.

57.Assertion: In , the axial P Cl bonds are stronger than the equatorial PCl bonds.Reason:Axial PCl bonds have greater d-character.1) Which curve does not represent Boyles law ?

A)B)

C)D)

6) The apparatus shown consists of three bulbs connected by stopcocks of negligible volume. The temperature is constant.

PA = 2.13 atm PB = 0.861 atm PC = 1.15 atm VA = 1.50 L VB = 1.0 L VC = 2.0 L When all the stopcocks are opened, the pressure in the bulb B will be

A)1.41atmB)0.861 atmC)1.38 atmD)1.18 atm

7) Which of the assumption of the kinetic molecular theory best explains. Dalton's law of partial pressure?

A)Gas molecules move at random with no attractive force between them

B)the velocity of gas molecules is proportional to the absolute temperature

C)the amount of space, occupied by a gas is much greater than the space, occupied by the actual gas molecules.

D)collisions with the wall of the container or with other molecules are elastic.

8) The ratio between the root mean square speed of H2 at 50 K and that of O2 at 800 K is,

A)4B)2C)1D)

1) A 40ml solutions of weak base is titrated with 0.1N solution. The of the solution is found to be 10.04 and 9.14 after the addition of 5ml and 20ml of the acid respectively. The dissociation constant of the base will be.

A)B)C)D)

1) X mL of H2 gas effuses through a pinhole in a container in 5 seconds. The time taken for the effusion of the same volume of the gas specified below under indentical condition is

A)10 seconds : HeB)20 seconds : O2

C)25 seconds : COD)55 seconds : CO2

2) A gaseous mixture contains 56 g of N2, 44 g CO2 and 16 g of CH4.The total pressure of mixture is 720 mm Hg. The partial pressure of CH4 is :

A)180 mmB)360 mmC)540 mmD)720 mm

3) The circulation of blood in human body supplies O2 and releases CO2. The concentration of O2 and CO2 is variable but on the average, 100 mL blood contains 0.02 g of O2 and 0.08 g of CO2. The volume of O2 and CO2 at 1 atm and at body temperature of 370C, assuming 10 litre blood in human body, would be

A)2 litre, 4 litreB)1.5 litre, 4.5 litre

C)1.59 litre, 4.627 litreD)3.82 litre, 4.62 litre

4) If the pressure of a gas contained in a closed vessel is increased by 0.4% when heated by 10C its initial temperature must be :

A)250 KB)250CC)25 KD)25C

1) Equal weights of methane and oxygen are mixed in an empty container at 250C. The fraction of the total pressure exerted by oxygen is

A)1/2B)2/3C)1/3D)

2) A gas has vapour density 11.2. The volume occupied by 1 g of the gas at N.T.P. will be

A)11.2 LB)22.4 LC)1 LD)Unpredictable

3) At a temperature TK, the pressure of 4.0g argon in a bulb is P. The bulb is now put in a bath having temperature 50K higher by T. 0.8g of argon had to be removed to maintain original pressure. The temperature T is equal to

A)510 KB)200 KC)100 KD)73 K

4) Use of hot air balloons in sports and meteorological observation is an application of

A)Boyles lawB)Charles law

C)Kelvins lawD)Ideal gas equation

5) A sealed container with a gas at 2.00 atm is heated from 20.0 K ot 40.0 K. The new pressure is:

A)0.50 atmB)1.0 atmC)4.00 atmD)2.14 atm

6) Which curve does not represent Boyles law ?

A)B)C)D)

7) Density of a gas is found to be 5.46 g/dm3 at 270 C at 2 bar pressure. What will be its density at STP?

A)6 g/lB)8 g/lC)2.75 g/lD)1.5 g/l

8) A 10 g of a gas at atmospheric pressure is cooled from 2730C to 00C keeping volume constant. Its pressure would become

A)1/2 atmB)1/273 atmC)2 atmD)273 atm

23) The vapour pressures of two pure liquids A and B, that form an ideal solution are 100 and 900 torr respectively at temperature T. This liquid solution of A and B is composed of 1 mole of A and 1 mole of B. What is the vapour pressure above the liquid mixture.

A)800 torrB)500 torrC)300 torrD)none of these

24) An industrial waste water is found to contain 8.2% Na3PO4 and 12% MgSO4 by weight in solution. If % ionization of Na3PO4 and MgSO4 are 50 and 60 respectively then its normal boiling point is

A)B)C)D)none of these

25) 0.1 M KI and 0.2 M AgNO3 are mixed in 3 : 1 volume ratio. The 0.2 depression of freezing point of the resulting solution will be

A)3.72 KB)1.86 KC)0.93 KD)0.279 K

26) If 0.1 M H2SO4 (aq.) solution shows freezing point, then what is the Ka2 for H2SO4 ? (Assume m = M and )

A)0.122B)0.0122C)D)none of these

27) The total vapour pressure of a 4 mole % solution of NH3 in water at 293 K is 50.0 torr, the vapour pressure of pure water is 17.0 torr at this temperature. Applying Henrys and Raoults laws, calculate the total vapour pressure for a 5 mole % solution.

