Question 1

Identify the oxidation state of H in H2(g). 
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

Accepted Answer

A)  +1 
B)  +2 
C)  0 
D)  -1 
E)  -2 
A)  +1 
B)  +2 
C)  0 
D)  -1 
E)  -2

Question 2

What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

Accepted Answer

A)  O 
B)  H 
C)  C 
D)  both C and H 
E)  This is not an oxidation-reduction reaction. 
A)  O 
B)  H 
C)  C 
D)  both C and H 
E)  This is not an oxidation-reduction reaction.

Question 3

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction? Zn2+(aq) + NH4+(aq) → Zn(s) + NO3⁻(aq)

Accepted Answer

A)  Zn = 1, H⁺ = 8 
B)  Zn = 1, H⁺ = 4 
C)  Zn = 4, H⁺ = 10 
D)  Zn = 2, H⁺ = 4 
E)  Zn = 3, H⁺ = 5 
A)  Zn = 1, H⁺ = 8 
B)  Zn = 1, H⁺ = 4 
C)  Zn = 4, H⁺ = 10 
D)  Zn = 2, H⁺ = 4 
E)  Zn = 3, H⁺ = 5

Question 4

If 100. mL of 0.400 mol L-1 Na2SO4 is added to 200. mL of 0.600 mol L-1 NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.

Accepted Answer

A)  0.534 mol L-1 
B)  0.667 mol L-1 
C)  1.00 mol L-1 
D)  1.40 mol L-1 
A)  0.534 mol L-1 
B)  0.667 mol L-1 
C)  1.00 mol L-1 
D)  1.40 mol L-1

Question 5

Which of the following compounds is an Arrhenius base?

Accepted Answer

A)  CH3OH 
B)  CH3CO2H 
C)  HOCl 
D)  CsOH 
A)  CH3OH 
B)  CH3CO2H 
C)  HOCl 
D)  CsOH

Question 6

Match the following.
-CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

Accepted Answer

A) acid-base 
B) oxidation-reduction 
C) precipitation 
D) gas evolution 
E) combustion 
A) acid-base 
B) oxidation-reduction 
C) precipitation 
D) gas evolution 
E) combustion

Question 7

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kilograms of iodine were produced?

Accepted Answer

A)  13.3 kg 
B)  22.5 kg 
C)  79.2 kg 
D)  44.4 kg 
E)  92.4 kg 
A)  13.3 kg 
B)  22.5 kg 
C)  79.2 kg 
D)  44.4 kg 
E)  92.4 kg

Question 8

Identify the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.

Accepted Answer

A)  2H+(aq) + CO32-(aq) → H2CO3(s) 
B)  2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl-(aq) → H2CO3(s) + 2NaCl(aq) 
C)  2H+(aq) + CO32-(aq) → H2O(l) + CO2(g) 
D)  2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl-(aq) → H2CO3(s) + 2Na+(aq) + 2Cl-(aq) 
E)  No reaction occurs. 
A)  2H+(aq) + CO32-(aq) → H2CO3(s) 
B)  2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl-(aq) → H2CO3(s) + 2NaCl(aq) 
C)  2H+(aq) + CO32-(aq) → H2O(l) + CO2(g) 
D)  2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl-(aq) → H2CO3(s) + 2Na+(aq) + 2Cl-(aq) 
E)  No reaction occurs.

Question 9

According to the following reaction, what volume of 0.244 mol L-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L-1 Pb(NO3)2 solution? 
2KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2KNO3(aq)

Accepted Answer

A)  97.4 mL 
B)  116 mL 
C)  43.0 mL 
D)  86.1 mL 
E)  58.1 mL 
A)  97.4 mL 
B)  116 mL 
C)  43.0 mL 
D)  86.1 mL 
E)  58.1 mL

Question 10

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H2O? Assume an excess of KO. 
4KO(s) + 2H2O(l) → 4KOH(s) + O2(g)

Accepted Answer

A)  2.72 moles KOH 
B)  16.7 moles KOH 
C)  10.9 moles KOH 
D)  8.33 moles KOH 
E)  4.87 moles KOH 
A)  2.72 moles KOH 
B)  16.7 moles KOH 
C)  10.9 moles KOH 
D)  8.33 moles KOH 
E)  4.87 moles KOH

Question 11

What is the concentration of magnesium ions in a 0.125 mol L-1 Mg(NO3)2 solution?

