Question 1

If ?rG° for the following reaction is -22.2 kJ/mol-rxn, calculate  Ecell ∘E _ { 	ext {cell } } ^ { \circ }Ecell ∘​  for the following reaction: Cu2+(aq)  + 2 Ag(s)  + 2 Cl-(aq)  ? Cu(s)  + 2 AgCl(s)

Accepted Answer

A)   -0.460 V
B)   -0.115 V
C)   +0.115 V
D)   +0.230 V
E)   +0.559 V F) C) and D)
G) B) and E)

Question 2

Calculate Ecell for the following electrochemical cell at 25 °C Pt(s)  | H2(g, 1.00 atm)  | H+(aq, 1.00 M)  || Sn2+(aq, 0.350 M) , Sn4+(aq, 0.020 M)  | Pt(s) 
The standard reduction potentials are as follows:
Sn4+(aq)  + 2 e- → Sn2+(s) 
E° = +0.15 V
2 H+(aq)  + 2 e- → H2(g) 
E° = 0.00 V

Accepted Answer

A)   -0.19 V
B)   +0.08 V
C)   +0.11 V
D)   +0.19 V
E)   +0.22 VF) A) and B)
G) A) and C)

Question 3

The cell potential of the following electrochemical cell is determined by using an unspecified concentration of acid. Calculate the pH of the acid solution, given that the measured cell potential is -0.431 V and the anode reduction potential (E°)  is 0.222 V at 25 °C. ​
Ag(s)  | AgCl(s)  | Cl−(aq, 1.0 M)  || H+(aq)  | H2(g, 1.0 atm)  | Pt(s) 
​

Accepted Answer

A)   3.53
B)   11.0
C)   4.03
D)   7.06
E)   3.47F) A) and D)
G) C) and E)

Question 4

Batteries used in watches contain mercury(II)  oxide. As the current flows, mercury(II)  oxide is reduced to mercury according to the following reaction: HgO(s)  + H2O(  ℓ\ellℓ  )  + 2 e- ? Hg(  ℓ\ellℓ  )  + 2 OH-(aq) 
If 2.3 × 10-5 amperes flows continuously for 1200 days, calculate the mass of mercury, Hg(  ℓ\ellℓ  ) , produced.

Accepted Answer

A)   2.5 g
B)   5.0 g
C)   9.9 g
D)   13 g
E)   15 g F) B) and E)
G) B) and D)

Question 5

Calculate ΔrG° for the disproportionation reaction of copper(I)  ion (Cu+)  at 25 °C. 2 Cu+(aq)  → Cu2+(aq)  + Cu(s) 
The standard reduction potentials are as follows:
Cu+(aq)  + e- → Cu(s) 
E° = +0.518 V
Cu2+(aq)  + 2 e- → Cu(s) 
E° = +0.337 V

Accepted Answer

A)   -165 kJ/mol⋅rxn
B)   -135 kJ/mol⋅rxn
C)   -34.9 kJ/mol⋅rxn
D)   +17.5 kJ/mol⋅rxn
E)   +135 kJ/mol⋅rxnF) C) and D)
G) D) and E)

Question 6

The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn4+(aq, 1.0 M) , Sn2+(aq, 1.0 M)  || Cu2+(aq, 0.200 M)  | Cu
Which of the following factors will increase the measured cell potential of the given electrochemical cell?

Accepted Answer

A)   Switching from a platinum to a graphite anode
B)   Increasing the size of the anode
C)   Decreasing the concentration of Cu2+
D)   Increasing the concentration of Sn4+
E)   Decreasing the temperature of the cellF) A) and B)
G) B) and C)

Question 7

Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

Accepted Answer

A)   2 H2O2(  ℓ\ellℓ  )  ? 2 H2O(  ℓ\ellℓ  )  + O2(g) 
B)   2 H2O2(  ℓ\ellℓ  )  + 2e- ? 2 H2O(  ℓ\ellℓ  )  + O2(g) 
C)   H2O2(  ℓ\ellℓ  )  + 2 H+(aq)  + 2 e- ? 2 H2O(  ℓ\ellℓ  ) 
D)   H2O2(  ℓ\ellℓ  )  + 4 H+(aq)  + 2 e- ? 2 H2O(  ℓ\ellℓ  )  + H2(g) 
E)   H2O2(  ℓ\ellℓ  )  + 2 H+(aq)  + 4 e- ? 2 H2(g)  + O2(g)  F) A) and B)
G) A) and E)

Question 8

Which of the following statements concerning voltaic cells is not true?

