Final Examination: Course: Date of Examination: Time of Examination:

PLEASE PRINT:

BROCK UNIVERSITY

April 2013 CHEM IF92 Wednesday April 24, 2013 9:00 am 12:00 pm

Number of pages: Number of students: Number of hours: Instructor:

(

First Name:

26 458

3 Niri

----------------------

Student ID#: Laboratory section number: ---------------------- ----------------~.~~

No examination aids other than those specified are permitted (this regulation does not preclude special arrangements being made for students with disabilities).

Use or possession of unauthorized materials will automatically result in the award of a zero grade for this examination.

A minimum mark of 30% must be obtained on this final examination in order to achieve a passing grade in the course.

You should SHOW YOUR WORK to get full marks.

All questions are to be answered on the examination paper. If you need more space please write on blank pages at end of this paper.

CALCULATORS AND MODEL KITS ARE PERMITTED.

The following information is provided at the end of the paper; These pages may be

Q.l

Q 8

III

List of physical constants and conversions Table of Electronegativities Solubility rules Standard reduction potentials Table of thermodynamic data Formula sheet Periodic Table

Q.2 Q 3

Q 9 Q.10

16 /10

Q.4

Q. 11

/8

Q 5 Q 6

I Total BONUS

1100 /4

Q 7

GRADE, % I

Course: CHEM IF92 April 24, 2013 Page 2 of26 QUESTION 1 (6 marks) keep correct significant figures and include units where needed. Tris(pentafluorophenyl)borane, commonly known by its acronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalyst transition metal compound. It is composed solely ofC, F, and B; it is 42.23% C by mass and 55.66% F by mass.

a) What is the empirical formula of BARF?

b) A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267 111 solution. What is the molecular formula of BARF?

Course: CHEM IF92 April 24, 2013 Page 3 of26 QUESTION 2 (12 marks) keep correct significant figures and include units where needed. Hydrogen for use in ammonia production is produced by the reaction:

Ni catalyst CH/g) + H20(g) ------?) CO(g) + 3H2(g) MJDrxn = 206 kJ/mol, t:,Srxn 216.UKmol

a) Check the appropriate boxes in the following table, using LeChatelier's principle to predict what will happen to the reaction above by applying each of the following stresses

Direction of shift Kind of Stress towards no towards

reactants change products

Adding CH4(g) Removing IhO (g) Removing CO (g) Increasing Temperature by adding heat

Increasing Pressure (decreasing volume) Removing Ni catalyst

b) How does !':,.}?rxn change for the reaction if the Ni catalyst is NOT used? !':,.}? rxn increases MiO rXI1 decreases !':,.}? rXI1 does not change

c) How does activation energy (Ea) change for the reaction if the Ni catalyst is NOT used? Ea increases Ea decreases Ea does not change

d) Calculate I1Go rxn at 25C for this reaction in kJ/mo!.

Course: CHEM IF92 April 24, 2013 Page 4 of26 QUESTION 2 (Cont'd) keep correct significant figures and include units where needed. e) Calculate Kp at 25C for this reaction.

f) Is this reaction spontaneous or nonspontaneous at 25C? __________ _

g) Calculate the temperature range (in C) over which this reaction is spontaneous.

Course: CHEM I F92 April 24, 2013 Page 5 of26

QUESTION 3 (14 marks) a) Within each period of the periodic table, the atomic radius generally _________ _

(increases/decreases) with increasing atomic number.

b) The conjugate base ofH2P04 is _____ _

c) How many unpaired electrons does 34Se have? 00 01 02 03 04

d) What is the frequency of the yellow-orange light (Ie = 589 nm) produced by sodium-vapor streetlights?

o 1.96 xlO- IS Hz 1.96 xl 0-6 Hz

05.09 Hz o 5.09 xl05 Hz o 5.09 xlO I4 Hz

e) The Lewis structure of the CO} 2- ion is ___ _

1/1 ~ .. Q!

