Ch8 Chemical Equations – Test Bank | Practice Set – 15e - Test Bank | Foundations of College Chemistry 15e by Hein Arena by Hein Arena, Willard. DOCX document preview.
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Package Title: Hein Test Bank
Course Title: Hein 15e
Chapter Number: 8
Question type: Multiple Choice
1) Given the unbalanced equation: Al + CuSO4 → Al2(SO4)3 + Cu. When properly balanced, the sum of the balancing coefficients is
a) 6.
b) 7.
c) 8.
d) 9.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
2) Given the unbalanced equation: H2O2 → H2O + O2. When properly balanced, the sum of the balancing coefficients is
a) 4.
b) 5.
c) 6.
d) 7.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
3) The reaction of glucose, C6H12O6, with oxygen produces carbon dioxide and water. What is the sum of the coefficients in the balanced equation?
a) 19
b) 17
c) 12
d) 6
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
4) Given the unbalanced equation: C2H2 + O2 → CO2 + H2O. When properly balanced, the sum of the balancing coefficients is
a) 10.
b) 11.
c) 12.
d) 13.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
5) Given the unbalanced equation: C2H4 + O2 → CO2 + H2O. When properly balanced, the balancing coefficient of C2H4 is
a) 0.
b) 1.
c) 2.
d) 3.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
6) Given the unbalanced equation: Al + CuO → Al2O3 + Cu. When properly balanced, the balancing coefficient of Al2O3 is
a) 3.
b) 2.
c) 1.
d) 0.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
7) Given the unbalanced equation: KClO3 → KCl + O2. When properly balanced, the sum of the balancing coefficients is
a) 6.
b) 7.
c) 8.
d) 9.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
8) Given the unbalanced equation: PbCl2 + Na2Cr2O7 → PbCr2O7 + NaCl. When properly balanced, the sum of the balancing coefficients is
a) 2.
b) 3.
c) 4.
d) 5.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
9) Given the unbalanced equation: AgNO3 + CaCl2 → AgCl + Ca(NO3)2. When properly balanced, the sum of the balancing coefficients is
a) 4.
b) 5.
c) 6.
d) 7.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
10) Given the unbalanced equation: C6H6 + O2 🡪 H2O + CO2. When properly balanced, the coefficient of oxygen is
a) 1.
b) 9.
c) 12.
d) 15
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
11) Given the unbalanced equation: magnesium and silver nitrate producing magnesium nitrate and silver. When properly balanced, the sum of the balancing coefficients is
a) 4.
b) 6.
c) 8.
d) 10.
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
12) Nitrogen gas combines with oxygen gas to form dinitrogenpentoxide. When properly balanced, the sum of the balancing coefficients is
a) 5.
b) 6.
c) 7.
d) 9.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
13) Given the unbalanced equation: Zn + HCl → ZnCl2 + H2. When properly balanced, the sum of the balancing coefficients is
a) 4.
b) 5.
c) 6.
d) 7.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
14) Given the unbalanced equation: Na + H2O 🡪 NaOH + H2.When properly balanced, the sum of the balancing coefficients is:
a) 4.
b) 5.
c) 6.
d) 7.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
15) Given the unbalanced reaction: NH3 + O2 🡪 N2 + H2O. When properly balanced, the sum of the balancing coefficients is
a) 8.
b) 12.
c) 15.
d) 14.
Difficulty: Medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
16) The following reaction: Mg + FeO → MgO + Fe, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
17) The following reaction: CH4 + 2O2 → CO2 + H2O, is an example of
a) combustion
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
18) The following reaction: LiOH + HCl → LiCl + H2O, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
19) The following reaction: Na2O + 2HCl → 2NaCl + H2O, is an example of
a) synthesis.