A)58.25 torrB)33 torrC)42.1 torrD)52.25 torr

47) 10 moles of an ideal gas confined to a volume of 10 lit is released into atmosphere at 300K, Where the pressure is 1 bar. The work done by the gas is

A)249 L barB)220 L barC)259 L barD)239 L bar

48) Hf0 of Benzene and cyclohexane respectively are + 49 KJ and + 156 KJ. Calculate amount of heat involved in the hydrogenation of Benzene involving 3g of Hydrogen is

A)B)C)D)

49) of combustion of yellow P and Red P are 11KJ and 9.78 KJ respectively. The heat of transition of yellow P to red P is

A)B)C)D)

50) For the reaction,

.Bond energy of bond is 20 K.cal greater than the bond energy of bond. Bond energies of and are same in magnitude. Then H value for the reaction is

A)B)

C)D)

51) During a reversible isothermal compression of one mole of an ideal gas originally at, 0.525 atm and 43.2 lit, 975 J of heat was removed. The final pressure of gas is [Antilog (]


52) 10 moles of Ideal gas expand isothermally and reversibly from a pressure of 10 atm to 1 atm at 300K. What is the largest mass which can be lifted through a height of 100 meter.

A)31842 kgB)58.55 kgC)342.58 kgD)116.11 kg

57) Statement - I : The heat absorbed during isothermal expansion of an ideal gas against vacuum is zero.Statement - II : There will be no work against zero external pressure.

A)Statement 1 is True, Statement 2 is True; Statement 2 is a correct explanation for Statement 1.

B)Statement 1 is True, Statement 2 is True; Statement 2 is NOT a correct explanation for Statement 1.

C)Statement 1 is True, Statement 2 is False.

D)Statement 1 is False, Statement 2 is True.

58) Statement - I: The enthalpy of formation of is greater than that of .Statement-II: Enthalpy change is negative for the condensation reaction .





59) Statement - I : The internal energy of an isothermal process doesnt change.Statement - II : The internal energy of a system depends only on pressure of the system.





60) Statement - I : When 1 lit of 1 M HF aqueous solution is mixed with 1 lit of 1 M aqueous NaOH solution 68.6 KJ of heat is liberated.Statement - II : HF is a weak acid.





45) The enthalpies of combustion of Carbon and Carbon monoxide are and . The enthalpy of formation of CO(g) is

A)B)C)D)

46) A solution of 500 ml of 2M KOH is added to 500 ml of 2M HCl solution, the mixture is shaken well and the rise in temperature T1 is noted. The experiment is repeated with 250 ml of each of 0.5M solutions of KOH and HCl and rise in temperature T2 is again noted. Assume that all heat is taken by the solution. Which of the following is correct?

A)T1 = 4T2B)T1 = T2C)2T1 = T2D)4T1 = T2

47) Given

, The value of at 300K for the following reaction is

A)B)C)D)

48) Given, Then the formation constant of is

A)B)C)D)

49) , X on heating up to 10000C Y is obtained. Y on heating with excess of HF, a final product Z is obtained. The covalency of central atom in Z is

A)2B)4C)6D)5

51) The equilibrium constant Kp for the reaction is 1.64 x 10-4 atm-2 at 4000C and 0.144 x 10-4 atm-2 at 5000C. The mean heat of formation of NH3 from its elements in this temperature range [Assume is constant in this temperature range][log11.39=1.0565]

A)B)C)D)

52) An impure sample of NaCl weighing 2 grams was dissolved in water and excess of AgNO3 solution was added. The weight of precipitate formed was 0.287 grams. The percentage purity of the sample is

A)11.7%B)5.85%C)25%D)2.85%

55) Statement- I: On increasing the intensity of incident radiation the number of photoelectrons ejected increases but kinetic energy remains same.Statement-II: Higher the intensity means more the energy of radiation.





57) Statement - I : Phenolphthalein does not give pink colour with NaHCO3 aqueous solution.Statement - II : Aqueous solution of NaHCO3 is basic in nature.





1) is a stable isotope. 13Al29 is expected to disintegrate by

A)-emissionB)-emission

C)positron emissionD)proton emission

2) 23Na is the more stable isotope of Na. Find out the process by which can undergo radioactive decay

A)- emissionB)-emission

C)positron emissionD)proton emission

3) 84Po210 decays by particle emission to 82Pb206 with a half life of 138.4 days. If 1.0 g of 84Po210 is placed in a sealed tube, how much helium will accumulate in 69.2 days. Express the answer in cm3 at STP.

A)25.21B)42.32C)37.25D)31.25

4) During a negative -decay

A)An atomic orbital electron is ejected

B)An electron which is already present within the nucleus is ejected

C)A neutron in the nucleus decays emitting an electron

D)A part of the binding energy of the nucleus is converted into an electron

5) Time required to deposit one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium ion is

A)30 sB)10 sC)30,000 sD)10,000 s

6) Electrolysis of a solution of ions produces . Assuming 75% current efficiency, the current that should be employed to achieve a production rate of 1 mole per hour is nearly

A)43.3 AB)71.5 AC)35.2 AD)58.3 A

7) Same quantity of electricity is being used to liberate iodine (at anode) and a metal x (at cathode). The mass of x deposited is 0.617g and the iodine is completely reduced by 46.3 cc of 0.124 M sodium thiosulphate. The equivalent mass of x is nearly

A)213.5B)108.2C)111.2D)310.6

8) A current of 9.65 A is drawn from a Daniel cell for exactly 1 hr. The loss in mass at anode and gain in mass at cathode, respectively are

A)11.43 g, 11.77 gB)11.77 g, 11.43 g

C)22.86 g, 23.54 gD)23.54, 22.86 g

1) The freezing point of a solution of 0.1965 mole of KCN in 1 kg of water is (Tf)1 after adding to the solution, 0.095 mole of Hg(CN)2, the freezing point is (Tf)2. Complex formation occurs according to the equation Hg(CN)2(s) + mC(in solution) [Hg(CN)m + 2]m-. If the ratio , Calculate the value of m.