:0 0: ~ II

C I :0 ~

2

:0 e II c

/ \ :0 * :0 :

o

2-:0 :

II C

/ \ :0 -0'

1) What is the pH of a buffer that is 0.12 M in lactic acid, lactate? (Ka for lactic acid is L4x 1 0-4 )

0.08 o 1.20 03.77

3.93 7.00

2-

:0 : I

/C\ :0 :0

2-'* ~C $

/ \

\ I .0.

o

and 0.1 0 M in sodium

2

Course: CHEM IF92 April 24, 2013

QUESTION 3 (Cont'd) g) A real gas will behave most like an ideal gas under conditions of ____ _

o high temperature and high pressure o high temperature and low pressure

low temperature and low pressure o low temperature and high pressure o standard temperature and pressure (STP)

h) What types of intermolecular forces exist between HI and H2S? o dispersion forces and dipole-dipole o dispersion forces, hydrogen bonding, dipole-dipole, and ion-dipole o dispersion forces, dipole-dipole, and ion-dipole o dipole-dipole and ion-dipole o dispersion forces, dipole-dipole, and ion-dipole

i) The normal boiling point of the substance with the fol1owing phase diagram is

1.5

Page 6 of26

-----

o 10C D20C D30C D40C D50C {) -10 () 10 ~o :3tI

Course: CHEM IF92 April 24, 2013 Page 70f26

QUESTION 4 (J 2 marks) a) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:

2N02 -j> 2NO + O2 In a particular experiment at 300C, [N02] drops from 0.0100 M to 0.00650 1M in 100 s. The average rate of appearance of 02 for this period is ___ _

o 7.0 xlO-3 Mis o 3.5 xlO-5 Mis o 7.0 x 10-5 Mis o 3.5 xlO-3 Mis o 1.8 x10-5 Mis

b) The rate constant for a particular second-order reaction is 0.47 MIS-I. If the initial concentration of reactant is 0.25 mol/L, how long will it take for the concentration to decrease to 0.13 mollL.

o 0.13 s 07.9 s o 1.7 s 03.7 s 01.4s

c) The reaction below is first order in [H202]: 2 H202 (I) -j> 2 H20 (1) + 02 (g)

A solution originally at 0.600 MI-b02 is found to be 0.075 M after 54 min. reaction is

-----

o 14 min o 18 min

6.8 min 54 min 28 min

d) The following reaction occurs in aqueous solution: NH/ (aq) + N02 (aq) -j> N2 (g) + 2 H20 (1)

data below is obtained at 25C.

The order of the reaction in

o 1 ') L,

o 0-2

fNH4+] eM) [NOr] (M) Initial rate (MIs) 0.01 00 0.200 3.2 )( 10-3 0.02.00 0.200 6.4 )( 10--3 ~I

IS -----

half-life for this

Course: CHEM IF92 April 24, 2013 Page 8 of26

QUESTION 4 (Cont'd) e) The rate law for a reaction is

rate = k [A][B]2

Which one of the following statements is false?

o The reaction is first order in A. o The reaction is second order in B. o The reaction is second order overall. o If [B] is doubled, the reaction rate will increase by a factor of 4. o k is the reaction rate constant

f) Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction?

Ox Oy

x y o x+y o y x

Reaction pathway

g) Which energy difference in the energy profile above corresponds to the activation energy for the reverse reaction?

x

Oy Ox y o x+y o y-x

h) For the elementary reaction

the molecularity of the reaction is ___ _

o

02 3 4

i) For the elementary reaction

the rate law is ----_.

Rate = k [N03] Rate k [N03] [CO] Rate k [N02] [C02] Rate k [N03] [CO] [N02]

ORate = k [N03][CO] [N02] [C02]

Course: CHEM 1 F92 April 24, 2013 Page 9 of26 QUESTION 5 (8 marks) a) Of the following, which is the strongest acid?

