SCH 3U1 Exam Review
Date: Friday, January 23, 2015
Time: 8:30 am – 10:30 am
Room: P23
Exam Prep:
 Review all past tests and quizzes
 Practice writing self quizzes found at the end of each chapter
 Look at unit reviews for each unit for practice questions
 Make a list of MAIN topics from each unit
 Review notes (you are only responsible for the sections we covered in class, may not be EVERY section)
 Bring pencils, pens, eraser and CALCULATOR!!!!
Exam Breakdown
Part A: Multiple Choice (30 marks)
 From all chapters, Chapter 1 to Chapter 12
Part B: Thinking (30 marks)
 balancing / types of reactions, Lewis structures, bond types, polarity, intermolecular forces, ionic
equations, acid-base calculation, gas calculation, parts per calculation
Part C: Application (20 marks)
 molecular/empirical formula calculation, mole calculation, gas calculation, solutions calculation
Part D: Communication (20 marks)
 titration, trends in the periodic table, chemical reactions
SCH3U: Final Exam Review
1.Draw Lewis Diagrams for the following and determine if the bonds are polar, non-polar, or ionic.
a. H2O
b) CBr4
c) O2
2. Write the chemical Formulas for the following:
a. dinitrogen tetroxide
b. carbon monoxide
c. mercury(II) sulfate
d. lead(IV) fluoride
3. Name the types of reactions:
a. N2(g) +3H2(g) → 2NH3(g)
b. 2HI(g) → I2(g) + H2(g)
c. C7H16(l) + 11O2(g) → 7CO2(g) + 8H2O(g)
d. Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g)
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4. Balance the equations:
a. Na3PO4 + Pb(NO3)2 → Pb3(PO4)2 + NaNO3
b. NO2 + H2O → HNO3 + NO
c. C2H6 + O2 → CO2 + H2O
d. Cu + H2SO4 → CuSO4 + H2O + SO2
5. Examine the following reactants, predict the type of reaction that will occur and classify the type of
reaction.
a) CuNO3(aq) + BaCl2(aq) →
b) HNO3(aq) + Ca(OH)2(aq) →
c) NH4NO3(aq) + KOH(aq) →
d) Pb(s)+ CuCl2(aq) →
e) HgO(s) + heat →
6. Terms and Definitions
A
____i. a substance that has other substances dissolved in it
____ii. a substance that is present in a smaller amount in a solution
____iii. a solution in which water is the solvent
____iv. liquids that readily dissolve in each other
____v. liquids that do not readily dissolve in each other
7. Units of Concentration
A
____i. mass solubility
____ii. molar concentration
____iii. parts per billion
____iv. mass/volume percentage
____v. volume/volume percentage
B
a. immiscible
b. aqueous
c. solute
d. miscible
e. solvent
f. solubility
g. alloy
B
a. mol/L
b. g/100mL
c. ppm
d. ppt
e. % (v/v)
f. % (m/v)
g. 1 mg/L
8. Calculating Concentration
A
____i. 30 g of NaCl in 500 mL of solution
____ii. 46 g of NaOH in 100 mL of water
____iii. 5.25 g of AgNO3 in 50 g of water
____iv. 3 mL of hydrogen peroxide in 10 mL of water
____v. 125 g of copper(II) sulfate in 500 g of water
B
a. 46% (m/v)
b. 25% (m/m)
c. 1.03 mol/L
d. 5.25% (m/m)
e. 30% (v/v)
f. 10.5% (m/m)
9. Explain the statement “Like dissolves like.”
10. 0.25 mol of potassium nitrate is added to enough water to make a 175 mL solution. What is the molar
concentration of potassium nitrate?
11. What is the mass/volume percentage of 3.0 g in 50.0 mL of solution?
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12. Calculate the mass (in grams) of sodium sulfide that is needed to make 350 mL of a 0.50 mol/L solution.
13. Calculate the concentration of 0.75 mL of hydrogen peroxide in 10 mL of solution. Express the
concentration as a volume/volume percentage.
14. Calculate the concentration of 0.575 g of magnesium acetate in 265 g of water. Express the
concentration as a mass/mass percentage.
15. 35 mL of a 0.250 mol/L solution of hydrochloric acid is mixed with an excess of silver nitrate. A white
precipitate of silver chloride forms. What is the mass of the silver chloride precipitate?
