Chapter 4 2 Calcium oxide reacts with water in a combination reaction to

21) If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to

produce 15.0 g of CO2 according to the following chemical equation?

C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)

A) 6.19 mL

B) 9.95 mL

C) 19.9 mL

D) 39.8 mL

22) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:

2Mg(s) + O2(g) → 2MgO(s)

When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.

A) 4.00

B) 6.63

C) 0.165

D) 3.32

E) 13.3

23) If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to

produce 32.0 g of O2?

2 KClO3(s) → 2 KCl(s) + 3 O2(g)

A) 53.1 g

B) 81.7 g

C) 126 g

D) 283 g

24) If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in the

reaction, how many grams of nitric acid, HNO3(aq) are produced?

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

A) 30.8 g

B) 41.1 g

C) 54.8 g

D) 69.3 g

25) Determine the theoretical yield of H2S (in moles) if 64 mol Al2S3 and 64 mol H2O are reacted

according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol.

Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)

A) 192 mol H2S

B) 64 mol H2S

C) 128 mol H2S

D) 96 mol H2S

E) 32 mol H2S

26) Lithium and nitrogen react in a combination reaction to produce lithium nitride:

6Li(s) + N2(g) → 2Li3N(s)

In a particular experiment, 3.50-g samples of each reagent are reacted. The theoretical yield of lithium

nitride is ________ g.

A) 3.52

B) 2.93

C) 17.6

D) 5.85

E) 8.7

27) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:

CaO(s) + H2O(l) → Ca(OH)2(s)

A 4.50-g sample of CaO is reacted with 4.34 g of H2O. How many grams of water remain after the

reaction is complete?

A) 0.00

B) 0.00892

C) 2.90

D) 1.04

E) 0.161

28) If 294 grams of FeS2 is allowed to react with 176 grams of O2 according to the following

unbalanced equation, how many grams of Fe2O3 are produced?

FeS2 + O2 → Fe2O3 + SO2

29) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:

CaO(s) + H2O(l) → Ca(OH)2(s)

In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)2

is recovered. What is the percent yield in this experiment?

A) 122

B) 1.22

C) 7.19

D) 92.5

E) 81.9

30) Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react

with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was

involved in the reaction?

A) 4.68 g

B) 5.98 g

C) 10.14 g

D) 10.66 g

31) Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g

of sodium hydroxide according to the following chemical equation

:

2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na2SO4(aq) + 2 H2O(l)

A) S(s)

B) O2(g)

C) NaOH(aq)

D) None of these substances is the limiting reactant.

32) When 7.00 × 1022 molecules of ammonia react with 6.00 × 1022 molecules of oxygen according to

the chemical equation shown below, how many grams of nitrogen gas are produced?

4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g)

A) 1.63 g

B) 1.86 g

C) 4.19 g

D) 6.51 g

33) When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How

many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium

chloride?

A) 8.44 g

B) 9.40 g

C) 11.9 g

D) 18.8 g

34) When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced.

Using the following balanced equation, calculate the percent yield for the reaction?

Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g)

A) 12.3%

B) 24.6%

C) 45.5%

D) 84.0%

35) 7.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical

equation shown below. Which one of the following statements is false?

N2(g) + 3 H2(g) → 2 NH3(g)

A) 3.5 g of hydrogen are left over.

B) Hydrogen is the excess reactant.

C) Nitrogen is the limiting reactant.

D) The theoretical yield of ammonia is 15 g.

36) 5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below. Which

one of the following statements is false?

3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g)

A) 6.91 g of Fe3O4 are produced.

B) 2.85 g of H2O are left over.

C) Mass is conserved in this reaction.

D) Water is the limiting reactant.

37) Which of the following solutions will have the highest concentration of chloride ions?

A) 0.10 M LiCl

B) 0.10 M MgCl2

C) 0.10 M AlCl3

D) 0.05 M CaCl2

E) All of these solutions have the same concentration of chloride ions.

38) Which of the following solutions will have the highest concentration of chloride ions?

A) 0.20 M LiCl

B) 0.40 M MgCl2

C) 0.60 M AlCl3

D) 0.40 M CaCl2

E) All of these solutions have the same concentration of chloride ions.

39) How many milliliters of a 0.184 M CsNO3 solution contain 0.113 moles of CsNO3?

A) 543 mL

B) 163 mL

C) 614 mL

D) 885 mL

E) 326 mL

40) How many moles of CH3CH2F are contained in 548 mL of 0.0788 M CH3CH2F solution?

A) 4.32 × 10-2 mol

B) 2.32 × 10-2 mol

C) 6.95 × 10-2 mol

D) 1.44 × 10-2 mol

E) 5.26 × 10-2 mol

41) How many milliliters of a 0.266 M NaNO3 solution are required to make 150.0 mL of 0.075 M

NaNO3 solution?