HCIO all are the same

b) Which of the following is the strongest base? H3P04: pKaJ = 2.15, pKa2 7.20, pKa3 12.38

o H2P04 HP04

o pol-HS04 SO/-

H2S04: pKaJ strong acid, pKa2 1.99

c) What is the concentration of hydronium ions (H30+) in a solution with pH 4.32? (pay attention to the number of significant figures)

o 5xlO-5 M o 4.8xlO-5 M o 4.79xlO-5 M o 2.1xl04 jVf o 2.09x104 M

d) For which equilibrium, Kp Kc? A(g) + B(g) ~ C(g)

o A(g) + 3B(g) ~ 2C(g) 2A(g) ~ 2B(g) + C(g) A(g) ~ B(g) + C(g) A(g) + B(g) ~2C(g)

e) The value of equilibrium constant Kp for the reaction H2 (g) h (g) ~ 2 HI (g)

is 794 at 25C. What is the value of Kp for the equilibrium below?

0.0013 0.035

028 0397

1588

(g) ~ '12 (g) + Yz h (g)

Course: CHEM 1 F92 April 24, 2013 Page 10 of26

QUESTION 6 (8 marks) No calculations are required for these questions. Think CAREFULLY. The following plot shows the pH curves for several acid-base titrations. In each case, 50.00 mL acid is titrated with 0.10 MNaOH.

12,0

1(10

RO

6.0

4,0

10 2IJ j;() 40

O. lv1

a) Which curve corresponds to the strongest acid? _____ _

b) Which curve corresponds to the weakest acid? _____ _

c) Which curve corresponds to the acid with Ka =10-6? _____ _

d) Which of the following acid-base indicators would be most appropriate to use for titration curve (e )? ___ _

e) What volume of 0.10 MNaOH should be added to acid (c) to make a buffer? ____ _

t) Over what pH range could a buffer made from acid (c) be used? ______ _

g) All of the acids depicted above are at the same initial concentration. What is the initial acid concentration?

~--------

Course: CHEM IF92 April 24, 2013 Page 11 of26 QUESTION 7 (5 marks) a) Which one of the following processes produces a decrease of the entropy of the system?

o dissolving a lump of sugar in a cup of coffee evaporating of liquid bromine, Br2(l)

o sublimation of dry ice, CO2(s) o deposition of sulfur (S) on the wall of a flask o explosion of TNT

b) The first law of thermodynamics states that

o the entropy of the universe increases for spontaneous processes. o the entropy of the universe does not change for nonspontaneous processes. o the entropy of a pure, perfect crystalline substance at absolute zero is zero. o the total energy of the universe will not change. D the first two are correct.

c) What is the best thermodynamic term used for predicting spontaneity of a process?

o Enthalpy change (M-!) o Entropy change (M) o Free energy change (llG) D Temperature (7)

Pressure (P)

d) Which of the following is NOT a state function?

Intemal energy o Enthalpy o Entropy D Work

Gibbs free energy

e) Which of the following is true when a reaction is at equilibrium?

llHrxn 0 llHrxn < 0 L'lSrxn = 0 llGrxn = 0 llGrxn 0

Course: CHEM IF92 April 24, 2013 Page 12 of26 QUESTION 8 (11 marks) keep correct significant figures and include units where needed. Consider the following electrochemical cell:

Ni(s) I Ni2+(O.050 M) II Ag+(O.OIO M) I Ag(s) a) Write down the balanced half-reaction happening in anode (include states):

b) Write down the balanced half-reaction happening in cathode (include states):

c) Write down the balanced redox reaction happening in the cell (include states):

d) Given the standard reduction potentials at the table attached to this paper, calculate FecI! (in Volts) at 25C and indicate if it is a galvanic (voltaic) or electrolytic cell as it is shown.

Course: CHEM IF92 April 24, 2013 Page 13 of26 QUESTION 8 (Cont 'd) keep correct Hgni{icant figures and include units where needed. e) Calculate the cell potential, ECeli (or emf) in Volts for the cell as shown at 25C.

f) Calculate I1Go in kJ for the reaction at 25C. (hint: Faraday constant is in the attached physical constants)

g) Calculate Kc for the redox reaction at 25C.