A)4B)3C)1D)2

3) A direct current of 1.25A was passed through 200 ml of 0.25M Fe2(SO4)3 solution for a period of 1.1 hour. The resulting solution in cathod chamber was analysed by titrating against acidic solution of 25 ml KMnO4 was required to reach the end point. What is the molarity of KMnO4 solution

A)41 MB)4.1 MC)0.41 MD)2.0 M

8) Using van der Waals equation, calculate the constant a , when two mole of a gas confined in a 4L flask exerts a pressure of 11.0 atmospheres at a temperature of 300 K. The value of b is 0.05 L

A)B)

C)D)

23) In thermodynamics, a process is called reversible when :

A)Surroundings and system change into each other

B)There is no boundary between system and surroundings

C)The surroundings are always in equilibrium with the system

D)The system changes into the surroundings spontaneously.

24) The internal energy change when a system goes from state A to B is 40 KJ/mol. If the system goes from A to B by a reversible path and returns to state A by an irreversible path, the net change in internal energy is :

A)< 40 KJB)zero C)40 KJD)> 40 KJ

25) When 1mol of gas is heated at constant volume, temperature is raised from 298K to 308K.The energy supplied to the system during this process is 500J. Then which statement is correct ?

A)B)

C)D)

26) The difference between the heats of reaction at constant pressure and constant volume for the reaction at in kJ is

A)B)C)D)

27) Molar heat capacity of water in equilibrium with ice at constant pressure is

A)ZeroB)C)D)

28) One mol of an ideal gas (CV = 20 J K-1 mol-1) initially at STP is heated at constant volume to twice the initial temperature. For the process, W and q will be :

A)W = 0; q = 5.46 kJB)W = 0; q = 0

C)W = -5.46kJ ; q = 5.46 kJD)W = 5.46 kJ; q = 5.46 kJ

29) The dissociation energy of CH4 and C2H6 are respectively 360 and 620 kcal/mol. The bond energy of C - C bond is:

A)260 kcal/molB)180 kcal/molC)130 kcal/molD)80 kcal/mol

30) The enthalpy of Vaporization of water at 1000C is 40.63 KJ mol-1. The value of for this process would be

A)37.53 KJ mol-1 B)39.08 KJ mol-1

C)42.19 KJ mol-1D)43.73 KJ mol-1

31) 20 mL of 0.5 M NaOH are mixed with 100 mL of 0.1 M HCl. If x kJ heat is liberated, the enthalpy of neutralization (in kJ ) is

A)-100xB)-50xC)100xD)50x

32) Statement I : During compression between the same initial & final volume for an ideal gas work done on gas is lesser for reversible process than for irreversible process.Statement II : reversible process is more efficient than an irreversible process.

A)Statement 1 is true, statement 2 is true ; Statement 2 is the correct explanation for statement 1.

B)Statement 1 is true, Statement 2 is true ; Statement 2 is not the correct explanation for statement 1.

C)Statement 1 is true, Statement 2 is false

D)Statement 1 is false, Statement 2 is true

33) Statement I : A process is called adiabatic if the system does not exchange heat with the surroundingsStatement II : It does not involve increase or decrease in temperature of the system

A)Statement 1 is true, statement 2 is true ; Statement 2 is the correct explanation for statement 1.

B)Statement 1 is true, Statement 2 is true ; Statement 2 is not the correct explanation for statement 1.



34) Statement 1: Heat of neutralization of perchloric acid, , with is same as that of with .Statement 2: Both and are strong acids.

A)Statement 1 is true, Statement 2 is true; Statement 2 is a correct explanation for Statement 1.

B)Statement 1 is true, Statement 2 is true; Statement 2 is not a correct explanation for Statement 1.



35) Statement I: Enthalpy of combustion is always negative but enthalpy of oxidation (involving combination with oxygen) may be negative or positive. Statement II: Oxidation reaction involving combination with oxygen is always a combustion reaction.

A)If both Statement I and Statement II are true and Statement-II is the correct explanation of Statement I

B)If both Statement-I and statement II are true but statement II is not the correct explanation of statement I.

C)If statement I is true but Statement-II is false.

D)If statement I is false and Statement II is true.

1.A hydrogen electrode placed in a buffer solution of NaCN and HCN in the mole ratio of X : Y and Y : X has an oxidation electrode potential values E1 and E2 volts respectively at 25C. The pKa value of HCN is

(A) (B)

(C)(D)

2.The e.m.f. of the cell Cd (s) + Hg2+ (aq) Cd+2 (aq) + Hg is given by E = 0.6708 1.02 104 (T 25 V) where T is the temperature in C and E in volts. The entropy change for the reaction is (A) 19.69 J deg1 (B) 129.3 kJ (C)19.69 kJ deg1 (D) 9.85 J deg1

3.If and , then is (A)+0.28 V (B) 0.28 V (C)+ 0.74 V (D)+ 1.69 V

4.A graph is plotted between Ecell of quinhydrone half cell and pH of solution. Intercept is 0.699 V. At what pH, Ecell will become 0.492 V? (A)3.5 (B)4.2 (C)7(D)10

5.Calculate the cell EMF in mV for

at 298 K

Given : (AgCl) = 109.56 kJmol1 and (H+ + Cl)(aq) = kJ mol1 (A)456 mV (B)654 mV (C)546 mV (D)none of these

6.At what does the following cell have its reaction at equilibrium?