b) combustion.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
20) The following reaction: K + NaBr → KBr + Na, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
21) The following reaction: Cl2 + KBr → KCl + Br2, is an example of
a) synthesis.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
22) The following reaction: calcium carbonate producing calcium oxide and carbon dioxide, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
23) The following reaction: Na2CO3 + CaCl2 → 2NaCl + CaCO3, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
24) The following reaction: C + O2 → CO2, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
25) The following reaction: F2 + 2KBr→ 2KF + Br2, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
26) The following reaction: H2 + I2 → 2HI, is an example of
a) synthesis.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a synthesis reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
27) The following reaction: Ca + 2H2O → Ca(OH)2 + H2, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
28) The following reaction: NaCl + AgNO3 → AgCl + NaNO3, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
29) The following reaction: hydrogen and oxygen producing water, is an example of
a) synthesis.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: medium
Learning Objective 1: Give examples of a synthesis reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
30) The following reaction: 2FeO → 2Fe + O2, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
31) Which shows a balanced chemical equation for the decomposition of aluminum oxide?
a) Al2O3 → 2Al + O2
b) Al2O3 → 2Al + 3O2
c) 2Al2O3 → 4Al + 3O2
d) 4Al + 3O2 → 2Al2O3
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
32) Which shows a balanced chemical equation for the complete combustion of methane (CH4) gas?
a) CH4 + 2O2 → CO2 + 2H2O
b) CH4 → CO2 + + 2O2 + H2O
c) CO2 + H2O → CH4 + 2O2
d) 2CH4 + 3O2 → 2CO + 4H2O
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
33) The following reaction: potassium chlorate producing potassium chloride and oxygen, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
34) The following reaction: MgCl2 → Mg + Cl2, is an example of
a) combination.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
35) The following reaction: 2Al + 3O2 → Al2O3, is an example of
a) synthesis.
b) decomposition.
c) single-displacement.
d) double-displacement.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
36) The reaction: CH4 + 2O2 → CO2 + 2H2O + 890.4 kJ, is
a) endothermic.
b) exothermic.
c) isothermic.
d) protothermic.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
37) The reaction: N2 + O2 + 182.6 kJ → 2NO, is
a) endothermic.
b) exothermic.
c) isothermic.
d) protothermic.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
38) The reaction: 2C + H2 + 227.4 kJ → C2H2, is
a) endothermic.
b) exothermic.
c) isothermic.
d) protothermic.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
39) The reaction: 2C + 3H2 → C2H6 + 84.0 kJ, is
a) endothermic.
b) exothermic.
c) isothermic.
d) protothermic.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
40) In the expression, 2AlCl3,
a) 2 and 3 are subscripts
b) 2 and 3 are coefficients
c) 2 is a subscript and 3 is a coefficient
d) 3 is a subscript and 2 is a coefficient
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
41) In the expression, 3CaBr2,
a) 2 and 3 are subscripts
b) 2 and 3 are coefficients
c) 2 is a subscript and 3 is a coefficient
d) 3 is a subscript and 2 is a coefficient
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
42) In the following reaction: KOH + CuNO3 → KNO3 + CuOH
a) KOH and KNO3 are reactants
b) KNO3 and CuOH are reactants
c) CuOH and KOH are products
d) KOH and CuNO3 are reactants
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
43) In the following reaction: Ba + MgO → Mg + BaO
a) Mg and BaO are products
b) Mg and MgO are products
c) Ba and MgO are products
d) Ba and Mg are products
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
44) In the reaction: copper(II) sulfate and barium bromide producing copper(II) bromide and barium sulfate
a) BaBr2 and BaSO4 are reactants
b) BaSO4 and CuBr2 are products
c) Cu2SO4 and BaBr are reactants
d) CuSO4 and BaBr2 are products
Difficulty: medium
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
45) Which of the following balanced reactions is the decomposition of potassium chlorate into potassium chloride and oxygen?
a) KClO2 🡪 KCl + O2
b) KClO3 🡪 KCl + O2
c) 2KClO2 🡪 2KCl + 2O2
d) 2KClO3 🡪 2KCl + 3O2
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
46) Natural gas is primarily composed of
a) butane.
b) propane.
c) octane.
d) methane.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
47) The combustion of hydrocarbon fuels is
a) endothermic.
b) exothermic.
c) isothermic.
d) protothermic.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
48) The products of the complete combustion of the hydrocarbon methane are
a) carbon monoxide and water.
b) carbon dioxide and water.