Course: CHEM IF92 April 24, 2013

QUESTION 9 (6 marks) a) The purpose of the salt bridge in an electrochemical cell is ____ _

o to provide a source of ions to react at the anode and cathode. o to maintain electrical neutrality in the half-cells via migration of ions. o to provide oxygen to facilitate oxidation at the anode. o to provide a means for electrons to travel from the anode to the cathode.

to provide a means for electrons to travel from the cathode to the anode.

b) Consider an electrochemical cell based on the reaction: Sn (s) + 2H+ (aq) - Sn2\aq) + H2 (g)

Which of the following actions would change the measured cell potential?

o lowering the pH in the cathode compartment o increasing the pH in the cathode compartment o increasing the pressure of hydrogen gas in the cathode compartment o increasing the [Sn2+ ] in the anode compartment

any of the above will change the measure cell potential.

c) Which of the following reactions will occur spontaneously as written?

Page 14 of26

o 2Cr3\aq) + 3Fe(s) - 2Cr(s) + 3Fe2\aq) Half-reaction EO (V) ~~---------------4--~-

o 2C?\aq) + 3Sn2+(aq) _ 2Cr(s) + 3Sn4+(aq) Cr3+ (aq) + 3e- -+ Cr (s) -0.74 Fe2+(aq) + 2e- -+ Fe(s) -0.440 Fe3+ (aq) + e- -+ Fe2+ (s) +0.771 Sn4+ (aq) + 2e- -? Sn2+ (aq) +0.154 o 3Sn4\aq) + 2Cr(s) - 3Sn2+(aq) + 2Cr3\aq)

d) Cathodic protection of a metal pipe against corrosion usually entails ____ _ o coating the pipe with another metal whose standard reduction potential is less negative than

that of the pipe. o attaching an active metal to make the pipe the anode in an electrochemical cell.

attaching an active metal to make the pipe the cathode in an electrochemical cell. o attaching a dry cell to reduce any metal ions which might be formed. o coating the pipe with a fluoropolymer to act as a source of fluoride ion (since the latter is so

hard to oxidize).

e) How many minutes will it take to plate out 16.22 g of Al metal from a solution of A13+ using a current of 12.9 amps in an electrolytic cell?

60.1 min 225 min

074.9 min 13480 min 173 min

Course: CHEM 1 F92 2013

QUESTION 10 (10 marks) a) Which systematic name is most correct for the following compound?

2-ethyl-2-methyl-4-propylhexane 2-ethyl-2-methyl-4-ethylheptane 3,3-dimethyl-5-propyl-heptane 3,3-dimethyl-5-ethyloctane

o 5-ethyl-3,3-dimethyloctane

b) Which systematic name is most correct for the following compound? 3-methyl-5-ethyl-7-propyl-2,4,6-decatrien

o 5-ethyl-3-methyl-7-propyl-2,4,6-decatrien o 4-propyl-6-ethyl-8-methyl-4,6,8-decatrien o 6-ethyl-8-methyl-4-propyl-4,6,8-decatrien o 3-methyl-7 -propyl-5-ethyl-2,4,6-decatrien

c) Which systematic name is most correct for the following compound? o 3 ,4-dichloro-l ,2,3 ,4-tetramethylcyc1obutene o 1 ,2-dichloro-l ,2,3 ,4-tetramethylcyc1obutene o 1 ,2-dichloro-l ,2-dimethyl-3,4-dimethylcyc1obutene o 3,4-dichloro-l,2-dimethyl-3,4-dimethylcyc1obutene o 1,2,3,4-tetramethyl-3,4-dichlorocyc1obutene

d) Which systematic name is most correct for the following compound? I-heptylbenzene

o 3-heptylbenzene o 3-phenylheptane o 5-phenylheptane

l-ethyl-l-pentylbenzene

e) Which systematic name is most correct for the following compound? I-methyl-2-ethyl-4-bromocyc1ohexane 4-bromo-2-ethyl-l-methylcyc1ohexane I-bromo-3-ethyl-4-methylcyclohexane

o 4-bromo-5-ethyl-6-methylcyclohexane o I-methyl-4-bromo-2-ethylcyclohexane

150f26

Cl Cl

Course: CHEM 1 F92 April 24, 2013 Page 16 of26

QUESTION 10 (Cont'd) :f) Which of the followings shows the structure of 2-bromo-3-chlo:ro-trans-2-pentene?