Given : Ksp = 8 1012 for Ag2CO3 and Ksp = 4 1013 for AgBr

(A)(B)

(C)(D)

7.Calculate the EMF of the cell at 298 K

Pt | H2 (1 atm) | NaOH (xM), NaCl (xM) | AgCl (s) | Ag (Given )(A)1.048 V (B) 0.04 V (C) 0.604 V (D)emf depends on x and cannot be determined unless value of x is given

8.Consider the cell Ag Ag. Given that C2 = 10C1 and that x and y are degrees of dissociation in AgNO3 solution of concentrations C1 and C2 in the two half cells, then log in terms of the emf E of the cell at 298 Kelvin will be

(A)(B)

(C)(D)1) A positron is emitted from . The ratio of the atomic mass and atomic number of the resulting nuclide is

A)22 ; 10B)22 ; 11C)23 ; 10D)23 ; 12

2) A freshly prepared radioactive source of half life period of 2hr emits radiation of intensity which is 64 times the permissible safe level. Minimum time after which it would be possible to work with the source is

A)6hrB)12hrC)24hrD)48hr

3) Mathematical representation for life i.e., when 1/4th reaction is over is given by :

A)B)C)D)

4) Two faradays of electricity will liberate one gram atom of the metal from the aqueous solution of :

A)B)C)D)

1) is one of the most widely used oxidizing reagent. The following equilibria are established in aqueous solution of Cr (VI)

All other equilibria involving other chromium species should be ignored.

Evaluate the equilibrium constant for

A)

B)

C)

D)0.436

2)

. If = degree of dissociation, initial pressure and temperature are and at equilibrium (Vconstant), then is equal to

A)

B)

C)

D)All

5) 1L concentrated NaCl solution is electrolysed using Hg cathode. Calculate the pH of solution after passing 0.005 F charge to this solution. Assume volume of electrolyte remains constant during the electrolysis

A)12.7

B)11.7

C)5.3

D)Will remain unchanged, i.e solution will have pH = 7

8) Oxide ions are arranged in ccp (Cubic Close Packing) in a spinel-structure. One eighth

of tetrahedral holes occupied by ions and one half of the octahedral holes are

occupied by . The volume unoccupied in unit cell of this spinel approximately is

A)38%B)46%C)32%D)24%

3)

The degree of dissociation of at one atmosphere is . The pressure at which is dissociated to is nearly


8.n containers having volumes v, 2v, 3v..nv containing gaseous moles n, 4n, 9n,..n3 respectively are connected with stopcock at same temperature. If pressure of first container is P, then the final pressure when all the stopcocks are opened is

(A) (B)

(C) (D)

2.In 0.1 M aq. H2S solution Kb for is 109 . If [S2] in this solution is 1010, then the dissociation constant for will be (approximately)(A) 1015(B) 1013(C) 1019(D) 1018

4.1 mole HCOOH salt Total moles of H2 gas produced in this entire process is

(A) (B) 1

(C) (D) 21.Three graphs are plotted between P and V for a sample of constant amount of an ideal gas at three different temperatures 400C, 400F, 400K. Match the corresponding graph with their corresponding temperature.

(A)a at 400K ; b at 400F ; c at 400C(B)a at 400K ; b at 400C ; c at 400F(C)a at 400C ; b at 400K ; c at 400F(D)a at 400F ; b at 400K ; c at 400C

2.In a solid xy having the rock salt structure, y-atoms are in FCC. If the atoms at body centered octahedral void and at one edge centred octahedral void is missing, then the formula of the compound will be (A)x16y11(B)x3y4(C)x11y16(D)x4y3

3.10 ml of 0.02 M weak monoacidic base (Kb = 1 1012) is titrated with 0.02 M HCl in water at 298 K. The concentration of H+ at equivalence point is (Kw = 1 1014 at 25C) (A)6.18 103M(B)2.7 102M(C)0.01 M(D)0.1 M

1) 0.1 mol of benzene (Po = 100 mm Hg) and 0.1 mol of toluene (Po = 80 mm Hg) are mixed. To this solution 0.1 mole of urea is added. The decrease in vapour pressure by addition of urea is

A)60 mm HgB)50 mm HgC)40 mm HgD)30 mm Hg

2) Which of the following ions have highest molar ionic conductance at infinite dilution.

A)Ca2+B)K+C)Cl-D)H+

4) For a liquid, the normal boiling point is , then at 2atm pressure its boiling point should be nearly

A)

B)

C)

D)

1) When conc. is electrolysed using mercury as cathode and graphite as anode then which of the following is true :

A)Cl2 is liberated at cathodeB)O2 is liberated at cathode

C)Pure Na is formed at cathodeD)Na + is reduced at cathode

2) An element crystallizes in bcc as well as fcc having edges 300 and 400 pm respectively. The ratio of their densities would be

A)1.18B)2.28C)3.38D)4.48

3) A first order reaction is 50% complete in 200 hrs at 27oC & in 20 hrs at 27oC in presence of catalyst. The decrease in activation energy caused by catalyst is nearly

A)5.7 kJB)7.5 kJC)6.7 kJD)7.6 kJ

5) The gaseous reaction,

is found to be first order with respect to A. If the reaction is started with , the pressure after 10 min is found to be 180 mm Hg. The rate constant of the reaction is

A)

B)

C)

D)

1.Three graphs are plotted between P and V for a sample of constant amount of an ideal gas at three different temperatures 400C, 400F, 400K. Match the corresponding graph with their corresponding temperature.

