Chemistry 2202 Midyear Exam
January 2004
Page 1
Initials: __________
Part A: Multiple Choice (30 marks)
Write the letter of the selection that best answers the following questions in the appropriate blank
on the answer sheet provided. Each question is worth 1 mark.
(1) The coefficients are missing from the reaction equation below.
Cr(s) + Fe(NO3)2(aq)  Fe(s) + Cr(NO3)3(aq)
The correct order of the missing coefficients is _____.
(a) 4,6,6,2
(c) 2,3,3,2
(b) 2,3,2,3
(d) 1,3,3,1
(2) Which of the following compounds is soluble in water?
(a) Ca(OH)2
(b) AgBr
(c) Sr(OH)3
(d) FeSO4
(3) Which of the following compounds is NOT soluble in water?
(a) NH4OH
(b) CuCl2
(c) Na2SO4
(d) CaCO3
(4) The coefficients are missing from the following reaction equation:
N2 + H2  NH3
The order of the missing coefficients is _____.
(a) 1,1,2
(c) 3,1,2
(b) 1,3,3
(d) 1,3,2
(5) For the following chemical reaction:
__ H2SO4(aq) + __ Al(OH)3(s)  __ HOH(l) + __ Al2(SO4)3(s)
Which coefficients will balance the equation?
(a) 1,2,2,3
(c) 3,2,6,1
(b) 1,2,3,1
(d) 3,2,3,1
(6) Freons are compounds that are used as refrigerants. The molar mass of the freon with the formula
CCl2F2(g), is
(a) 58.00 g/mol
(c) 101.91 g/mol
(b) 66.46 g/mol
(d) 120.91 g/mol
(7) What is the number of moles of beryllium atoms in 36 g of Be?
(a) 0.25 mol
(b) 4.0 mol
(c) 45.0 mol
(d) 320 mol
(8) What mass of oxygen is present in 32 g of oxygen gas?
(a) 1.0 moles
(b) 2.0 moles
(c) 3.0 moles
(d) 4.0 moles
(9) A vinegar label reads 8% (v/v) acetic acid. What does this means in terms of the
concentration of acetic acid?
(a) 8 mL of pure acetic acid in every 100 mL of solution
(b) 8 g of pure acetic acid in every 100 mL of solution
(c) 8 mL of pure water in every 100 mL of acetic acid
(d) 8 mL of pure acetic acid in every 100 mL of solvent
(10) What is the percent by volume of 400 mL of a solution that contains 80mL of calcium
chloride, CaCl2?
(a) 10%
(b) 20%
(c) 30%
(d) 40%
Chemistry 2202 Midyear Exam
January 2004
Page 2
Initials: __________
(11) A typical household ammonia solution has a concentration of 1.44 mol/L. What volume of
this solution would contain 1.340 mol of NH3?
(a) 0.403 L
(b) 0.605 L
(c) 0.930 L
(d) 1.07 L
(12) What does not change when a solution is diluted by the addition of solvent?
(a) Concentration of solution
(b) Mass of solvent
(c) Number of moles of solute
(d) Volume of solvent
(13) What is the molarity of 500 mL of solution in which 5.0 moles of sodium bromide is
dissolved?
(a) 0.25M
(b) 2.5 M
(c) 5.0 M
(d) 10M
(14) What is the molality of a solution where 1.50 moles of salt are dissolved in 500g of ethanol?
(a) 0.75M
(b) 3.0 M
(c) 5.0 M
(d) 10M
(15) A solution that has the maximum solute dissolved in the solvent is called
(a) concentrated
(b) dilute
(c) limiting reagent
(d) saturated
(16) A solution that has little solute dissolved in the solvent is called
(a) concentrated
(b) dilute
(c) limiting reagent
(d) saturated
(17) A solution with a concentration of 1.0 M is diluted from 100 mL to 200 mL. The
concentration of the diluted solution is
(a) 0.5 M
(b) 1.0 M
(c) 2.0 M
(d) 10 M
(18) A solution with a concentration of 5.0 M is diluted to a concentration of 10 M. If the
original volume was 100 mL, the volume of the new solution is
(a) 50 mL
(b) 100 mL
(c) 200 mL
(d) this is not possible
(19) An aqueous solution is one which
(a) is clear
(c) has water as the solute
(b) is colourless
(d) has water as the solvent
(20) What is the molar mass of C5H12?
