Student Integrity*

The highest standards of honesty and integrity must apply to your actions while taking your final exams.

LHS Policy mandates a penalty of cheating on an exam to be a grade of ZERO.

Please note:The minimum academic penalty for all parties involved will be a ZERO on the exam.

Cheating includes (but is not limited to) possessing any unauthorized item that might give a student an advantage.

Cell phones and PDA’s MUST be kept out of sight. Cell phones and PDA’s are unauthorized items that might give a student an advantage. As such, if a cell phone is seen during an exam, you will receive a grade of ZERO.

All calculators may be checked for inclusion of extraneous material. No papers should be placed in calculators. No information should be written on calculators.

It is YOUR responsibility to ensure you HAVE NOT violated the policy. Whether you are the person who gives or receives the information, you are guilty of a dishonest act.

CHEMISTRY CP FINAL EXAM REVIEW Name:

1. For each reaction below: identify the reaction type, predict the products and write the complete balanced reaction:

__________________ a. iron (III) hydroxide → iron (III) oxide and water

_____________________________________________________________

__________________ b. ethylene (C2H4) burns in pure oxygen →

___________________________________________________________

__________________ c. magnesium + nitrogen →

____________________________________________________________

2. Complete and balance the reactions below in the space provided.

_____KOH + _____ Pb(NO3)2 _____ Pb(OH)2 + _____ KNO3

_____ Cl2 + _____NaBr ___________________________________________

3. Sodium reacts with calcium chloride to produce sodium chloride and calcium metal.a. Balance ____Na + ____CaCl2 ____Ca + ____NaCl

b. If 43.0g of calcium chloride reacts, how many grams of sodium chloride will be produced? (ans: 45.3g NaCl)

c. The reaction above is performed in lab, and 40.0g of sodium chloride are collected. Determine the percent error and the percent yield. (ans: 88.3%)

Synthesis Decomposition Single Replacement

Double Replacement Combustion

4. Sodium sulfate reacts with aluminum bromide. a. Balance: _____ Na2SO4 + ____ AlBr3 _____NaBr + _____Al2(SO4)3

b. Predict the mass of aluminum sulfate that will form if 25.0g of sodium sulfate react with 60.0g of aluminum bromide. (ans: 20.1g Al2(SO4)3)

c. The limiting reactant is: _______________________________________.

5. Hydrogen reacts with nitrogen to produce ammonia (NH3). If 4.4 liters of ammonia are produced at STP, how many grams of hydrogen reacted? (ans: 0.59g H2)

N2(g) + 3H2 → 2 NH3(g)

6. Use collision theory to explain the effect of each factor below on the rate of a chemical reaction:

a. temperature:

b. surface area

c. stirring

d. adding a catalyst

7. What are the three components to the kinetic theory (for gases)?

1.

2.

3.

8. Use the phase diagram below to identify: a) the triple point b) the normal boiling point c) the state of the substance at 0.5atm and 25°C and d) the change that occurs as the substance is heated from 25°C to 100ºC at 0.5atm.

9. List 2 ways water could be made to boil at 105°C:

a. ___________________________________________________________________________

b. ___________________________________________________________________________

10. Pressure and volume of a gas at constant temperature are __________________ proportional. If the

volume of a gas triples, its pressure will ______________________.

11. Volume and temperature of a gas at constant pressure are __________________ proportional. If the

volume of a gas triples, its temperature will _______________________.

12. Pressure and temperature of a gas at constant volume are ___________________ proportional. If the

temperature of a gas triples, the pressure will __________________________.

0.5atm

1 atm

25 50 75 100 ºCelsius

13. If two containers are at the same temperature and pressure and their volumes are equal, they must contain

the same number of ________________________________.