CH3CH2" /CH, CH}CI-h,,- /13r CH,CIh /Br c=c c=c "C=C

/ " / " / - " (1 BI' Cl CIl, CH3 C1 .'

0 0 0

g) Which of the followings is a secondary (2) alcohol?

o o

h) The compound below is a(n) ___ _ D primary amine o secondary amine o tertiary amine D primary amide o tertiary amide

i) The compound below is a(n) ___ _ o aldehyde o ketone D ester o carboxylic acid

amme

CH)CH3 I - . CH3 CCH2CH3

I OH o

j) Which structure below represents an ether?

-0-

o II

c-

CH CH, C1 CH3CI-h" /(H1 3 _" / C=C C=C

/ " Br/ . "Cl Br CH3 0 0

I CH,:\CH.,CHCH

~ -I . OH

o o

CH3 I ~ CH3 -N-CH -~ 2

H 0 H I II I

H- C- C- ()--- C-H I I H H

Course: CHEM IF92 April 24, 2013

Question 11 (8 marks) Consider the following organic compound to answer the following questions:

(1)0

a bee II (2) CH2-CH-CH2- -OH

a) This compound is D Aldehyde D Ketone D Carboxylic acid D Ester D Amide

b) What is the hybridization of carbon (f)?

D sp

c) What is the hybridization of carbon (c)?

D sp

d) What is the hybridization of oxygen (2)?

D sp 3 sp

d l CH3

e) Which carbon is an asymmetric centre (chiral centre)?

a b c d

3 :) D.spa

none

Page 17 of26

f) In the real three-dimensional molecule, what is the approximate bond angle marked a?

g) What is the systematic name of the compound?

Course: CHEM IF92 April 24, 2013 Page 18 of26 .::::...:;;;~= (4 marks): Let's see how many faces you remember! '-"uvv,,'- the right person and do your

best to dawn your choice's name.

a) Who was the winner of Nobel Prize for his work on photoelectric effect? --------------------

b) Another Nobel Prize winner who developed a model of atom with the atomic nucleus at the centre and electrons in orbits around it?

--------------------------

o

c) Who had a dream about the structure of benzene molecule? _________________ _

o

Who was the instructor of your first-year chemistry (Chern 1 F92) course? -----------------

Course: CHEM 1F92 April 24, 2013 Page 19 of26

EXTRA PAGE FOR YOUR ;;;..::;:;..;..::;;....:...:..;::;;:;::;.= (IF NEEDED)

Course: CHEM IF92 April 24, 2013 Page 20 of26 EXTRA PAGE FOR CALCULATIONS .....

Course: CHEM IF92 April 24, 2013 Page 21 of26

PHYSICAL CONSTANTS and CONVERSION FACTORS:

Avogadro's Number NA

Planck's Constant h

Speed of light c

Rydberg constant RH Ideal Gas Constant R

Faraday constant F

Pressure

Temperature

Energy units

Electrical current unit

Molar heat capacity H20(l) Specific heat capacity H20(l)

Molar heat capacity H20(g) Specific heat capacity H20(g)

Molar heat capacity H20(s) Specific heat capacity HlO(s)

Heat of vaporization H20(!)