Accepted Answer

A)  0.125 mol L-1 
B)  0.0625 mol L-1 
C)  0.375 mol L-1 
D)  0.250 mol L-1 
E)  0.160 mol L-1 
A)  0.125 mol L-1 
B)  0.0625 mol L-1 
C)  0.375 mol L-1 
D)  0.250 mol L-1 
E)  0.160 mol L-1

Question 12

What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution? 
________ NO3-(aq) + ________ Cu(s) → ________ NO(g) + ________ Cu2+(aq)?

Accepted Answer

A)  2, 3 
B)  2, 6 
C)  3, 4 
D)  3, 6 
A)  2, 3 
B)  2, 6 
C)  3, 4 
D)  3, 6

Question 13

Define a limiting reactant.

Accepted Answer

A limiting reactant is a react

Question 14

Which of the following statements is FALSE?

Accepted Answer

A)  Aqueous reactions can be represented with a molecular equation. 
B)  Aqueous reactions can be represented with a complete ionic equation. 
C)  Aqueous reactions can be represented with a net ionic equation. 
D)  Precipitation reactions isoccur when two aqueous solutions are mixed a to form a solid precipitate. 
E)  Spectator ions change the course of the reaction and are included in the net ionic equation. 
A)  Aqueous reactions can be represented with a molecular equation. 
B)  Aqueous reactions can be represented with a complete ionic equation. 
C)  Aqueous reactions can be represented with a net ionic equation. 
D)  Precipitation reactions isoccur when two aqueous solutions are mixed a to form a solid precipitate. 
E)  Spectator ions change the course of the reaction and are included in the net ionic equation.

Question 15

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. A possibly useful molar mass is 
BCl3 = 117.16 g mol-1. BCl3(g) + 3H2O(l) → H3BO3(s) + 3HCl(g)

Accepted Answer

A)  75.9 g HCl 
B)  132 g HCl 
C)  187 g HCl 
D)  56.0 g HCl 
E)  25.3 g HCl 
A)  75.9 g HCl 
B)  132 g HCl 
C)  187 g HCl 
D)  56.0 g HCl 
E)  25.3 g HCl

Question 16

What are the required coefficients to properly balance the following chemical reaction? 
MnCl2(s) + H2O(l) + Cl2(g) → HCl(aq) + MnO2(s)

Accepted Answer

A)  1, 2, 1, 4, 1 
B)  2, 2, 1, 4, 2 
C)  1, 1, 1, 2, 1 
D)  1, 1, 1, 4, 1 
E)  2, 1, 1, 4, 2 
A)  1, 2, 1, 4, 1 
B)  2, 2, 1, 4, 2 
C)  1, 1, 1, 2, 1 
D)  1, 1, 1, 4, 1 
E)  2, 1, 1, 4, 2

Question 17

Determine the oxidation state of C in CO32-.

Accepted Answer

A)  +4 
B)  +2 
C)  -2 
D)  -4 
E)  +6 
A)  +4 
B)  +2 
C)  -2 
D)  -4 
E)  +6

Question 18

What is the concentration of nitrate ions in a 0.125 mol L-1 Mg(NO3)2 solution?

Accepted Answer

A)  0.125 mol L-1 
B)  0.0625 mol L-1 
C)  0.375 mol L-1 
D)  0.250 mol L-1 
E)  0.160 mol L-1 
A)  0.125 mol L-1 
B)  0.0625 mol L-1 
C)  0.375 mol L-1 
D)  0.250 mol L-1 
E)  0.160 mol L-1

Question 19

What are the required coefficients to properly balance the following chemical reaction? 
C6H12O6(s) + O2(g) → CO2(g) + H2O(l)

Accepted Answer

A)  1, 3, 3, 3 
B)  2, 6, 6, 3 
C)  1, 6, 6, 6 
D)  1, 1, 3, 3 
E)  2, 2, 6, 3 
A)  1, 3, 3, 3 
B)  2, 6, 6, 3 
C)  1, 6, 6, 6 
D)  1, 1, 3, 3 
E)  2, 2, 6, 3

Question 20

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) + 3H2(g) → 2NH3(g)

Accepted Answer

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. 
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.

