Ch.2 Driessen Measurements in Chemistry Exam Prep - MCQ Test Bank | Introductory Chemistry - 2nd Edition by Burdge and Driessen by Julia Burdge, Michelle Driessen. DOCX document preview.
Student name:__________
MULTIPLE CHOICE - Choose the one alternative that best completes the statement or answers the question.
1)
Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp and textiles). |
SO2(g) + 2Cl2(g) → SOCl2(g) + Cl2O(g) |
If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed? |
A) 0.800 mol
B) 0.400 mol
C) 0.200 mol
D) 0.100 mol
E) 0.0500 mol
2)
Aluminum reacts with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). |
Al(s) + Br2(l) → Al2Br6(s) [unbalanced] |
How many moles of Al are needed to form 2.43 mol of Al2Br6? |
A) 7.29 mol
B) 4.86 mol
C) 2.43 mol
D) 1.62 mol
E) 1.22 mol
3)
Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of aluminum, in uranium processing, and in the frosting of light bulbs). |
2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g) |
How many moles of NH3 are needed to react completely with 13.6 mol of F2? |
A) 34.0 mol
B) 27.2 mol
C) 6.80 mol
D) 5.44 mol
E) 2.27 mol
4) What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?
A) 3.26 g
B) 0.629 g
C) 13.04 g
D) 17.63 g
E) 6.52 g
5) What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?
A) 25.8 g
B) 12.9 g
C) 78.2 g
D) 38.7 g
E) 77.4 g
6) What mass of nitrogen gas is required to react completely with excess hydrogen gas to produce 13.6 g of ammonia?
A) 11.2 g
B) 0.06 g
C) 22.4 g
D) 16.5 g
E) 44.8 g
7) What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?
A) 28.1 g
B) 14.04 g
C) 4.96 g
D) 7.02 g
E) 400.0 g
8) How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to produce lead(II) chloride and nitric acid?
A) 5.82 g
B) 14.33 g
C) 0.086 g
D) 11.64 g
E) 16.52 g
9) How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?
A) 8.62 g
B) 34.5 g
C) 4.31 g
D) 40.1 g
E) 17.2 g
10) What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?
A) 12.8 g
B) 25.6 g
C) 6.39 g
D) 0.399 g
E) 51.1 g
11)
What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? |
3SCl2(l) + 4NaF(s) → SF4(g) + S2Cl2(l) + 4NaCl(s) |
A) 1.94 kg
B) 1.51 kg
C) 754 g
D) 205 g
E) 51.3 g
12) Phosphine, an extremely poisonous and highly reactive gas, reacts with oxygen gas to form tetraphosphorus decaoxide and water.
PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced]
Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.
A) 1880 g
B) 940. g
C) 900. g
D) 470. g
E) 56.3 g
13) Potassium chlorate (used in fireworks, flares, and safety matches) forms oxygen and potassium chloride when heated.
KClO3(s) → KCl(s) + O2(g) [unbalanced]
What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?
A) 223 g
B) 99.1 g
C) 10.3 g
D) 6.86 g
E) 4.60 g
14) Aluminum metal reacts with chlorine gas to form solid aluminum trichloride. What mass of chlorine gas is required to react completely with 163 g of aluminum?
A) 214 g
B) 286 g
C) 321 g
D) 428 g
E) 643 g
15) Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?
A) 151 g
B) 123 g
C) 50.3 g
D) 37.7 g
E) 9.41 g
16) How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?
