Question 1

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? 
HI + HNO3  →\rarr→  I2 + NO (acidic solution)

Accepted Answer

A)  5
B)  7
C)  14
D)  17
E)  None of these. F) A) and E)
G) C) and D)

Question 2

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s)  →\rarr→  2Ag(s) + 2Cl-  + Zn2+.
If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Accepted Answer

A)  increase by 0.06 V.
B)  increase by 0.18 V.
C)  decrease by 0.06 V.
D)  decrease by 0.18 V.
E)  increase by 0.35 V. F) B) and E)
G) C) and D)

Question 3

Consider the following standard reduction potentials in acid solution: 3+(aq)  B) Al(s)  C) I-(aq)  D) I2(s)  E) Sn4+(aq) " class="answers-bank-image d-inline" rel="preload" > Which is the weakest oxidizing agent in this list?

Accepted Answer

A)  Al3+(aq) 
B)  Al(s) 
C)  I-(aq) 
D)  I2(s) 
E)  Sn4+(aq) F) B) and E)
G) A) and B)

Question 4

Using a table of standard reduction potentials, determine which of these reactions (if any) is/are nonspontaneous in the direction indicated at 25°C.

Accepted Answer

A)  2Fe3+ + 2Cl-  →\rarr→  2Fe2+ + Cl2(g) 
B)  2Fe3+ + 2Br-  →\rarr→  2Fe2+ + Br2(l) 
C)  2Fe3+ + 2I-  →\rarr→  2Fe2+ + I2(s) 
D)  A and B
E)  All are spontaneous. F) C) and D)
G) B) and D)

Question 5

Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

Accepted Answer

A)  Pb
B)  Fe
C)  Zn
D)  Na
E)  AgF) D) and E)
G) A) and C)

Question 6

The overall reaction 2Co3+(aq) + 2Cl-(aq)  →\rarr→  2Co2+(aq) + Cl2(g) has the standard cell voltage E°cell = 0.46 V. Given E° = 1.36 V for the reaction Cl2(g) + 2e-  →\rarr→  2Cl-(aq) , calculate the standard reduction potential for the following the half reaction at 25°C: Co3+ + e-  →\rarr→  Co2+

Accepted Answer

A)  1.82 V
B)  -0.90 V
C)  0.90 V
D)  -1.82 V
E)  -1.36 V F) C) and E)
G) A) and B)

Question 7

Will H2(g)form when Fe is placed in 1.0 M HCl?

Accepted Answer

Question 8

Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s) 
What is the balanced overall (net) cell reaction?

Accepted Answer

A)  2H+(aq) + 2Ag+(aq)  →\rarr→ H2(g) + 2Ag(s) 
B)  H2(g) + 2Ag(s)  →\rarr→  H+(aq) + 2Ag+(aq) 
C)  2H+(aq) + 2Ag(s)  →\rarr→  H2(g) + 2Ag+(aq) 
D)  H2(g) + Ag+(aq)  →\rarr→  H+(aq) + Ag(s) 
E)  H2(g) + 2Ag+(aq)  →\rarr→ 2H+(aq) + 2Ag(s)  F) B) and D)
G) A) and E)

Question 9

Which of these metals will not reduce water to hydrogen in basic solution under standard conditions?

Accepted Answer

A)  Cd
B)  Sr
C)  Mg
D)  Ba
E)  KF) None of the above
G) B) and E)

Question 10

Given the following standard reduction potentials in acid solution
O2 + 4H+ + 4e- $\rarr$ 2H2O E° = +1.23 V
Sn4+ + 2e- $\rarr$ Sn2+ E° = +0.13 V
Zn2+ + 2e- $\rarr$ Zn(s)E° = -0.76 V
write the formula of the strongest oxidizing agent.

Accepted Answer

The answer of Given the following standard reduction potentials in...

Question 11

When a solution of a certain gadolinium salt is electrolyzed with a current of 1.0 A for 2.0 h, 0.025 mol of Gd metal forms. Calculate the charge on the gadolinium ion in the salt.