A) 53.2 mL

B) 42.3 mL

C) 18.8 mL

D) 23.6 mL

E) 35.1 mL

42) What volume (in mL) of 0.0887 M MgI2 solution is needed to make 275.0 mL of 0.0224 M MgI2

solution?

A) 72.3 mL

B) 91.8 mL

C) 10.9 mL

D) 69.4 mL

E) 14.4 mL

43) How many liters of a 0.0550 M NaBr solution contain 0.163 moles of NaBr?

A) 3.37 L

B) 1.48 L

C) 8.97 L

D) 2.96 L

E) 1.12 L

44) How many moles of LiF are contained in 258.6 mL of 0.0296 M LiF solution?

A) 1.31 × 10-3 mol

B) 8.74 × 10-3 mol

C) 1.14 × 10-3 mol

D) 3.67 × 10-3 mol

E) 7.65 × 10-3 mol

45) How many moles of KBr are required to make 250 mL of a 3.00 M solution?

A) 750 moles

B) 0.750 moles

C) 3 moles

D) 0.250 moles

46) What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?

A) 0.125 M

B) 0.0625 M

C) 0.375 M

D) 0.250 M

E) 0.160 M

47) What is the concentration of magnesium ions in a 0.125 M MgBr2 solution?

A) 0.125 M

B) 0.0625 M

C) 0.375 M

D) 0.250 M

E) 0.160 M

48) Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M

Ca(NO3)2 solution to 150.0 mL.

A) 1.13 M

B) 0.0887 M

C) 0.0313 M

D) 0.0199 M

E) 0.0501 M

49) Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M CsCl to 250.0

mL.

A) 0.160 M

B) 0.0320 M

C) 2.50 M

D) 0.00800 M

E) 0.0160 M

50) Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH.

A) 148

B) 1.68

C) 5.30 ×

D) 5.30

E) 1.68 × 10-3

51) How many grams of NaCl are required to make 500.0 mL of a 1.500 M solution?

A) 58.40 g

B) 175.3 g

C) 14.60 g

D) 43.83 g

52) What is the concentration of FeCl3 in a solution prepared by dissolving 20.0 g of FeCl3 in enough

water to make 275 mL of solution?

A) 4.48 × 10-4 M

B) 0.448 M

C) 2.23 M

D) 2.23 × 103 M

53) How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 M?

A) 0.0917 g

B) 0.174 g

C) 5.73 g

D) 91.7 g

54) What volume of a 0.540 M NaOH solution contains 11.5 g of NaOH?

A) 0.155 L

B) 0.532 L

C) 1.88 L

D) 6.44 L

55) What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na3P solution?

56) What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in

sufficient water to give exactly 230 mL of solution?

57) How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?

58) What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient

water to give 425 mL of solution?

59) How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

60) How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M

CH3OH?

61) What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted

with pure water to a total volume of 0.15 L?

A) 2.8 × 10-2 M

B) 5.2 M

C) 28 M

D) 5.2 × 103 M

62) How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.35 L of a 3.5 M solution?

A) 0.14 mL

B) 0.90 mL

C) 140 mL

D) 900 mL

63) A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL

of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water

to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution?

A) 0.274 M

B) 0.356 M

C) 2.81 M

D) 3.65 M

64) How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of

0.500 M HNO3?

A) 0.0444

B) 22.5

C) 2.78

D) 44.4

E) 0.0225

65) A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the

stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is

________ M.

A) 0.270

B) 1.48

C) 0.675

D) 675

E) 270

66) A FeCl3 solution is 0.175 M. How many mL of a 0.175 M FeCl3 solution are needed to make 450.

mL of a solution that is 0.300 M in Cl– ion?

A) 0.771 mL

B) 257 mL

C) 771 mL

D) It is not possible to make a more concentrated solution from a less concentrated solution.

67) Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of

a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give

500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL.

A) 1.26 × 103 M

B) 21.0 M

C) 0.0210 M

D) 0.350 M

E) 3.50 × 10-4 M

68) What is the concentration of NO3– ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in

enough water to produce 300. mL of solution?

A) 0.254 M

B) 0.508 M

C) 0.672 M

D) 1.02 M

69) If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a

solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution?

A) 0.0101 M

B) 0.0404 M

C) 0.162 M

D) 0.323 M

70) What is the concentration of an AlCl3 solution if 150. mL of the solution contains 450. mg of Cl–

ion?

A) 2.82 × 10-2 M

B) 6.75 × 10-2 M

C) 8.46 × 10-2 M

D) 2.54 × 10-1 M

71) How many fluoride ions are present in 65.5 mL of 0.210 M AlF3 solution?