c) carbon monoxide and hydrogen.
d) carbon dioxide and hydrogen.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
49) The products of the complete combustion of the fossil fuel coal are
a) carbon monoxide and water.
b) carbon dioxide and water.
c) carbon monoxide and hydrogen.
d) carbon dioxide and hydrogen.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
50) The reaction: Ba + CuO → BaO + Cu, will occur if
a) Cu is more active than Ba
b) Ba is more active than Cu
c) Ba is more active than O
d) O is more active than Cu
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
51) The driving force for the reaction: 2Na + 2HCl → 2NaCl + H2, is
a) Formation of a solid
b) Formation of a gas
c) Formation of water
d) Formation of salt
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
52) The reaction: Cl2 + 2KBr → 2KCl + Br2, will occur if
a) K is more active than Cl
b) Cl is more active than Br
c) K is more active than Br
d) Br is more active than Cl
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
53) Given the reaction: 4NH3 + 3O2 → 2N2 + 6H2O. How many moles of N2 are produced when 1.0 mol of NH3 is consumed?
a) 0.50 mol
b) 1.0 mol
c) 2.0 mol
d) 4.0 mol
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
54) Given the reaction: 2KClO3 → 2KCl + 3O2. How many moles of O2 are produced when 4.0 mol of KCl are produced?
a) 1.5 mol
b) 3.0 mol
c) 4.5 mol
d) 6.0 mol
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
55) Given the reaction: KOH + CO2 → K2CO3 + H2O. When properly balanced, how many moles of H2O are produced from 2.0 moles of KOH?
a) 0.0 mol
b) 1.0 mol
c) 2.0 mol
d) 3.0 mol
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
56) Given the reaction: Sn + H2SO4 → SnSO4 + SO2 +H2O. When properly balanced, how many moles of H2SO4 are consumed to produce 4.0 moles of H2O?
a) 1.0 mol
b) 2.0 mol
c) 3.0 mol
d) 4.0 mol
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
57) When a metal reacts with hydrochloric acid
a) a hydroxide is produced.
b) a new acid is produced.
c) hydrogen gas is produced.
d) a metal oxide is formed.
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
58) When solutions of an acid and a base are reacted, the products are
a) a new acid and a new base.
b) a salt and water.
c) a metal oxide and water.
d) a nonmetal oxide and water.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
59) A combustion reaction will always involve the release of
a) sound.
b) heat.
c) oxygen gas.
d) steam.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
60) Which of the following statements is not true during a chemical reaction?
a) Total mass is conserved.
b) The total number of atoms is conserved.
c) The total number of molecules is conserved.
d) Energy is involved.
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
61) The reaction of Mg(OH)2 and HBr produces
a) MgOH and HBr.
b) MgH2 and HBrO.
c) H2O and MgBr2.
d) Mg(BrO)2 and MgH.
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
62) The reaction of ZnBr2 and Ba(OH)2 produces
a) ZnO and BaBrH.
b) ZnBa and BrOH.
c) ZnBr2 and Ba(OH)2.
d) BaBr2 and Zn(OH)2.
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
63) Which of the following reactions is exothermic?
a) 2H2O2 🡪 H2O + O2
b) NaOH + HCl 🡪 NaCl + H2O
c) CaCO3 🡪 CaO + CO2
d) 2KClO3 🡪 2KCl + 3O2
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Learning Objective 2: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.2 and 8.3
64) When the equation NH4OH + H2SO4 → (NH4)2SO 4 + H2O is balanced, a term in the balanced equation is
a) 2H2SO4
b) NH4OH
c) 2(NH4)2SO4
d) 2H2O
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
65) When the equation H2 + V2O5 → V + H2O is balanced, a term in the balanced equation is
a) 2V2O5
b) 3H2O
c) 2V
d) 10 H2
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
66) When the equation PbO2 → PbO + O2 is balanced, a term in the balanced equation is
a) PbO2
b) 3O2
c) 3PbO
d) O2
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
67) Consider the reaction: C + O2 → CO2 + 393 kJ. When 2 mol of carbon react
a) 393 kJ of energy is released.
b) 393 kJ of energy is absorbed.
c) 786 kJ of energy is released .
d) 786 kJ of energy is absorbed.