(a) 13.02 g/mol
(c) 60.05 g/mol
(b) 17.00 g/mol
(d) 72.17 g/mol
(21) The mass of one mole of magnesium hydroxide is:
(a) 58.33 g/mol
(c) 40.31 g/mol
(b) 41.32 g/mol
(d) 42.33 g/mol
(22) 2.0 mol of Ba(NO3)2 contains ___ mol of oxygen atoms
(a) 12.0
(b) 6.0
(c) 3.0
(d) 2.0
(23) Which gas sample will occupy the most volume at STP?
(a) 2.0 mol of NH3
(b) 4.0 mol of O2
(c) 3.0 mol of H2
(d) 1.0 mol of CO2
(24) The volume of 2.357 mol of oxygen gas at STP is:
(a) 0.1052 L
(c) 9.504 L
(b) 52.80 L
(d) 37.71 L
Chemistry 2202 Midyear Exam
January 2004
Page 3
Initials: __________
(25) 10.0g of a metallic element is found to contain 0.4414 mol of that element. Which metal must
it be?
(a) Mg
(b) Ca
(c) K
(d) Cs
(26) The mass of 0.250 mol of chromium (II) sulfate is:
(a) 34.02g
(c) 50.02g
(b) 21.02g
(d) 37.02g
(27) Which statement correctly describes STP?
(a) 0OC and 100 kPa
(c) 0 OC and 101.3 kPa
(b) 100 OC and 100 kPa
(d) 101.3 OC and 0 kPa
(28) A solution of NaOH contains 1.5 moles in 250 mL of solution. What is the concentration of
solution?
(a) 1.5 mol/L
(b) 6.0 mol/L
(c) 16.7 mol/L
(d) 375 mol/L
(29) How many grams are in 0.400 mol Pd?
(a) 0.00376 g
(c) 26.6 g
(b) 18.4 g
(d) 42.6 g
(30) How many moles of CaBr2 are there in 5.0 grams of CaBr2?
(a) 2.5 x 10-2 mol
(b) 4.2 x 10-2mol
(c) 4.0 x 10 1mol
(d) 1.0 x 101mol
Part B: Short Answer (70 marks)
Answer all of the following questions in the space provided.
(31) Find the molar mass of each of the following (2)
(a) Uranium (V) phosphate
(b) hexasilicon monoxide
(32) Find the number of moles in each of the following (8)
(a) 31.2 g of aluminum nitrite
(b) 2.53 kg of sulphur trioxide
(c) 21.5 L of carbon dioxide at STP
(d) 250.0 mL of a 2.5 M Calcium chloride
solution
Chemistry 2202 Midyear Exam
January 2004
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Initials: __________
(33) Find the mass of 4.05 moles of water (2)
(34) What is the volume of 40.50 moles of nitrogen dioxide at STP? (2)
(35) What is the percent composition of C2H5OH? (6)
(36) Bugs Bunny is asked to prepare a solution for Yosemite Sam (Why I don’t know). He is
asked to make 655 mL of a 2.457 mol/L solution of sodium carbonate. Calculate the mass
required to make this solution. (6)
(37) Bugs is now asked to dilute the solution he just made in #36 above. If he adds 545 mL of
water to this solution, find the concentration of his diluted solution. (4)
Chemistry 2202 Midyear Exam
January 2004
Page 5
Initials: __________
(38) Stephanie is trying to find out the concentration of Lead in the lake near here home. She
conducts an experiment and finds that the concentration is 205 ppm. What is the concentration
of lead ions in her lake in moles per litre (Molarity)? (5)
(39) Write dissociation equations for each of the following compounds (5)
a. Na2SO4 (s) →
b. C6H6 (s) →
c. Al2(SO3)3 (s) →
d. NH4Cl (s) →
e. NH3 (s) 
(40) Use the following reaction to answer this question:
Na2CO3
+
AlBr3

NaBr
+
Al2(CO3)3
(a) Determine the solubility of the above substances (2)
(b) If [Na2CO3] = 0.150 M and [AlBr3] = 0.250 M, find the mass of precipitate if the volume of
both solutions is 300 mL. (10)
Chemistry 2202 Midyear Exam
January 2004
Page 6
Initials: __________
(41) Use the following reaction that occurs at STP to answer the following question:
S8 (s)
+
Cl2 (g)

S5Cl6 (s)
What mass of pentasulphur hexachloride is produced if 25.5 L of chlorine gas reacts with 200.0 g
of sulphur? (10)
(42) Find the formula of a compound that is 27.2% N, 3.9% H and 68.9% Cl if the compound
has a molar mass of 154.44 g/mol (8)
Chemistry 2202 Midyear Exam
January 2004
Page 7
Initials: __________
Multiple Choice Answer Sheet
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