A) 4.02 × 1023 fluoride ions

B) 5.79 × 1024 fluoride ions

C) 2.48 × 1022 fluoride ions

D) 8.28 × 1021 fluoride ions

E) 1.21 × 1022 fluoride ions

72) How many aluminum ions are present in 65.5 mL of 0.210 M AlF3 solution?

A) 4.02 × 1023 aluminum ions

B) 5.79 × 1024 aluminum ions

C) 2.48 × 1022 aluminum ions

D) 8.28 × 1021 aluminum ions

E) 1.21 × 1022 aluminum ions

32

73) How many ions are present in 30.0 mL of 0.600 M K2CO3 solution?

A) 3.25 × 1022 ions

B) 2.17 × 1022 ions

C) 1.08 × 1022 ions

D) 5.42 × 1022 ions

E) 3.61 × 1021 ions

74) How many lithium ions are present in 30.0 mL of 0.600 M Li2CO3 solution?

A) 3.25 × 1022 ions

B) 2.17 × 1022 ions

C) 1.08 × 1022 ions

D) 5.42 × 1022 ions

E) 3.61 × 1021 ions

75) How many carbonate ions are present in 30.0 mL of 0.600 M K2CO3 solution?

A) 3.25 × 1022 ions

B) 2.17 × 1022 ions

C) 1.08 × 1022 ions

D) 5.42 × 1022 ions

E) 3.61 × 1021 ions

76) A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He

took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution.

How many grams of NO3– ion are there in the final solution?

A) 0.0197 g

B) 0.0394 g

C) 0.0542 g

D) 0.108 g

77) There are ________ mol of bromide ions in 0.900 L of a 0.500M solution of AlBr3.

78) How many moles of Co2+ are present in 0.150 L of a 0.200 M solution of CoI2?

33

79) What is the molar concentration of sodium ions in a 0.450 M Na3PO4 solution?

A) 0.150 M

B) 0.450 M

C) 1.35 M

D) 1.80 M

80) Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M

solution of sodium sulfide to a total volume of 300 mL.

81) Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas

produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen

monoxide at 25°C is 1.23 g/L.

_____ NH3(g) + _____ O2(g) →______ NO(g) + _____ H2O(l)

A) 7.32 L

B) 11.1 L

C) 11.5 L

D) 17.3 L

82) How many milliliters of 0.260 M Na2S are needed to react with 40.00 mL of 0.315 M AgNO3?

Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s)

A) 24.2 mL

B) 48.5 mL

C) 66.0 mL

D) 96.9 mL

83) How many grams of CaCl2 are formed when 15.00 mL of 0.00237 M Ca(OH)2 reacts with excess

Cl2 gas?

2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l)

A) 0.00197 g

B) 0.00394 g

C) 0.00789 g

D) 0.0507 g

84) When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of

AgCl are formed?

AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq)

A) 1.07 g

B) 2.24 g

C) 3.31 g

D) 6.44 g

85) How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 1.38

g of Fe2S3 if the percent yield for the reaction is 65.0%?

3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq)

A) 25.5 mL

B) 43.1 mL

C) 51.1 mL

D) 102 mL

86) If 100. mL of 0.400 M Na2SO4 is added to 200. mL of 0.600 M NaCl, what is the concentration of

Na+ ions in the final solution? Assume that the volumes are additive.

A) 0.534 M

B) 0.667 M

C) 1.00 M

D) 1.40 M

87) How many milliliters of 0.550 M hydriodic acid are needed to react with 15.00 mL of 0.217 M

CsOH?

HI(aq) + CsOH(aq) → CsI(aq) + H2O(l)

A) 0.0263 mL

B) 0.169 mL

C) 5.92 mL

D) 38.0 mL

88) Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M

phosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide.

_____ Ca(OH)2(aq) + _____ H3PO4(aq) → _____ Ca3(PO4)2(aq) + _____ H2O(l)

A) 3.04 mL

B) 15.0 mL

C) 22.5 mL

D) 33.8 mL

89) According to the balanced equation shown below, 4.00 moles of oxalic acid, H2C2O4, reacts with

________ moles of permanganate, MnO4–.

5 H2C2O4(aq) + 2 MnO4–(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l)

A) 1.60

B) 4.00

C) 8.00

D) 9.00

90) Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is

needed to completely react with 24.88 mL of 0.125 M KI3(aq), according to the following chemical

equation.

2 S2O32-(aq) + I3–(aq) → S4O62-(aq) + 3 I–(aq)

A) 6.22 mL

B) 12.4 mL

C) 24.9 mL

D) 99.5 mL