Difficulty: medium
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
68) Consider the reaction: H2 + I2 + 12.6 kJ → 2 HI. Whe1 mol of HI is produced
a) 12.6 kJ of energy is absorbed.
b) 6.3 kJ of energy is absorbed.
c) 12.6 kJ of energy is released.
d) 6.3 kJ of energy is released.
Difficulty: medium
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
69) When the equation Al + O2 → Al2O3 is balanced, a term in the balanced equation is
a) 2Al
b) 2Al2O3
c) 3Al
d) 2O2
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
70) When the equation H2O2 → H2O + O2 is balanced, a term in the balanced equation is
a) H2O2.
b) H2O.
c) 2H2O.
d) 2O2.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
71) Which of the following changes is endothermic?
a) freezing water
b) burning wood
c) condensing water vapor
d) melting ice
Difficulty: medium
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
72) Which of the following changes is exothermic?
a) boiling water
b) melting ice
c) condensing water vapor
d) the reaction inside an ice pack
Difficulty: medium
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
73) When the equation Al(OH)3 + H2SO4 → Al2(SO4)3 + H2O is balanced, the sum of the balancing coefficients is
a) 5.
b) 7.
c) 11.
d) 12.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
74) What type of compound is formed when a nonmetal oxide reacts with water?
a) base
b) acid
c) salt
d) metal oxide
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
75) What type of compound is formed when carbon dioxide reacts with water?
a) base
b) acid
c) salt
d) metal oxide
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
76) What type of compound is formed when a metal oxide reacts with water?
a) base
b) acid
c) salt
d) nonmetal oxide
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
77) What type of compound is formed when a calcium oxide reacts with water?
a) acid
b) base
c) salt
d) nonmetal oxide
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
78) When 2.0 mol of H2 react with 1.0 mol of O2 to produce 2.0 mol of H2O, how many grams of H2O are produced?
a)18.0 g
b) 2.0 g
c) 36 g
d) 1.0 g
Difficulty; medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
79) When the equation CaCO3 → CaO + CO2 is balanced, the coefficient of carbon dioxide is
a) 1.
b) 2.
c) 3.
d) 4.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
80) When the equation NH4Cl + CaO → NH3 + CaCl2 + H2O is balanced, the coefficient of water is
a) 1.
b) 2.
c) 3.
d) 4.
Difficulty: easy
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
81) Reactions which liberate heat are
a) endothermic.
b) exothermic.
c) isothermic.
d) protothermic.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
82) Given the balanced reaction: N2 + O2 🡪 2NO. How many grams of NO are produced from the reaction of 2.0 mol of N2 with 2.0 mol of O2?
a) 30. g
b) 60. g
c) 2.0 g
d) 40. g
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
83) Hydrocarbons are composed of
a) hydrogen, only.
b) carbon, only.
c) hydrogen and carbon.
d) hydrogen, carbon, and oxygen.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
84) The amount of energy that must be supplied to start a chemical reaction is called the
a) heat of reaction.
b) heat of fusion.
c) heat of vaporization.
d) activation energy.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
85) In an endothermic reaction
a) the reactants have greater potential energy than the products.
b) the products have greater potential energy than the reactants.
c) the products and the reactants have the same potential energy.
Difficulty: medium
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
86) In an exothermic reaction
a) the reactants have greater potential energy than the products.
b) the products have greater potential energy than the reactants.
c) the products and the reactants have the same potential energy.
Difficulty: medium
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
87) Balance the following chemical equation using the smallest set of integers. The coefficient on H2O is
I2 + Cl2 + H2O 
HIO3 + HCl
a) 1.
b) 5.
c) 6.
d) 2 .