A) 90. g
B) 36 g
C) 42 g
D) 45 g
E) 108 g
17)
What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole of calcium based on the following chemical equation? |
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s) |
A) 1.0 mol
B) 1.6 mol
C) 2.0 mol
D) 2.4 mol
E) 4.0 mol
18)
What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V2O5 with 4.0 moles of calcium based on the following chemical equation? |
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s) |
A) 1.0 mol
B) 1.6 mol
C) 2.0 mol
D) 0.80 mol
E) 3.2 mol
19)
How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? |
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O |
A) 6.52 g
B) 7.29 g
C) 13.0 g
D) 14.6 g
E) 58.4 g
20)
Hydrochloric acid can be prepared by the following reaction: |
2NaCl(s) + H2SO4(aq) → 2HCl(g) + Na2SO4(s) |
What mass of HCl can be prepared from 2.00 mol H2SO4 and 150. g NaCl? |
A) 2.57 g
B) 46.8 g
C) 93.6g
D) 146 g
E) 167g
21)
What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S8? |
8Fe(s) + S8(s) → 8FeS(s) |
A) 186 g
B) 142 g
C) 119 g
D) 14.8 g
E) 0.169 g
22)
What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? |
2SO2 + O2 → 2SO3 |
A) 10.0 g
B) 12.5 g
C) 22.5 g
D) 55.0 g
E) 77.5 g
23)
What is the maximum number of grams of ammonia, NH3, that can be obtained from the reaction of 10.0 g of H2 and 80.0 g of N2? |
N2 + 3H2 → 2NH3 |
A) 34.1 g
B) 48.6 g
C) 56.3 g
D) 90.0 g
E) 97.3 g
24)
What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following chemical equation? |
2Al + Cr2O3 → Al2O3 + 2Cr |
A) 15.1 g
B) 30.2 g
C) 67.4 g
D) 99.9g
E) 104 g
25) If 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia, what is the limiting reactant and what mass of ammonia is produced?
A) Hydrogen is the limiting reactant and 0.22 g of ammonia are produced.
B) Nitrogen is the limiting reactant and 2.07 g of ammonia are produced.
C) Nitrogen is the limiting reactant and 4.15 g of ammonia are produced.
D) Hydrogen is the limiting reactant and 23.5 g of ammonia are produced.
E) Hydrogen is the limiting reactant and 15.8 g of ammonia are produced.
26) If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?
A) Calcium is the limiting reactant and 47.2 g of calcium oxide are produced.
B) Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced.
C) Calcium is the limiting reactant and 48.7 g of calcium oxide are produced.
D) Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced.
E) Calcium is the limiting reactant and 23.6 g of calcium oxide are produced.
27) If 31.3 g of manganese(II) chloride, 48.3 g of chlorine gas, and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid, what is the limiting reactant and what mass of hydrochloric acid is produced?
A) manganese(II) chloride is the limiting reactant and 9.07 g of hydrochloric acid is produced.
B) chlorine is the limiting reactant and 99.3 g of hydrochloric acid is produced.
C) chlorine is the limiting reactant and 24.8 g of hydrochloric acid is produced.
D) manganese(II) chloride is the limiting reactant and 36.3 g of hydrochloric acid is produced.
E) water is the limiting reactant and 52.0 g of hydrochloric acid is produced.
28) Aluminum reacts with oxygen to produce aluminum oxide, which can be used as an adsorbent, desiccant, or catalyst for organic reactions. A mixture of 82.49 g of aluminum and 117.65 g of oxygen is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.
A) Oxygen is the limiting reactant; 19.81 g of aluminum remain.
B) Oxygen is the limiting reactant; 35.16 g of aluminum remain.
C) Aluminum is the limiting reactant; 16.70 g of oxygen remain.
D) Aluminum is the limiting reactant; 35.16 g of oxygen remain.
E) Aluminum is the limiting reactant; 44.27 g of oxygen remain.
29) Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron. A mixture of 41.0 g of magnesium and 175.0 g of iron(III) chloride is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.
A) Limiting reactant is Mg; 7.4 g of FeCl3 remain.
B) Limiting reactant is Mg; 46.5 g of FeCl3 remain.
C) Limiting reactant is FeCl3; 1.7 g of Mg remain.
D) Limiting reactant is FeCl3; 37.8 g of Mg remain.
E) Limiting reactant is Mg; 134.0 g of FeCl3 remain.
30) Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.
A) Chlorine is the limiting reactant; 1.14 g of potassium remain.
B) Potassium is the limiting reactant; 2.00 g of chlorine remain.
C) Potassium is the limiting reactant; 2.47 g of chlorine remain.
D) Chlorine is the limiting reactant; 3.07 g of potassium remain.
E) Potassium is the limiting reactant; 4.50 g of chlorine remain.
31) Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction?