Heat of condensation H20(g)

Heat of fusion (melting)

Heat of freezing H}O(g)

Density of t-bO(l)

Conversion factors:

6.022 x 1023 mOrl

6.6256 x 10-34 J s 2.9979 x 108 m S-l

2.] 79907 x 10-18 J 0.08205 L atm I (mol K) 8.314 J I (mol K) 9.647x104 Clmol e- or IN.mol

I atm 101.325 kPa 1 atm = 760 mm Hg I mm Hg= 1 torr I mm Hg 13.6 mm H20(l)

K = 273.15 + C

1 J kg.m2li I cal = 4.184 J 1 L atm 1 0 1.3 J

Ampere = Columblsecond or A = Cis

75.36 J K- I marl 4.183 J K-I g-l

33.76 J K-I marl 1.874 J K-I g-I

38.07 J marl K- I 2.113 J g-I K- I

40.79 kJ morl 2257 J g-I

between OC and 100C between OC and 100C

at constant pressure at constant pressure

at constant pressure at constant pressure

at 100C at 100C

Heat of vaporization H20(!)

6.007 kJ marl 333.4 J g-I

- Heat of fusion (melting) H20(s)

0.9971 g/mL at 25C

1 kg = 1000 g 1 g 1000 mg 1 cc = 1 cm3 1 mL Inm 10-9 m

Course: CHEM IF92 April 24, 2013 Page 22 of26 Pauling Electronegativities from Chang:

H 2.1 Li Be B C N 0 F 1.0 1.5 2.0 2.5 3.0 3.5 4.0 Na Mg AI Si P S CI 0.9 1.2 1.5 1.8 2.1 2.5 3.0 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br 0.8 1.0 1.3 1.5 1.6 1.6 1.5 1.8 1.9 1.9 1.9 1.6 1.6 1.8 2.0 2.4 2.8

Soluble compounds: Most nitrates, chlorates, acetates and bicarbonates are soluble. Most compounds containing alkali metal (Group lA) cations and ammonium ion NH/ are soluble.

I bl C h fA + C 7+ S 7+ B ?+ H 7+ d Pb7+ Most sulfates are so u e except lor t ose 0 g, a-, r-, a-, g2-, an - . Most chlorides, bromides, and iodides are soluble except those of Ag+, Hgl+, and Pb2+.

Insoluble compounds: Most hydroxides are insoluble except for those of alkali metal (Group lA) cations and Ba2+. Most phosphates, carbonates, chromates and sulfides are insoluble except for those of alkali metal (Group I A) cations and ammonium ion NH/.

Standard Reduction Potentials (EO) at 25 Potential (V) Reduction

+2.87 FZ{l?) + 2 e- -- 2 F-{aq) Mn04 + 8 f-I + 5 e -- Mnl+(fut) 4

2 (aq) 7 2

+H)6 -- NO(g) + 2

+0.68 1- 4

2 I 4e 4

.... ~

-~

--

--

--0.8:5 2 L66

Ij(s)

Course: CHEM 1 F92 April 24, 2013

Table of Thermodynamic Date

o --Hi7J59

llO.525

0

~46.1 J

42.55

0 Ht

143.9 205.79 19L6J I

Page 23 of26

o

671.257 o

o

57.244

() 16.45

()

o 194

Course: lF92 April 24, 2013 Page 24 of26

Table (page 1 of 2) Relationship between energy and wavelength or frequency of light: Formal charge =

I

E = h v or E = h5'i # valence electrons - (2 x # lone pairs + 1 x # bonding pairs)

Energy of an electron in the ntl1 shell of Bohr model of hydrogen-like Energy change when an electron moves between two shells of atom: hydrogen-like atom:

E =-R (L J II H 1 n- M=R+J,-~J n, 11/ Ideal Gas Law: PV nRT an-[ '] van der Waal' s equation: P + V 2 [V - nb] = nRT Dalton's Law of Partial Pressures: Relationship of partial pressure to mole fraction:

Ptotal = PA + PB + Pc + . P A = XA,Ptotal

Heat change due to change of phase: q = nW Heat change due to change of temperature at constant P:

q = mS{T/ - ~) (where S = specific heat) Heat change due to change of temperature at constant V: Standard enthalpy change for a reaction:

q - Ccal !"J.t (where Ccal = heat capacity of calorimeter) W;)w, = InW~(products)- ImLVl~(reactants)