Exam 4: Chemical Reactions and Stoichiometry

Identify the oxidation state of H in H2(g). Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction? Zn2+(aq) + NH4+(aq) → Zn(s) + NO3⁻(aq)

If 100. mL of 0.400 mol L-1 Na2SO4 is added to 200. mL of 0.600 mol L-1 NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.

Which of the following compounds is an Arrhenius base?

Match the following. -CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kilograms of iodine were produced?

Identify the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.

According to the following reaction, what volume of 0.244 mol L-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L-1 Pb(NO3)2 solution? 2KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2KNO3(aq)

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H2O? Assume an excess of KO. 4KO(s) + 2H2O(l) → 4KOH(s) + O2(g)

What is the concentration of magnesium ions in a 0.125 mol L-1 Mg(NO3)2 solution?

What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution? ________ NO3-(aq) + ________ Cu(s) → ________ NO(g) + ________ Cu2+(aq)?

Define a limiting reactant.

Which of the following statements is FALSE?

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl3 = 117.16 g mol-1. BCl3(g) + 3H2O(l) → H3BO3(s) + 3HCl(g)

What are the required coefficients to properly balance the following chemical reaction? MnCl2(s) + H2O(l) + Cl2(g) → HCl(aq) + MnO2(s)

Determine the oxidation state of C in CO32-.

What is the concentration of nitrate ions in a 0.125 mol L-1 Mg(NO3)2 solution?

What are the required coefficients to properly balance the following chemical reaction? C6H12O6(s) + O2(g) → CO2(g) + H2O(l)

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) + 3H2(g) → 2NH3(g)

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Identify the oxidation state of H in H₂(g). Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

What element is undergoing oxidation (if any) in the following reaction? CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Znand H⁺ in the balanced reaction? Zn²⁺(aq) + NH₄⁺(aq) → Zn(s) + NO₃⁻(aq)

If 100. mL of 0.400 mol L^-1 Na₂SO₄ is added to 200. mL of 0.600 mol L^-1 NaCl, what is the concentration of Na⁺ ions in the final solution? Assume that the volumes are additive.

Match the following. -CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)

Identify the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

According to the following reaction, what volume of 0.244 mol L^-1 KCl solution is required to react exactly with 50.0 mL of a 0.210 mol L^-1 Pb(NO₃)₂ solution? 2KCl(aq) + Pb(NO₃)₂(aq) → PbCl₂(s) + 2KNO₃(aq)

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

What is the concentration of magnesium ions in a 0.125 mol L^-1 Mg(NO₃)₂ solution?

What are the coefficients in front of NO₃^-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution? NO₃^-(aq) + Cu(s) → NO(g) + Cu²⁺(aq)?

Determine the theoretical yield of HCl if 60.0 g of BCl₃and 37.5 g of H₂O are reacted according to the following balanced reaction. A possibly useful molar mass is BCl₃ = 117.16 g mol^-1. BCl₃(g) + 3H₂O(l) → H₃BO₃(s) + 3HCl(g)

What are the required coefficients to properly balance the following chemical reaction? MnCl₂(s) + H₂O(l) + Cl₂(g) → HCl(aq) + MnO₂(s)

Determine the oxidation state of C in CO₃^2-.

What is the concentration of nitrate ions in a 0.125 mol L^-1 Mg(NO₃)₂ solution?

What are the required coefficients to properly balance the following chemical reaction? C₆H₁₂O₆(s) + O₂(g) → CO₂(g) + H₂O(l)

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) + 3H₂(g) → 2NH₃(g)