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
88) Balance the following chemical equation using the smallest set of integers. The coefficient on NO2 is:
HNO3 + S 
NO2 + H2SO4 + H2O
a) 4
b) 6
c) 1
d) 2
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
89) Which of the following reactants would you add to an aqueous solution of ammonium sulfate in order to precipitate quantitatively all the sulfate?
a) CaCl2
b) Al(NO3)3
c) Zn(C2H3O2)2
d) KBr
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
90) Which of the following reactants would you add to an aqueous solution of silver nitrate in order to precipitate quantitatively all the silver?
a) NaNO3
b) NaCl
c) KF
d) H2O
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
91) Which of the following combinations will not form a precipitate?
a) Pb(NO3)2 + NaCl
b) SnCl2 + KOH
c) FeCl2 + (NH4)2S
d) NH4Br + K2SO4
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
92) Which of the following combinations will not form new substances?
a) I2 + KBr
b) Fe + HCl
c) Ag + AuCl3
d) Ca + H2O
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
93) Which of the following combinations will form a precipitate?
a) AgNO3 + KBr
b) FeSO4 + NaI
c) LiBr + (NH4)3PO4
d) NH4Br + K2SO4
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
94) Consider the following incomplete reaction. Choose the formula for the missing substance Y.
4NH3 + 5O2 
4NO + 6 Y
a) O3
b) H2O
c) H2
d) H2O2
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
95) The following incomplete reaction. Choose the formula for the missing substance Y.
Mg + 2 Y 
MgCl2 + H2
a) H2Cl
b) Cl
c) Cl2
d) HCl
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
96) The formula of the salt produced from the neutralization reaction between nitric acid and barium hydroxide is:
a) H2O.
b) NO3OH.
c) Ba(NO3)2.
d) Ba(OH)2.
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
97) The formula for the salt produced from the neutralization reaction between sulfuric acid and sodium hydroxide is:
a) Na2SO4
b) Na2S
c) NaSO4
d) Na2SO3
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
98) Which of the following combinations will result in the formation of an insoluble solid?
a) NH4Br + NaNO3
b) HBr + KOH
c) CrCl2 + K2S
d) KOH + NaCl
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
99) The decomposition of CaCO3 upon heating will form:
a) CaO + CO2
b) CaC2 + O3
c) CaO2 + CO
d) Ca + CO3
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
100) According to the law of conservation of mass, matter can be
a) created.
b) destroyed.
c) created and destroyed.
d) converted from one form to another.
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
101) Which region in the following diagram corresponds to the activation energy for the reaction?
a) A
b) B
c) C
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
102) Which region in the following diagram corresponds to the heat of reaction?
a) A
b) B
c) C
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
Question type: True/False
103) The quantity of heat produced by a reaction is known as activation energy.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
104) In all chemical reactions, atoms are neither created nor destroyed.
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
105) Chemical reactions always produce substances which are different from those started with.
Difficulty: easy
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
106) When acids and bases react they always produce a new acid and a new base.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
107) Magnesium oxide on reaction with water produces acid.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
108) Nitrogen dioxide on reaction with water produces base.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
109) Carbon monoxide is a colorless odorless gas, which can bond to a hemoglobin molecule and inhibit the transport of oxygen in the body.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
110) The fact that copper cannot replace hydrogen means that copper is less active than hydrogen.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
111) Sodium oxide is a basic oxide.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
112) Phosphorus trioxide is an acidic oxide.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
113) A precipitation reaction will occur if one of the products is an insoluble solid.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
114) According to the Greenhouse Effect, rising levels of carbon dioxide, methane, and water vapor in our atmosphere are trapping heat near the surface of the Earth.
Difficulty: easy
Learning Objective 1: Discuss the possible causes and results of the greenhouse effect
Section Reference 1: Section 8.5
115) The Greenhouse Effect is causing global warming.
Difficulty: easy
Learning Objective 1: Discuss the possible causes and results of the greenhouse effect
Section Reference 1: Section 8.5
116) The levels of Greenhouse Gases in our atmosphere have decreased significantly in the past century.
Difficulty: easy
Learning Objective 1: Discuss the possible causes and results of the greenhouse effect
Section Reference 1: Section 8.5
117) A neutralization reaction is a single displacement reaction.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
118) In a neutralization reaction, one of the reactants behaves as an acid and the other behaves as a base.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
119) The products of a neutralization reaction are a salt and water.