Accepted Answer

The answer of When a solution of a certain gadolinium...

Question 12

Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu2+(aq) + H2(g)  →\rarr→  Cu(s) + 2H+(aq) . Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Accepted Answer

A)  The emf will increase.
B)  The emf will decrease.
C)  No change in the emf will be observed. D) A) and B)
E) A) and C)

Question 13

For the electrochemical cell Ni(s) | Ni2+(1 M) || H+(1 M) | H2(1 atm) | Pt(s) , which one of the following changes will cause a decrease in the cell voltage?

Accepted Answer

A)  Increase the pressure of H2 to 2.0 atm.
B)  Decrease the mass of the nickel electrode.
C)  Lower the pH of the cell electrolyte.
D)  Decrease the concentration of Ni2+ ion.
E)  None of the above.F) A) and C)
G) D) and E)

Question 14

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + SO32-  →\rarr→  Mn2+ + SO42-  (acidic solution)

Accepted Answer

A)  3
B)  4
C)  5
D)  8
E)  None of these. F) A) and B)
G) B) and C)

Question 15

Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br- (aq) + I2(s)  →\rarr→ Br2(l) + 2I- (aq)

Accepted Answer

A)  5.7 * 10-19
B)  18.30
C)  1.7 * 1054
D)  1.9 * 1018
E)  5.7 * 10-55 F) B) and C)
G) C) and E)

Question 16

Which one of the following reagents is capable of transforming Br- (aq) to Br2(l) under standard-state conditions?

Accepted Answer

A)  I- (aq) 
B)  NO3- (aq) 
C)  Ag+ (aq) 
D)  Al3+ (aq) 
E)  Au3+ (aq) F) None of the above
G) C) and D)

Question 17

Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H2O + 2Cl- (1.0 M)  →\rarr→  H2(1 atm) + Cl2(1 atm) + 2OH- (1 * 10-7 M)

Accepted Answer

A)  2.19 V
B)  1.78 V
C)  0.41 V
D)  -0.41 V
E)  -1.78 V F) A) and E)
G) B) and C)

Question 18

A certain electrochemical cell has for its cell reaction: Zn + HgO  →\rarr→  ZnO + Hg
Which is the half-reaction occurring at the anode?

Accepted Answer

A)  HgO + 2e-  →\rarr→  Hg + O2-
B)  Zn2+ + 2e-  →\rarr→  Zn
C)  Zn  →\rarr→  Zn2+ + 2e-
D)  ZnO + 2e-  →\rarr→  Zn E) B) and C)
F) All of the above

Question 19

Calculate the cell emf for the following reaction at 25°C:
2Ag+(0.010 M)+ H2(1 atm)$\rarr$ 2Ag(s)+ 2H+(pH = 6.0)

Accepted Answer

The answer of Calculate the cell emf for the following...

Question 20

Determine the equilibrium constant (Keq) at 25°C for the reaction Cl2(g) + 2Br- (aq)  →\rarr→  2Cl- (aq) + Br2(l)

Accepted Answer

A)  1.5 * 10-10
B)  6.3 * 109
C)  1.3 * 1041
D)  8.1 * 104
E)  9.8 F) A) and B)
G) A) and C)

Exam 19: Redox Reactions and Electrochemistry

For the electrochemical cell Ni(s) | Ni²⁺(1 M) || H⁺(1 M) | H₂(1 atm) | Pt(s) , which one of the following changes will cause a decrease in the cell voltage?

Correct Answer
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Which of these metals will not reduce water to hydrogen in basic solution under standard conditions?