(A)a at 400K ; b at 400F ; c at 400C(B)a at 400K ; b at 400C ; c at 400F(C)a at 400C ; b at 400K ; c at 400F(D)a at 400F ; b at 400K ; c at 400C

2.In a solid xy having the rock salt structure, y-atoms are in FCC. If the atoms at body centered octahedral void and at one edge centred octahedral void is missing, then the formula of the compound will be (A)x16y11(B)x3y4(C)x11y16(D)x4y3

3.10 ml of 0.02 M weak monoacidic base (Kb = 1 1012) is titrated with 0.02 M HCl in water at 298 K. The concentration of H+ at equivalence point is (Kw = 1 1014 at 25C) (A)6.18 103M(B)2.7 102M(C)0.01 M(D)0.1 M

1) The rate constant of a first order reaction, product, is . Its rate at (A) = 0.01 would be

A)B)

C)D)

2) In the presence of catalyst the activation energy of reaction decreased by 4.606 k.cal at . The rate of the reaction will be increased by

A)2 timesB)10 timesC)100 timesD)1000 times

3) The activation energy of a reaction is 94.14 kJ/mole and the value of rate constant at 313 K is. Calculate frequency factor A.

A)collision/secB)collision/sec

C)collision/secD)collision/sec

1) The root mean square velocity of one mole of a monoatomic gas having molar mass M is Ur.m.s. The relation between the average kinetic energy (E) of the gas and Ur.m.s. is

A)B)C)D)

2) The compressibility of a gas is less than unity at N.T.P. Therefore

A)litersB)litresC)litresD)litres

3) For a real gas obeying van der Waals equation, a graph is plotted between PVm (y- axis) and P (x-axis) where Vm is molar volume. y-intercept of the graph is

A)RTB)

C)D)can not be determined

4) Equal weights of methane and oxygen are mixed in any empty container at 250C. The fraction of the total pressure exerted by oxygen is

A)1/2B)2/3C)1/3D)

47) On electrolyzing K2SO4 solution using inert electrodes, 1.68 L (STP) of gases were obtained. How many moles of could be reduced to Mn2 + by the same quantity of electricity?

A)0.10B)0.20C)0.15D)0.02

48) One litre of 0.1M acetic acid containing enough NaCl is electrolysed by passing 25 milli faradays of electricity. The pH of the solution after electrolysis is, (assume electrolysis of only aq.NaCl & pka of acetic acid = 4.74)

A)4.26B)4.74C)4.44D)5.22

49) One gram of molten SnCl2 is electrolysed for some time using inert electrodes until 0.238g of Sn (At.wt=119)is deposited at cathode. No substance is lost during electrolysis, the % by weight of SnCl2 remaining is,

A)62%B)76%C)24%D)50%

50) Specific conductance of 0.01 M KCl solution is . When conductivity cell is filled with 0.01 M KCl the conductance observed is y . When the same cell is filled with 0.01 M H2SO4, the observed conductance was Z. Hence specific conductance of 0.01 M H2SO4 is:

A)XzB)C)D)

51) A saturated solution of AgBr is taken. Ksp of AgBr is. If mole of AgNO3 are added to 1 litre of this solution find conductivity (specific conductance) of this solution? Given, Molar conductance of and .

A)B)C)D)

52) Given the following molar conductivities at; HCl, NaC (sodium crotonate), . The conductivity of 0.001 mol/dm3 acid solution is . The dissociation constant of crotonic acid is

A)B)C)D)

57) STATEMENT 1: Specific conductance decreases with dilution whereas equivalent conductance increases for strong electrolytes.STATEMENT 2: On dilution, no. of ions per milli litre decreases but total number of ions increases considerably.

A)Statement1 is True, Statement2 is True; Statement2 is a correct explanation for Statement1

B)Statement1 is True, Statement2 is Tue; Statement2 is NOT a correct explanation for Statement1.

C)Statement - 1 is True, Statement - 2 is False

D)Statement - 1 is False, statement - 2 is True.

58) STATEMENT 1: During the electrolysis of water two faraday of charge will produce a total of 33.6 litre of gases at STP at electrodes.STATEMENT 2: In the electrolysis of H2O, four faraday of charge will produce one mole of H2 gas and 1/2 mole of O2 gas





59) STATEMENT 1: Among the alkali metal salts Li salts exhibit the least electrical conductance in aqueous solutions.STATEMENT 2: Smaller the radius of the hydrated cation, lower is the electrical conductance in aqueous solution.





60) STATEMENT 1: The equivalence conductance of HNO2 varies linearly with square root of molar concentrations.STATEMENT 2: The extent of ionization increases with dilution for all weak electrolytes and the equivalence conductance increases.