Difficulty: easy
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
120) The products of the complete combustion of hydrocarbons are CO and H2O.
Difficulty: easy
Learning Objective 1: Explain the following terms and how they relate to a chemical reaction: exothermic reaction, endothermic reaction, heat of reaction, and activation energy.
Section Reference 1: Section 8.4
Question type: essay
121) Change these word equations into balanced chemical equations.
a) Magnesium plus oxygen yields magnesium oxide.
b) Water decomposes to yield hydrogen and oxygen.
c) Sodium sulfate plus barium chloride yields barium sulfate and sodium chloride.
d) Sodium plus iron(III) nitrate yields sodium nitrate plus iron.
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: a) 2Mg + O2 → 2MgO; b) 2H2O → 2H2 + O2; c) Na2SO4 + BaCl2 → BaSO4 + 2NaCl; d) 3Na + Fe(NO3)3 → 3NaNO3 + Fe
122) Change these word equations into balanced chemical equations.
a) Carbon plus oxygen yields carbon monoxide.
b) Sodium chlorate decomposes to form sodium chloride and oxygen.
c) Phosphoric acid and potassium hydroxide yields potassium phosphate and water.
d) Fluorine and potassium bromide yields potassium fluoride and bromine.
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: a) 2C + O2 → 2CO; b) 2NaClO3 → 2NaCl + 3O2; c) H3PO4 + 3KOH → K3PO4 + 3HOH; d) F2 + 2KBr → 2KF + Br2
123) The following questions refer to a reaction in which sodium and water react to produce sodium hydroxide and hydrogen gas.
a) Write a balanced chemical equation for the reaction.
b) When one mole of hydrogen is produced, how many moles of sodium are consumed?
c) When one mole of hydrogen is produced, how many moles of water are consumed?
d) When one mole of hydrogen is produced, how many moles of sodium hydroxide are produced?
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: a) 2Na + 2H2O → 2NaOH + H2; b) 2 mol of sodium are consumed; c) 2 mol of water are consumed; d) 2 mol of sodium hydroxide are produced
124) The following questions refer to a reaction in which calcium bromide and silver nitrate react to produce calcium nitrate and silver bromide.
a) a balanced chemical equation for the reaction.
b) When one mole of calcium bromide is consumed, how many moles of silver nitrate are consumed?
c) When one mole of calcium bromide is consumed, how many moles of calcium nitrate are produced?
d) When one mole of calcium bromide is consumed, how many moles of silver bromide are?
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: a) CaBr2 + 2AgNO3 → Ca(NO3)2 + 2AgBr; b) 2 mol of silver nitrate are consumed; c) 1 mol of calcium nitrate is produced; d) 2 mol of silver bromide are produced
125) Complete and balance the equation for each example in which a double-displacement reaction will occur. If no reaction will occur write the words “No Reaction” on the right side of the equation.
a) AlBr3 + AgNO3 →
b) ZnBr2 + Na2S →
c) NH4Br + AlI3 →
d) K2CO3 + HCl →
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
Solution: a) AlBr3 + 3AgNO3 → Al(NO3)3 + 3AgBr; b) ZnBr2 + Na2S → 2NaBr + ZnS; c) NH4Br + AlI3 → No Reaction; d) K2CO3 + 2HCl → 2KCl + H2O + CO2
126) Complete and balance the equation for each example in which a double-displacement reaction will occur. If no reaction will occur write the words “No Reaction” on the right side of the equation.