Correct Answer
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Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H₂O + 2Cl^-(1.0 M) $\rarr$ H₂(1 atm) + Cl₂(1 atm) + 2OH^-(1 * 10^-7 M)

Correct Answer
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Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

Correct Answer
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Correct Answer
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Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) $\rarr$ 2Ag(s) + 2Cl^- + Zn²⁺. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct Answer
verified

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? HI + HNO₃ $\rarr$ I₂ + NO (acidic solution)

Correct Answer
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Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu²⁺(aq) + H₂(g) $\rarr$ Cu(s) + 2H⁺(aq) . Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Correct Answer
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When a solution of a certain gadolinium salt is electrolyzed with a current of 1.0 A for 2.0 h, 0.025 mol of Gd metal forms. Calculate the charge on the gadolinium ion in the salt.

Correct Answer
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Determine the equilibrium constant (K_eq) at 25°C for the reaction Cl₂(g) + 2Br^-(aq) $\rarr$ 2Cl^-(aq) + Br₂(l)

Correct Answer
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Given the following notation for an electrochemical cell Pt(s) | H₂(g) | H⁺(aq) || Ag⁺(aq) | Ag(s) What is the balanced overall (net) cell reaction?

Correct Answer
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Which one of the following reagents is capable of transforming Br^-(aq) to Br₂(l) under standard-state conditions?

Correct Answer
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Given the following standard reduction potentials in acid solution O₂ + 4H⁺ + 4e^- $\rarr$ 2H₂O E° = +1.23 V Sn⁴⁺ + 2e^- $\rarr$ Sn²⁺E° = +0.13 V Zn²⁺ + 2e^- $\rarr$ Zn(s)E° = -0.76 V write the formula of the strongest oxidizing agent.

Correct Answer
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Using a table of standard reduction potentials, determine which of these reactions (if any) is/are nonspontaneous in the direction indicated at 25°C.

Correct Answer
verified

Consider the following standard reduction potentials in acid solution: Which is the weakest oxidizing agent in this list?

Correct Answer
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Determine the equilibrium constant, K_eq, at 25°C for the reaction 2Br^-(aq) + I₂(s) $\rarr$ Br₂(l) + 2I^-(aq)

Correct Answer
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Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\rarr$ 2Ag(s)+ 2H⁺(pH = 6.0)

Correct Answer
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Complete and balance the following redox equation. What is the coefficient of H₂O when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + SO₃^2- $\rarr$ Mn²⁺ + SO₄^2- (acidic solution)

Correct Answer
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Will H₂(g)form when Fe is placed in 1.0 M HCl?

Correct Answer
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A certain electrochemical cell has for its cell reaction: Zn + HgO $\rarr$ ZnO + Hg Which is the half-reaction occurring at the anode?

Correct Answer
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Exam 19: Redox Reactions and Electrochemistry

For the electrochemical cell Ni(s) | Ni2+(1 M) || H+(1 M) | H2(1 atm) | Pt(s) , which one of the following changes will cause a decrease in the cell voltage?

Correct AnswerverifiedShow Answer

Which of these metals will not reduce water to hydrogen in basic solution under standard conditions?

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Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H2O + 2Cl- (1.0 M) →\rarr→ H2(1 atm) + Cl2(1 atm) + 2OH- (1 * 10-7 M)

Correct AnswerverifiedShow Answer

Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) →\rarr→ 2Ag(s) + 2Cl- + Zn2+. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct AnswerverifiedShow Answer

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? HI + HNO3 →\rarr→ I2 + NO (acidic solution)

Correct AnswerverifiedShow Answer

Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu2+(aq) + H2(g) →\rarr→ Cu(s) + 2H+(aq) . Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Correct AnswerverifiedShow Answer

When a solution of a certain gadolinium salt is electrolyzed with a current of 1.0 A for 2.0 h, 0.025 mol of Gd metal forms. Calculate the charge on the gadolinium ion in the salt.

Correct AnswerverifiedShow Answer

Determine the equilibrium constant (Keq) at 25°C for the reaction Cl2(g) + 2Br- (aq) →\rarr→ 2Cl- (aq) + Br2(l)

Correct AnswerverifiedShow Answer

Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s) What is the balanced overall (net) cell reaction?

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Which one of the following reagents is capable of transforming Br- (aq) to Br2(l) under standard-state conditions?