A) 57.5%
B) 48.8%
C) 38.0%
D) 89.4%
E) 16.3%
32)
If 119.3 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3, what is the percent yield? |
PCl3(g) + Cl2(g) → PCl5(g) |
A) 94.6%
B) 66.3%
C) 57.3%
D) 51.3%
E) 48.6%
33)
Methanol (CH3OH) is converted to bromomethane (CH3Br) as follows: |
CH3OH + HBr → CH3Br + H2O |
If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield? |
A) 12.9%
B) 33.8%
C) 40.9%
D) 59.1%
E) 82.6%
34)
The first step in the Ostwald process for producing nitric acid is as follows: |
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g). |
If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction? |
A) 29.0%
B) 32.9%
C) 49.5%
D) 61.8%
E) 77.3%
35)
One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na3(CO3)(HCO3)·2H2O. |
2Na3(CO3)(HCO3)·2H2O(s) → 3Na2CO3(s) + CO2(g) + 5H2O(g) |
When 1.00 metric ton (1.00 × 103 kg) of trona is decomposed, 0.650 metric ton of Na2CO3 is recovered. What is the percent yield of this reaction? |
A) 92.4%
B) 72.1%
C) 65.0%
D) 48.1%
E) 35.0%
36)
What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below? |
2Al + Cr2O3 → Al2O3 + 2Cr |
A) 7.7 g
B) 15.4 g
C) 27.4 g
D) 30.8 g
E) 49.9 g
37)
Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: |
4NH3 + 5O2 → 4NO + 6H2O |
What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react? |
A) 1.56mol
B) 1.88 mol
C) 3.52 mol
D) 3.91 mol
E) 2.35 mol
38)
What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium based on the following chemical equation? |
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s) |
A) 11.2 g
B) 5.6 g
C) 22.4 g
D) 40.0 g
E) 20.3 g
39)
What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? |
Al2O3 + 3C → 2Al + 3CO |
A) 15.9 g
B) 31.8 g
C) 44.9 g
D) 63.6 g
E) 67.4 g
40) Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO3)2 solution.2KI(aq) + Pb(NO3)2(aq) → PbI2(s) + 2KNO3(aq)
A) 5.19 g
B) 2.59 g
C) 12.0 g
D) 3.48 g
E) 9.55 g
41) What volume of 0.233 M H2SO4 is needed to react exactly with 15.0 grams of aluminum?2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
A) 2.39 L
B) 0.556 L
C) 0.864 L
D) 4.22 L
E) 3.58 L
42) What mass of precipitate forms when 25.0 mL of 0.147 M NiCl2 solution reacts with excess sodium phosphate according to the given balanced chemical equation.3NiCl2(aq) + 2Na3PO4(aq) → Ni3(PO4)2(s) + 6NaCl(aq)
A) 0.149 g
B) 0.448 g
C) 1.35 g
D) 0.368 g
E) 0.234 g
43) How many milliliters of 0.0150 M KOH are required to react exactly with 75.0 mL of 0.0150 M H3PO4?H3PO4(aq) + 3KOH(aq) → K3PO4(aq) + 3H2O(l)
A) 25.0 mL
B) 1000 mL
C) 225 mL
D) 250 mL
E) 75.0 mL
44) What volume of 0.200 M H2SO4 solution is required to react exactly with 50.0 mL of 0.100 M KOH?H2SO4(aq) + 2KOH(aq) → 2H2O(l) + K2SO4(aq)
A) 62.5 mL
B) 12.5 mL
C) 50.0 mL
D) 25.0 mL
E) 75.0 mL
45) What volume of 0.307 M K2SO4 solution is required to react exactly with 85.0 mL of 0.100 M AgNO3?K2SO4(aq) + 2AgNO3(aq) → 2KNO3(aq) + Ag2SO4(s)
A) 52.2 mL
B) 26.1 mL
C) 55.4 mL
D) 27.7 mL
E) 13.8 mL
46) Given the following reaction, how much AgCl (in g) can be formed from 25.0 mL of 0.115 M AgNO3 and 45.0 mL of 0.0533 M MgCl2?2AgNO3(aq) + MgCl2(aq) →2AgCl(s) + Mg(NO3)2(aq)
A) 0.344 g
B) 0.688 g
C) 1.10 g
D) 0.412 g
E) 0.276 g
47)
Zinc dissolves in hydrochloric acid to yield hydrogen gas as follows: |
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) |
What mass of hydrogen gas is produced when a 7.35-g sample of zinc dissolves in 500.mL of 1.200 M HCl? |
A) 0.605 g
B) 0.113 g