a) HF + KOH →
b) AgNO3 + KCl →
c) KOH + ZnCl2 →
d) NH4Cl + Ca(NO3)2 →
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
Solution: a) HF + KOH → KF + H2O; b) AgNO3 + KCl → KNO3 + AgCl; c) 2KOH + ZnCl2 → 2KCl + Zn(OH)2; d) NH4Cl + Ca(NO3)2 → No Reaction
127) Complete and balance the equation for each example in which a single-displacement reaction will occur. If no reaction will occur write the words “No Reaction” on the right side of the equation. Use this activity series:
More Active K
Mg
Al
H
Cu
Less Active Ag
a) Al + HCl →
b) Ag + HNO3 →
c) Al + KBr →
d) Mg + CuCl2
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
Solution: a) 2Al + 6HCl → 2AlCl3 + 3H2; b) Ag + HNO3 → No Reaction; c) Al + KBr → No Reaction; d) Mg + CuCl2 → MgCl2 + Cu
128) Complete and balance the equation for each example in which a single-displacement reaction will occur. If no reaction will occur write the words “No Reaction” on the right side of the equation. Use this activity series:
More Active F2
Cl2
I2
Less Active Br2
a) Br2 + KCl →
b) F2 + LiBr →
c) Cl2 + KI →
d) I2 + NaCl →
Difficulty: medium
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
Solution: a) Br2 + KCl → No Reaction ; b) F2 + 2LiBr → 2LiF + Br2; c) Cl2 + 2KI → 2KCl + I2; d) I2 + NaCl → No Reaction
129) Benzene, C6H6, reacts with nitric acid, HNO3. Two products are formed, one of which is water. The second product has a molar mass of 213 grams. The second product is composed of 33.8% carbon, 1.42% hydrogen, 19.7% nitrogen, and 45.1% oxygen. Write a balanced chemical equation for this reaction.
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: C6H6 + 3HNO3 → C6H3N3O6 + 3H2O
130) Sulfuric acid is prepared commercially by the following series of reactions:
a) Sulfur is burned in oxygen to produce sulfur dioxide.
b) Sulfur dioxide is further reacted with oxygen to form sulfur trioxide.
c) Sulfur trioxide is reacted with sulfuric acid to produce pyrosulfuric acid, H2S2O7.
d) Pyrosulfuric acid is reacted with water to produce sulfuric acid.
Write a balanced chemical equation for each step in the commercial production of sulfuric acid.
Difficulty: medium
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: a) S + O2 → SO2; b) 2SO2 + O2 → 2SO3; c) SO3 + H2SO4 → H2S2O7; d) H2S2O7 + H2O → 2H2SO4
131) Use the following diagram and the reaction given below to calculate the number of water molecules that will be produced. Explain your reasoning.
2C2H2 + 5O2 
4CO2 + 2H2O
Difficulty: hard
Learning Objective 1: Write and balance chemical equations.
Section Reference 1: Section 8.2
Solution: 6 molecules H2O. The number molecules of C2H2 and O2 in the figure are three times the coefficients in the equation, so three times the number of water molecules (3 × 2 = 6) show in the balanced equation will be produced.
132) Absent-minded Joe prepared two colorless aqueous solutions but forgot to label the flasks! He knew that one solution was made with potassium sulfate and the other with zinc bromide. List three reactants that you might add to a small portion of the solutions in order to differentiate between them using the selective formation of a solid.
Difficulty: hard
Learning Objective 1: Give examples of a combination reaction, single displacement reaction, and double displacement reaction.
Section Reference 1: Section 8.3
Solution: There are several possible answers to this problem. The main point is to have students recognize that they may use the selective formation of a solid as the means of identifying the solutions. Some suggestions are given below.
Reactant | K2SO4 | ZnBr2 |
Ba(NO3)2 | BaSO4 precipitates | No precipitate |
NaOH | No precipitate | Zn(OH)2 precipitates |
Na2S | No precipitate | ZnS precipitates |
Ca(NO3)2 | CaSO4 precipitates | No precipitate |
Na2CO3 | No precipitate | ZnCO3 precipitates |
133) When 16.7 mL of water at 20°C are cooled to a temperature slightly below 0°C, the volume occupied by the water increases to 18.2 mL. Explain this observation taking into account the law of conservation of mass.
Difficulty: medium
Learning Objective 1: Describe the information present in a chemical equation.
Section Reference 1: Section 8.1
Solution: In any change, whether physical or chemical, mass is conserved. Therefore, the resulting change in volume must be due to a change in some other property that links mass and volume (i.e. density). Thus, we can conclude that ice has a lower density than liquid water and that the Law of Conservation of Mass is obeyed.
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Test Bank | Foundations of College Chemistry 15e by Hein Arena
By Hein Arena, Willard