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Given the following standard reduction potentials in acid solution O2 + 4H+ + 4e- →\rarr→ 2H2O E° = +1.23 V Sn4+ + 2e- →\rarr→ Sn2+ E° = +0.13 V Zn2+ + 2e- →\rarr→ Zn(s)E° = -0.76 V write the formula of the strongest oxidizing agent.

Correct AnswerverifiedShow Answer

Using a table of standard reduction potentials, determine which of these reactions (if any) is/are nonspontaneous in the direction indicated at 25°C.

Correct AnswerverifiedShow Answer

Consider the following standard reduction potentials in acid solution: Which is the weakest oxidizing agent in this list?

Correct AnswerverifiedShow Answer

Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br- (aq) + I2(s) →\rarr→ Br2(l) + 2I- (aq)

Correct AnswerverifiedShow Answer

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M)+ H2(1 atm) →\rarr→ 2Ag(s)+ 2H+(pH = 6.0)

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Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + SO32- →\rarr→ Mn2+ + SO42- (acidic solution)

Correct AnswerverifiedShow Answer

Will H2(g)form when Fe is placed in 1.0 M HCl?

Correct AnswerverifiedShow Answer

A certain electrochemical cell has for its cell reaction: Zn + HgO →\rarr→ ZnO + Hg Which is the half-reaction occurring at the anode?

Correct AnswerverifiedShow Answer

For the electrochemical cell Ni(s) | Ni²⁺(1 M) || H⁺(1 M) | H₂(1 atm) | Pt(s) , which one of the following changes will cause a decrease in the cell voltage?

Correct Answer
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Correct Answer
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Calculate the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution. 2H₂O + 2Cl^-(1.0 M) $\rarr$ H₂(1 atm) + Cl₂(1 atm) + 2OH^-(1 * 10^-7 M)

Correct Answer
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Correct Answer
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Correct Answer
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Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) $\rarr$ 2Ag(s) + 2Cl^- + Zn²⁺. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct Answer
verified

Complete and balance the following redox equation using the set of smallest whole-numbers coefficients. What is the sum of the coefficients? HI + HNO₃ $\rarr$ I₂ + NO (acidic solution)

Correct Answer
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Correct Answer
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Correct Answer
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Determine the equilibrium constant (K_eq) at 25°C for the reaction Cl₂(g) + 2Br^-(aq) $\rarr$ 2Cl^-(aq) + Br₂(l)

Correct Answer
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Given the following notation for an electrochemical cell Pt(s) | H₂(g) | H⁺(aq) || Ag⁺(aq) | Ag(s) What is the balanced overall (net) cell reaction?

Correct Answer
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Which one of the following reagents is capable of transforming Br^-(aq) to Br₂(l) under standard-state conditions?

Correct Answer
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Given the following standard reduction potentials in acid solution O₂ + 4H⁺ + 4e^- $\rarr$ 2H₂O E° = +1.23 V Sn⁴⁺ + 2e^- $\rarr$ Sn²⁺E° = +0.13 V Zn²⁺ + 2e^- $\rarr$ Zn(s)E° = -0.76 V write the formula of the strongest oxidizing agent.

Correct Answer
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Correct Answer
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Correct Answer
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Determine the equilibrium constant, K_eq, at 25°C for the reaction 2Br^-(aq) + I₂(s) $\rarr$ Br₂(l) + 2I^-(aq)

Correct Answer
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Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\rarr$ 2Ag(s)+ 2H⁺(pH = 6.0)

Correct Answer
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Complete and balance the following redox equation. What is the coefficient of H₂O when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + SO₃^2- $\rarr$ Mn²⁺ + SO₄^2- (acidic solution)

Correct Answer
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Will H₂(g)form when Fe is placed in 1.0 M HCl?

Correct Answer
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A certain electrochemical cell has for its cell reaction: Zn + HgO $\rarr$ ZnO + Hg Which is the half-reaction occurring at the anode?

Correct Answer
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