16. What volume of 0.20 mol/L acetic acid solution is needed to make 100 mL of 0.015 mol/L acetic acid
solution?
17. Use the solubility table to determine if the compound is soluble or insoluble:
a. magnesium sulfate
b. lithium hydroxide
c. calcium carbonate
d. silver nitrate
e. iron(II) sulfite
18. A solution of sodium sulfide is mixed with a solution of copper(II) chloride. Write the total ionic
equation and the net ionic equation for the reaction. Identify the spectator ions in the reaction.
19. An excess of sodium carbonate solution is added to 75.0 mL of calcium chloride solution. 7.50 g of
precipitate is formed. Calculate the concentration of the calcium chloride solution.
20. Name each acid.
a) HBr(aq)
b) H3PO2(aq)
c) H2SO3(aq)
d) HIO3(aq)
e) HBrO4(aq)
21. Write the chemical formula of each acid.
a) carbonic acid
b) hyponitrous acid c) sulfurous acid d) hydrocyanic acid e) perchloric acid
22. 34.2 mL of 0.200 mol/L sulfuric acid neutralizes 23.8 mL of lithium hydroxide. Determine the
concentration of the base.
23. 20.0 mL of 0.15 mol/L sodium hydroxide is reacted with 30.0 mL of 0.20 mol/L sulfuric acid.
a) How many grams of salt are produced?
b) What is the concentration of hydronium ions in the resulting solution?
24. When 15 mL of 0.20 mol/L potassium hydroxide is reacted with 25 mL of 0.20 mol/L hydrochloric acid.
a) How many grams of salt are produced?
b) What is the concentration of hydronium ions in the resulting solution?
25. Gas Laws
____ i. When the volume of a gas is doubled, the pressure is
halved.
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a. Charles' law
b. Boyle's law
____ ii. When the pressure of a gas is tripled, the temperature
c. Gay-Lussac's law
is tripled.
____ iii. When the volume of a gas is decreased by a factor of 5, the temperature is decreased by a
factor of 5.
____ iv. When the pressure of a gas is halved, the temperature is halved.
____ v. When the volume of a gas is increased by a factor of 5, the temperature is decreased by a
factor of 5.
26. What does STP stand for? State the temperature in two units and the pressure in four units.
27. The fuel supply for a course-correcting rocket engine on a communications satellite is contained in a
steel sphere. The volume of the sphere is 10.0 L. The sphere is able to deliver 1400 L of gas at room
temperature (25°C) and 101.3 kPa. Calculate the pressure that the sphere can withstand if the normal
operating temperature of the sphere is -10°C.
28. A car tire contains air at a pressure of 1520 mm Hg and 25°C. When the car is driven, the tire heats up
and the pressure increases to 1900 mm Hg. Assuming that the tire does not expand, calculate the new
temperature inside the tire.
29. A sample of gas has a volume of 30 mL at 1.5 atm. The gas is allowed to expand until its volume is 100
mL. Calculate the new pressure, assuming that the temperature remains constant.
30. What is molar volume? State the molar volume (including the units) of any gas at STP.
31. Calculate the volume that is occupied by 5.05 mol of hydrogen chloride, HCl, gas at STP.
32. Calculate the volume of water vapour that is produced from the combustion of 15.0 g of ethylene at
25°C and 100 kPa.
C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g)
33. How many fluorine gas molecules are in 9.2 L of fluorine gas at STP?
34. A 5.00 g sample of gas has a pressure of 1.20 atm and a volume of 750 mL, at a temperature of 35°C.
Calculate the molar mass of the gas.
35. 148 L of hydrogen gas reacts with nitrogen gas to produce ammonia gas at 65°C and 350 kPa. Calculate
the volume of ammonia gas that is produced at 700 mm Hg and 34°C. N2(g) + 3H2(g) → 2NH3(g)
36. Iron pyrite, FeS2, when roasted in air, reacts to produce sulfur dioxide and iron(III) oxide as follows:
4FeS2(s) + 11O2(g) → 2 Fe2O3(s) + 8SO2(g)
25.2 g of iron pyrite reacts with 5.50 L of oxygen gas at 20°C and 100 kPa. Calculate the mass of
iron(III) oxide that is formed.
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