14. Molecules of oxygen gas and nitrogen gas are at the same temperature in equal sized flasks. Which

molecules are moving faster? __________________________________________________

15. If the oxygen gas molecules and nitrogen gas molecules in the scenario above are all at the same

temperature, which gas has the greatest average kinetic energy? _____________________________________

16. A balloon is filled with 3.0 L of helium at 1 atm. What is the volume of the balloon when the pressure is only 0.25 atm? (ans: 12L)

Hint: Formula:

17. The gas left in a used aerosol can is at a pressure of 3.4 atm at 27.0C. If this can is thrown into a fire, what is the pressure of the gas when its temperature reaches 500.0C? (ans: 8.8 atm)

Hint: Formula:

18. 5.2 L of a gas is at STP. Find the new volume when the temperature rises to 38C and the pressure drops to 600.0 mmHg. (ans: 7.5L)

Hint: Formula:

19. Find the volume occupied by 14.0g of carbon dioxide at 25ºC and 0.880atm. (ans: 8.84L)

Hint: Formula:

20. Find the molar mass of a gas if 3.0g of the gas occupy 1.7L at 25°C and 780mmHg. (ans: 42g/mol)

Hint: Formula:

21. Find the density of Xenon gas at STP.

Hint: Formula:

22. Determine the volume of oxygen gas that required for the complete combustion of 25.0g of methane gas (CH4) at 23°C and 99kPa. (ans: 78L)

RXN: _________________________________________________________________________

23. Complete the table below describing the solubility of each solute.

SOLUTE Soluble in gasoline? Soluble in alcohol? Soluble in water?CBr4

KBrCH2OSiO2

24. Define hydrogen bonding:

25. Circle each of the molecules below that would exhibit hydrogen bonding:

a. HF b. CH2O c. NH3 d. CH4 e. H2

26. List four properties of water that are influenced by its strong hydrogen bonds.

a.

b.

c.

d.

27. Use the graph to answer the questions below:

a. How many grams of KClO3 need to dissolve in 50 g of water in order to have a saturated solution at 70C? ____________

b. Which substance is the most soluble in water at 0C? _____________

c. Which substance is least affected by temperature change? _____________

d. Which substance is the least soluble in water at 0C? ______________

e. Which substance becomes less soluble as the temperature increases? ____________

f. How would you describe the level of saturation of a solution of KNO3 at 40C if there are about 60g of KNO3 in 100g of water? ____________

28. Define “colligative property”:

29. Describe the effect that a solute has on the boiling point, freezing point and vapor pressure of the solvent:

boiling point –

freezing point –

vapor pressure –

30. Fill in the blanks of the following paragraph:

Word bank: pressure, temperature, concentration, high, low, solvent, solute

Molarity, molality, percent by mass and volume express __________________ of a solution. In order to dilute

a solution more of a ________________ can be added. In order to make more concentrated solution more of a

_______________ can be added.

Gases are most soluble in liquids under conditions of _____________________ pressure and

___________________ temperature.

31. Determine the molarity of a solution prepared by dissolving 15.0g of KCl in 525ml of water. (ans: 0.383M)

Hint: Formula:

32. How many grams of KCl are needed to prepare a 0.25 liters of a 3.0 M solution? (ans: 56g KCl)

Hint: Rewrite the molarity as:

33. What volume of 4.0M KCl solution is needed to prepare 750.0mL of a 0.33M solution? What volume of water would also be needed? (ans: 62mL KCl solution, 688mL H2O)

Hint: Formula:

34. What volume of 2.5M hydrochloric acid is needed to react with 32.5g of aluminum? (ans: 1.4L)

RXN: ___________________________________________________________________________

35. What volume of isopropyl alcohol is in 325mL of a 75.0% isopropyl alcohol/water solution? (ans: 244mL)

36. Find the mass percent of sodium chloride in a mixture containing 45.0g of sodium chloride in 255g of water. (ans: 15.0%)

37. Write dissociation equations and determine value of “i” for the following ionic compounds:

a. KCl__________________________________________________________ i = ______

b. Na2SO4 ______________________________________________________ i = ______

c. the value of “ i” for molecular compounds such as C6H12O6 is ____________

38. Determine the boiling point of a solution prepared by dissolving 40.0g of potassium nitrate in 300.0g of water. (kf for water = 1.86°C/m, kb = 0.512°C/m)

a. Find the molality of the solution: (ans: 1.32m)

b. The value for “i” is___________

c. Solve for ΔTb:

d. Find the boiling point: (ans: 101.4°C)

e. How would the problem be solved if you were looking for the freezing point of the solution?

39. What is the difference (in terms of energy) between water at 100C and steam at 100C?

40. Exothermic reactions ________________ (absorb/ release) heat; endothermic reactions _________________ (absorb/ release) heat.