C) 0.302 g
D) 0.453 g
E) 0.227 g
48)
What is the volume of NH3 produced in the following reaction when 3.0 L of N2 reacts with 4.0 L of H2 ? |
N2(g) + 3H2(g) → 2NH3(g) |
A) 1.5 L
B) 2.7 L
C) 6.0 L
D) 7.5 L
E) 12 L
49)
What volume of CO2 gas at 645 torr and 800. K could be produced by the decomposition of 45.0 g of CaCO3? |
CaCO3(s) → CaO(s) + CO2(g) |
(R = 0.08206 L • atm/K • mol) |
A) 0.449 L
B) 22.4 L
C) 25.0 L
D) 34.8 L
E) 45.7 mL
50)
What volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 in excess HCl(aq)? |
MnO2(s) + 4HCl(aq) → MnCl2(aq) + 2H2O(l) + Cl2(g) |
(R = 0.08206 L • atm/K • mol) |
A) 5.36 × 10−3 L
B) 0.138 L
C) 0.282 L
D) 3.09 L
E) 3.55 L
51)
Magnesium metal (0.100 mol) and hydrochloric acid (0.500 mol HCl) are combined and react to completion. What volume of hydrogen gas, measured at STP, is produced? |
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) |
(R = 0.08206 L • atm/K • mol) |
A) 2.24 L of H 2
B) 4.48 L of H 2
C) 5.60 L of H 2
D) 11.2 L of H 2
E) 22.4 L of H 2
52)
When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. |
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) |
(R = 0.08206 L • atm/K • mol) |
A) 3.4 × 10−3 L
B) 2.2 L
C) 2.9 L
D) 5.8 L
E) 11.7 L
53)
Calculate the volume of H2(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with 50.0 g Zn(s) to give hydrogen gas and aqueous zinc chloride. |
(R = 0.08206 L • atm/K • mol) |
A) 0.56 L
B) 1.12 L
C) 2.23 L
D) 4.47 L
E) 3.54 L
54)
What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) |
(R = 0.08206 L • atm/K • mol) |
A) 24.6 g
B) 70.8 g
C) 272 g
D) 408 g
E) 612 g
55)
Consider the following reaction. |
H2(g) + I2(s) → 2 HI(g) |
If the cylinder with a movable piston below contains 1 mol H2(g) and 1 mol I2(s), which represents the cylinder after the reaction is complete? |
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A)
B)
C)
D)
E) None of the answers is correct.
56) Given that CaO(s) + H2O(l) → Ca(OH)2(s),heat of reaction = −64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?
A) 6.92 g
B) 56.1 g
C) 454 g
D) 606 g
E) 3.40 × 104 g
57) The combustion of pentane produces heat according to the following thermochemical equation.
C5H12(l) + 8O2(g) → 5CO2(g) + 6H2O(l) heat of reaction = −3510 kJ/mol
How many grams of CO2 is produced per 2.50 × 103 kJ of heat released?
A) 6.27 g
B) 31.3 g
C) 61.8 g
D) 157 g
E) 220 g
58) How much heat is evolved if 0.600 kg of SO2 is burned in excess oxygen?
2SO2(g) + O2(g) → 2SO3(g) heat of reaction = −198 kJ/mol
A) 5.46 × 10−2 kJ
B) 927 kJ
C) 1.85 × 103 kJ
D) 59,400 kJ
E) 3.71 × 103 kJ
59) How much heat is released if 35.0 g of ethanol (C2H5OH) burns in excess oxygen?
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) heat of reaction = −1367 kJ/mol
A) 1797 kJ
B) 1367 kJ
C) 9.61 × 10−4 kJ
D) 4.78 × 104 kJ
E) 1040 kJ
60) How much heat is released if 7.15 g CaO(s) is added to 152 g of H2O(l)?
CaO(s) + H2O(l) → Ca(OH)2(s) heat of reaction = −64.8 kJ/mol
A) 7.68 kJ
B) 8.26 kJ
C) 508 kJ
D) 547 kJ
E) 555 kJ
61) The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together.
2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) heat of reaction = −847.6 kJ/mol |
What mass of iron is formed if 725 kJ of heat are released? |
A) 23.9 g
B) 47.8 g
C) 65.3 g
D) 95.5 g
E) 112 g
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MCQ Test Bank | Introductory Chemistry - 2nd Edition by Burdge and Driessen
By Julia Burdge, Michelle Driessen