45) 100ml of a sample of KMnO4 required 1amp of electricity for 1hr 20min and 25sec for the complete reduction of Mn in acidic medium to Mn + 2. The volume of 0.5M MnSO4 required for the complete neutralization of 100ml of same sample of KMnO4 in slightly alkaline medium,

A)120mlB)100mlC)60mlD)30ml

46) In the electrolysis of an aqueous solution of sulphuric acid 1.4L of oxygen and 5.6L of hydrogen at STP are liberated at anode and cathode respectively along with the formation of perdisulphuric acid. The weight of H2S2O8 formed will be

A)97gB)46gC)19.82gD)24.25g

47) The molar conductance at infinite dilution of Fe2(SO4)3 and are x and y respectively. The equivalent conductance at infinite dilution of is

A)B)C)D)

48) Equivalence conductance of saturated solution of BaSO4 is and specific conductance is. Hence of is:

A)B)C)D)

49) At the EMF of the cell Pb/PbCl2//AgCl/Ag is 0.5V and its temperature coefficient is . If the heat of formation of is . The heat of formation of AgCl is,

A)B)

C)D)

50) In acidic medium, MnO2 is an oxidant as, . If the pH of the solution is decreased by one unit, the electrode potential of the half cell Pt: will change by

A)-0.118 VB)0.118 VC)0.236 VD)-0.236 V

51) Given, The for the fuel cell reaction at 298K is,

A)-474.8JK-1B)-325.0JK-1C)474.8JK-1D)571.6JK-1

52) The heat of solution of anhydrous CuSO4 is and that of is. Calculate the heat of hydration of CuSO4.

A)B)C)D)

53) Given the data at What is the value of log Ksp for AgI?

A)B)C)D)

54) Statement 1: Only coloured metal ions give borax bead test. Statement 2: Borax on heating gives a glassy bead comprising of boric anhydride and sodium metaborate.





55) Statement 1: Decrease in freezing point () of ethanoic acid is more in benzene than in water.Statement 2: Molecules of ethanoic acid dimerise in solvents of low dielectric constants.





56) Statement 1: Entropy change in reversible adiabatic expansion of an ideal gas is zero.Statement 2: The increase in entropy due to volume increase just compensate the decrease in entropy due to fall in temperature.





57) Statement1: Lithium is the strongest reducing agent in aqueous solutions, yet it is the least reactive among alkali metal. Statement2: The reducing property and reactivity both are thermodynamically controlled.





1) Two moles of an ideal gas (= 3/2 ) is made to expand reversibly and adiabatically to four times to its initial volume . The change in entropy of the system during expansion is : [R= 2 cal , ln2=0.7]

A)5.6 cal B)11.2 cal C)2.8 cal D)Zero

2) At , gaseous dinitrogen tetra oxide is 50% dissociated. The standard free energy change per mole of at this temperature and at 1 atm is nearly R=8.3 JK-1mol-1, In 10= 2.3, log2=0.3, log3=0.48

A)-756 KJ mol-1B)-856 KJ mol-1

C)-656 KJ mol-1D)None of these

3) At, 1 atm pressure, = 75 J mol-1 = 30 kJ mol-1. The temperature of the reaction at equilibrium is :

A)400 KB)330 KC)200 KD)110 K

4) In which of the following cases entropy decreases?

A)Solid changing to liquidB)Expansion of a gas

C)Crystals dissolveD)Polymerisation

5) A dilute aqueous solution of is electrolysed using platinum electrodes. The product formed at the anode and cathode are

A)B)C)D)

6) When electric current is passed through a cell containing the electrolyte ; + ve ions move towards the cathode and ions move towards anode. If the cathode is pulled out of the solution

A)+ ve and ions both will move towards the anode.

B)+ ve ions will start moving towards anode and ions will stop moving

C)ions will continue moving towards the anode and + ve ions will stop moving

D)+ ve ions and ions will start moving randomly.

7) Which one of the following statements is correct for an electrolytic cell ?

A)Electrons flow from cathode to anode through the external battery.

B)Electrons flow form cathode to anode within the electrolytic solution.

C)Migration of ions takes place along with oxidation reaction at cathode and reduction reaction at anode.

D)Migration of ion takes place along with reduction reaction at cathode and oxidation reaction at anode.

8) In the electrolytic cell , flow of electrons is from

A)Cathode to anode in solution

B)Cathode to anode through external supply

C)Cathode to anode through internal supply

D)Anode to cathode through internal supply

1.The enthalpy of neutralization of a weak monobasic acid in 1M solution with a strong base is 56.1 kJ mol1 whereas the enthalpy of ionization of the acid is 1.5 kJ mol1 and Hneutralisation of strong acid against a strong base is 57.3 kJ equiv1. The percent ionization of the weak acid is (A)10(B)20(C)25 (D)80

2.Dissociation constant Ka value for H3O+ at 298 K will be (A)1014 (B)1.8 1016 (C)55.5(D)1 106 Given : Ionic product of water at 298 K = 1014 M2.

3.A certain mass of gas is expanded from (1L, 10 atm) to (4L, 5 atm) against a constant external pressure of 1 atm. If initial temperature of gas is 300 K and the heat capacity of process is 50 J / C. Then the enthalpy change during the process is (1L atm 100 J ) (A)H = 15 kJ (B)H = 15.7 kJ (C)H = 14.4 kJ (D)H = 14.7 kJ

4.If for the reaction: is 240 kJ, what is G298 for the reaction: (A)245.7 kJ(B)239.3 kJ(C)125.70 kJ(D)245.7 kJ1) The heats of neutralization of four acids A, B, C and D are and kcal equiv-1 respectively, when they are neutralized by a common base. The acidic character obeys the order:

A)A > B > C > DB)A > D > C > BC)D > C > B > AD)D > B > C > A

2) Calculate Q and w for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at a constant temperature of 273 K

A)B)C)D)

3) Latent heat of vaporisation of a liquid at 500 K and 1 atm pressure is 30.0 kcal/ mol. What will be the change in internal energy of 3 mole of liquid at same temperature?