41. A student is heating up sodium carbonate in order to decompose it according to following reaction:

Na2CO3 (s) Na2O (s) + CO2 (g)

Predict signs of ∆ H and ∆S for this process. ∆ H = _____ ∆ S = _____

Under what temperature conditions will this reaction be spontaneous? _____________________

42. Predict signs of ∆S for each process:

a. NaCl (s) Na+(aq) + Cl- (aq). ∆ S = _____

b. FeCl2(aq) + H2SO4(aq) FeSO4(s) + HCl(aq) ∆ S = _____

c. Salt dissolving in water ∆ S = _____

d. Condensation forming on the outside of a cold glass of water ∆ S = _____

43. Predict the amount of heat liberated when 25.0g of potassium chlorate decomposes, based on the reaction below: (ans: 9.11kJ)

2 KClO3 2 KCl + 3 O2 ∆ H = - 89.4kJ

44. The data below refers to substance X.Melting point

Boiling Point

Heat of Fusion

Heat of Va-porization

Specific Heat Ca-pacity (solid)

Specific Heat Ca-pacity (liquid)

Specific Heat Ca-pacity (vapor)

2.0°C 52.5C 275 J/g 1240 J/g 0.90 J/gºC 1.6 J/gºC 0.55 J/gºC

a. Draw a heating curve for substance X, going from -10ºC to 70ºC on the axis below. Write in all formu-las used to calculate heat. Label the phase present at each stage of your graph. Also label changes in potential and kinetic energy.

a.. Calculate the amount of heat needed to raise the temperature of 15g of this substance from 54.0°C to 67.3°C. (ans: 109.7J)

b. What mass of X can be heated from 20.0°C to 35.0°C using 4000J of heat.(ans: 167g X)

c. What amount of heat will be given off if 25.5g of X are cooled from 12.0°C to -5.00°C? (ans: 7580J)

STEP 1:

STEP 2:

STEP 3:

TOTAL:

45. The specific heat of aluminum is 0.910J/gºC. A student heats a sample of aluminum to 123°C and places it in a calorimeter containing 150. g of water at 23.0ºC. The final temperature of the system is 43.0ºC. What was the mass of the aluminum sample? (ans: 172g)

METAL WATERMassspecific heatTi

Tf

∆T

46. Equal mass of each substance below absorbs 1000J of heat, which would become the hottest? Why?

Substance Specific Heat Capacity

aluminum 0.897 J/g°Ciron 0.454 J/g°Clead 0.130 J/g°C

47. Given the diagram below, determine the: (include units)

a. Enthalpy of the reactants_______________

b. Enthalpy of the products_______________

c. Heat of the reaction, ΔH. ________________

d. Activation energy of the reaction. _____________

e. Exothermic or Endothermic? . ___________________

48. What is the pH of a solution that has a concentration of [H+] = 1.0 X 10-6M? ________

Is this solution acidic, basic, or neutral? ___________________

49. What is the pH of a solution that has a concentration of [OH-] = 1.0 X 10-13M? _________

Is this solution acidic, basic, or neutral? ___________________

50. Complete the following table:

Property Acids BasesDefinition

Taste

Touch

Reaction with metals

Electrical conductivity

Reaction with indicators(Phenolphthalein & litmus)2 examples of strong

51. If 25 mL of 1.5 M of HCl is required to completely neutralize 35 mL of NH4OH, what is the concentration of the ammonium hydroxide? (ans: 1.1M)

52. How many mL of 0.5 M NaOH is needed to neutralize 16 mL of a 0.35 M H2SO4? (ans: 22.4mL)

53. Find the molar mass and percent composition (% of each element) for calcium nitrate.

% Ca _______

%N ________

% O ________

54. Find the mass of 1.50 moles of dicarbon tetrachloride.

55. How many molecules are in 14.0 g of dicarbon tetrachloride.

56. Write the empirical formula for dicarbon tetrachloride.________________________

57. A student does a lab to determine the molar mass of barium chloride. In lab, he determines the mass to be 216.0 g/mol. Find his percent error.

58. Identify and give the use for each piece of lab equipment below:

(name both items!)

59. Read each piece of lab equipment below:

buret

____________ mL

graduated cylinder

____________ mL

Thermometer

_________________ °C