Graham's diffusion and effusion law: Ii = f!i r2

~3RT Root-mean-squ3Te speed of gas molecules: UrlllS = M

-----

Hemy's Law: c=kP pH = -log [H+]; pOH = -log [OH ]; pH + pOH = 14.00

K,,= [H+][A -]

Kb = [OH-][H+] [base]

[HA] [A -] Henderson-Hasselbalch eqn: pH = pK(j + log -[ -. -] aCId

[R"] [OH-] Kw KaKh = 10-14 S 1 . d' . - b -Ji ,2 4ac o utIOn to qua ratlc equatIOn: x = 2a

Course: IF92 April 24, 2013 Page 25 of26

(page 2 of2)

concentration-time equation: [A J/ = -kt + [A Jo First-order concentration-time equation: I

Zeroth order half-life: [AJo In[AJ/ -In[AJo =-kt or In [Al =-kt t --- [AL ]12 - 2k

First-order half-life: In(2) 0.623 tl!2 =-k-=-k-

Second-order concentration-time equation (A ---+ product): Arrhenius Equation: 1

=kt+ 1 k = Ae-EaIRT

[A]/ [AJo Arrhenius Equation (Ln form): Second-order half-life: In(2) 0.623 E till = -k = -k- Ink = InA--a

RT Standard enthalpy change for a reaction: Standard entropy change for a reaction:

M!,"m = L nM!; (products) - L mM!; (reactants) fhl~m = L nSo (products) - L mSo (reac tan ts) Standard free energy change for a reaction: Gibbs free energy under standard conditions, I1GO:

I1G;J,,, = nl1G; (products)- ml1G~ (reactants) I1Go = M-r - Tfhlo Relationship between equilibrium constant (K) and I1GO: Gibbs free energy under standard conditions, I1G:

I1Go = -RTlnK (gases: K = Kp solutions: K Kc) I1G = I1Go + RT In Q Relationship between Kp and Kc: Kp = KcCRT)M =Kc(0.0821T)b.n Entropy change for phase transition: fhl = M!1r For an electrochemical reaction:

= E:athode - E:rlOde Gibbs free energy for a redox reaction:

For a chemical redox reaction: (F=9.647x104 Clmol or .TN.mol) I1GO = -nFE;cll EO == Er:duction - E~xidatioll EO cell (in Volts) for an electrochemical system: Nemst Equation:

E;cll = :; In K al2S"( EO _ 0.0592 1 K E = EO _ RT lnQ 0125(, E = EO _ 0.0592 10gQ

) cell - og n nF n

Electrical charge: nF , n number of moles of exchanged e- Electrical charge for electrolysis: Q=I-t - - ----- --~~---~

--"-- ------_.-

Course: IF92 April 24, 2013 Page 26 of26

THE dl .... .lI.!.tlV,U)d. vmA

2 Ii Be

IIA rnA IVA VA VIA VIlA 4.00200 .3 .5 6 7 8 9 10 Li B C N' 0 F Ne

6.941 HUH 1 12.011 14.0067 15.9994 UI.9984 20.1.797 11 12 13 14 15 17 N~ AJ Sf P

22.9898 24.3050 IUS IVB VB VIB VIIB IS UB 26.9815 28.0855 30.9738 19 20 21 22 23 24- 25 27 28 29 30 31 33 K (A Se n V Mn. Co M C. ZIt G. As

39.0983 40.078 58:9332 Stt69 65.39 69~723 31 38 45 46 48 49 Itb Sr Itb Pd Cd In

85.4678 8U;2 102.906 106.42 112.41 114.82 121.75 55 .56 57 72 17 78 81 82 83 Cs Ba La* Dr Ta Os II' Pt '11 PI '81

132.905 131.33 138.906 178.49 180.948 190.2 192.22 195;08 204;383 '2n1.2 208.980 87 88 105 106 Fl" Ita

(223) 226.025

58 59 00 61 62 63 64 65 66 67 68 * Lanthanide series I Ce Pi' Nd Pm 8m E. Gd Tb D1 Bo Er

140.12 140.908 144.24- 157.25 158.925 162.50 164.930 167.26

Actillide series