A)13.0 kcalB)C)27.0 kcalD)

4) For the reaction at Given, the value of for the process is

A)B)C)D)

5) Calculate the enthalpy change when 50 mL of 0.01 M reacts with 25 mL of 0.01 M HCl. Given that neutralization of a strong acid and a strong base is

A)14 kcalB)C)D)

6) For the reaction, bond energy of then calculate the average bond energy of bond using the above data.

A)B)C)D)

7) Heat of neutralization of oxalic acid is using . Hence of

A)5.88 kJB)C)D)

8) Calculate the standard enthalpy of formation of from the following data:

A)B)C)D)

1) On the basis of information available from the reaction per mole of oxygen, the minimum emf required to carry out electrolysis of Al2O3 is

A)2.14VB)4.28 VC)6.42VD)8.56 V

2) Calculate the electrode potential at of electrode at pOH = 11 in a solution of 0.01M both in and . value for the cell is 1.33 V .

A)0.725 VB)0.936 VC)0.652 VD)0.213 V

3) In the following sequence of reactions, the standard reduction potentials in volts in acidic medium are given . Calculate for the reaction,

A)7.34 VB)1.468 VC)4.465 VD)0.897 V

4) The standard EMF of the cell in which the reaction occurs is 0.59 V at . The equilibrium constant for the given reaction is approximately .

A)B)C)D)

5) The numerical value of the useful work done during the cell reaction,under standard conditions

A)B)C)D)

6) In lead storage battery, during discharging process, which of the following is/are not the correct statement/s ?

A)PbO2 gets oxidizedB)is produced

C)Density of solution decreasesD)Density of solution increases

7) The emf of the cell: (ct = 1.0 M)Calomel electrode | HCl of unknown pH | Quinhydrone electrodeis 0.25 volt at . The of the calomel electrode at is volt and of the quinhydrone electrode is 0.699 volt. The pH of HCl solution is

A)3.0B)6C)8D)7

8) log graph is of the type as shown in figure where OA=0.34 V then electrode potential of the half cell of will be:

A)B)0.34 + 0.0591 VC)0.34 VD)0.17 V

Multiple Correct Choice Type

5.Of the following cells the condition Ecell = is met by

(A)

(B)

(C)

(D)6.An ideal gas is taken from the same initial pressure P1 to the same final pressure P2 by three different processes. If it is known that point 1 corresponds to a reversible adiabatic and point 2 corresponds to a single stage adiabatic then the correct statement (s) is / are

(A)Point 3 may be a two stage adiabatic (B)The average K.E. of the gas is maximum at point 1 (C)Work done by surrounding in reaction point number 3 will be maximum (D)If point 3 and 4 lie along an isotherm, then W4 3 > W4 2 > W4 1 7.Consider the standard red Pot. Values of species values :

+1.09 V +0.80V

+0.34 V H+ / H2 0.00V Sn+2 / Sn 0.14 V Fe+2/ Fe 0.41 V Al+3 / Al 1.67 V Under standard conditions the species that will oxidize iron but not mercury are (A)H+ (B)Sn+2 (C)Br2(D)Cu+2

8.Hydrogen peroxide can be obtained by the action of dilute acid on (A)PbO2(B)NaBO3(C)H2S2O8 (D)BaO2 9.Choose the correct statement

(A) is more stable than inspite of the fact that their bond order is same (B)When the concentration of the solution of sodium metal in liquid ammonia is increased the paramagnetism of the solution decreases. (C)The acidity of oxides follows the order : CO2 < SiO2 < N2O5 < SO3 (D)Amongst boron trihalides (BX3), the acidity increases as X is replaced gradually by F, Cl, Br and I.

11) The pressure of 11 gm of a gas which is placed in a 4 litres container at is 2 atm, then the gas would be ? (Take R = 0.08 ltr. atm/mol K)

A)N2OB)O3C)NO2D)CO2

12) For a gas having extremely low molecular weight

A)the value of can be neglected compared with p

B)the value of Z increases with increase in p

C)the value of Z decreases with increase in p

D)none of these

7.Pick out the correct statement(s) :A) All adiabatic changes are isoentropic.B) The heat of a reaction depends upon the temp at which it is carried outC) During a cyclic process, Q=0D) EMF of a cell is an extensive property.

09.Which is/are correct for metal sulphide sols?a) The solution particles are positively charged due to preferential adsorption of metal ionsb) The solution particles are negatively charged due to preferential adsorption of sulphide ionsc) The cations of added electrolytes are effective in causing the coagulation of the solutiond) The solution is unstabilised due to both electric charge and hydration of the particles

10.The activity and selectivity of zeolites as catalyst is based ona) Their pore sizeb) Their surface areac) Size of their cavities on the surfaced) Their amount

11.Which of the following statements is/are true?a) In an anti-fluorite structure, anions form fcc lattice and the cations occupy all the tetrahedral voids.

b) If the radius of cations and anions are and then the coordination number of the cations in the crystal is 4c) A cation is transferred from a lattice site to an interstitial position in Frenkel defect.d) Density of crystal always increases due to substitution (impurity) defect.

12.1 mole of a non-volatile compound AB is added to 1 kg of water (). If the ratio of quantities of the compound that undergo dissociation and dimerisation is 1 : 1, which is/are true ?

a) The R.L.V.P. of the solution is

b) The elevation in boiling point of the solution is

c) The depression in freezing point of the solution is

d) The osmotic pressure of the solution at is 49.26 atm.

13.Two different solutions of non-volatile and nonelectrolytic solutes A and B are prepared. The molar mass ratio . Both are prepared a 5% solution by weight in water. Then the correct statements is/are [assume m = M].

a) The ratio of freezing point depressions of the solutions is 3 : 1b) The ratio of L.V.P. of the solutions A and B is 9 : 1

c) The two solutions prepared above are mixed together in the ratio 2 : 3 and 3 : 2 by volume to prepare two other different solutions and respectively, the ratio of is 9 : 11

d) The ratio of osmotic pressures of the two solutions at the same temperature is 5 : 99.Which of the following is(are) correct for Cs Cl type crystal:(A) It is ideal BCC structure. (B) Cs+ and Cl both ions forms a simple cubic lattice which inter penetrate each other. (C) Cs+ ions are at the body centre of Cl unit cell (D) Cl ions are at the body centre of Cs+ unit cell.

10.The capacity of an ion to flocculate the colloidal solution depends upon: (A) amount of its charge (B) sign of its charge (C) formula weight(D) charge density9.Pick out the correct statement(s) from among the following :A) One gram each of Radium elemental and RaSO4 will have the same activityB) The beta particle emitted by a radio active element is from the valence shell of the atom.C) Nuclear isomers will have the same mass number as well as atomic number.

D) The fraction decayed during n half lives is 5.Pick out correct statements :A) An aqueous solution of a weak acid on being diluted its pH decreases.B) The conjugate acid of a weaker base is a stronger acidC) All Arrhenius acids are Lewis acidsD) The degree of hydrolysis of a salt of a weak acid versus strong base is more if the acid becomes weaker.

9.A 0.1M solution of has an osmotic pressure of 4.5atm at , then

(A) Vant Hoffs factor (B) degree of ionization = 0.82

(C) It is isotonic with 0.1M urea at (D) degree of dissociation = 0.96

11. is the packing fraction for structure(s) (A) Face centred cubic(B) HCP(C) BCC(D) cubic close packing

11.Which of the following have (Z is rank of unit cell = No of formula units per unit cell)

(A) ZnS(B) (C) (D)

12.Lyophilic solutions have/are(A) Surface tension is less than dispersion medium(B) Viscosity is more than dispersion medium(C) Surface tension and viscosity remains constant(D) Self stabilized5.Which of the following have the same mass?

A) 0.1 mole of gasB) 0.1 mole of gas

C) molecules of gas D) molecules of gas

6.In which of the following pairs do 1 g of each have an equal number of molecules?

A) andB) and C) and COD) and

7.The oxidation number of Cr is +6 in:

A) B) C) D)

8.Which of the following have been arranged in order of decreasing oxidation number of sulphur?

A) B)

C) D) 9.Which among the following are autoredox reactions?

A) B)

C) D)

9.Which of the following statements about the compound formed from P & Q is/are correct?

a) equivalent weight of = equivalent weight of P + equivalent weight of Q

b) 1 mole of contains y moles of P and x moles of Q

c) 1 mole of contains 1 mole of P and I mole of Q

d) 1 mole of contains x moles of P and y moles of Q

10. and behave as acids as well as reducing agents which are correct statements?

a) Equivalent weight of and are equal to their molecular weights when behaving as reducing agents

b) 100ml of 1 N solution of each is neutralised by equal volumes of 1M Ca

c) 100 ml of 1 N solution of each is neutralised by equal volumes of 1N Ca

d) behaves as acid salt 11)

For reaction , the value of cell potential of given redox reaction cannot be :

A)

B)

C)

D)

53) Identify the correct statements

A)increases with increase in temperature

B)decreases with increase in concentration

C)Specific conductance increases with increase in concentration

D)Specific conductance decreases with increase in temperature.

54) Which of the following concentrated aqueous solutions on electrolysis using inert electrodes liberate oxygen at anode and hydrogen at cathode.

A)MgSO4B)KNO3C)CH3COONaD)AgNO3

55) For which of the following electrolytes the equivalence conductance is same as molar conductance?

A)BaSO4B)NaClC)CaCl2D)CsBr3

56) Which of the following statement is/are correct?

A)In an electrolytic cell the anode is represented by negative sign

B)In an electrolytic cell reduction takes place at cathode

C)In an electrolytic cell a non spontaneous reaction takes place

D)During electrolysis only electrolyte takes part in electrochemical reaction

11. which are the correct statements?a) The product in above neutralisation contains an acidic hydrogen b) resulting mixture is neutralised by 1 mole of KOHc) resulting mixture can also be titrated against HCl

d) 1 mole of is completely neutralised by 1.5 mole of 12.Which of the following statements are wrong?

a) 1 mole of will exactly neutralize 3 moles of b) Weight fraction, vapour density and specific gravity have no units

c) 30 ml of is mixed with 60 ml of at to form a solution of density 0.88 g/d) Molarity of aqueous solution is independent of temperature

7.Which of the following each with 24 electrons can have electronic configuration?

A) B) C) D) 8.s orbitals is spherically symmetrical hence it isA) directional independentB) angular dependentC) directional dependentD) A,C9.On the following quantum state designations, which is/are not allowed state for an electron in an atom?

n m I3 2 -2 II 3 1 0 III 3 0 -1 IV 3 3 0 V 3 0 +1/2A) I,

physical chemistry objective

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