Accepted Answer

A)   A salt bridge allows cations and anions to move between half-cells.
B)   Electrons flow from a cathode to an anode in the external circuit.
C)   Oxidation occurs at an anode.
D)   A voltaic cell can be used as a source of energy.
E)   A voltaic cell consists of two half-cells.F) A) and B)
G) None of the above

Question 9

For the following cell reaction, the standard cell potential is 1.34 V. To determine the cell potential at nonstandard conditions, what is the value that should be used for n in the Nernst equation?  2MnO4−(aq) +5H2SO3(aq) →2Mn2+(aq) +5SO42−(aq) +4H+(aq) +3H2O(l) 2 \mathrm { MnO } _ { 4 } ^ { - } ( \mathrm { aq } )  + 5 \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } ( \mathrm { aq } )  \rightarrow 2 \mathrm { Mn } ^ { 2 + } ( \mathrm { aq } )  + 5 \mathrm { SO } _ { 4 } ^ { 2 - } ( \mathrm { aq } )  + 4 \mathrm { H } ^ { + } ( \mathrm { aq } )  + 3 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) 2MnO4−​(aq) +5H2​SO3​(aq) →2Mn2+(aq) +5SO42−​(aq) +4H+(aq) +3H2​O(l)

Accepted Answer

A)   8
B)   10
C)   5
D)   2
E)   6 F) A) and C)
G) None of the above

Question 10

Which of the following equations represents the Nernst equation?

Accepted Answer

A)    E=E∘−(RTnF) ln⁡QE = E ^ { \circ } - \left( \frac { R T } { n F } \right)  \ln QE=E∘−(nFRT​) lnQ 
B)    E=E∘+log⁡(RTnF) E = E ^ { \circ } + \log \left( \frac { R T } { n F } \right) E=E∘+log(nFRT​)  
C)    E=E∘−(RTnF) log⁡QE = E ^ { \circ } - \left( \frac { R T } { n F } \right)  \log QE=E∘−(nFRT​) logQ 
D)    E∘=E−(RTnF) ln⁡QE ^ { \circ } = E - \left( \frac { R T } { n F } \right)  \ln QE∘=E−(nFRT​) lnQ 
E)    E=E∘−(nFRT) ln⁡QE = E ^ { \circ } - \left( \frac { n F } { R T } \right)  \ln QE=E∘−(RTnF​) lnQF) All of the above
G) C) and D)

Question 11

The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( $\ell$ ), to produce solid sodium.

Accepted Answer

The answer of The use of electrical energy to produce...

Question 12

What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

Accepted Answer

A)   K(s)  → K+(l)  + e-
B)   Br2(l)  + 2 e- → 2 Br-(l) 
C)   2 Br-(l)  → Br2(l)  + 2 e-
D)   2 K+(l)  + 2 e- → 2 K(l) 
E)   2 H2O(l)  + 2 e- → H2(g)  + 2 OH-(l) F) A) and D)
G) All of the above

Question 13

Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? 
Fe3+(aq)  + Co(s)  → Fe2+(aq)  + Co2+(aq)

Accepted Answer

A)   Fe3+(aq)  is oxidized and Co(s)  is reduced.
B)   Fe3+(aq)  is oxidized and Co2+(aq)  is reduced.
C)   Co(s)  is oxidized and Fe3+(aq)  is reduced.
D)   Co(s)  is oxidized and Co2+(aq)  is reduced.
E)   Fe2+(aq)  is oxidized and Co(s)  is reduced.F) C) and E)
G) None of the above

Question 14

Which of the following statements is true concerning the electrochemical cell Zn(s)  | Zn2+(aq, 1.0 M)  || Ca2+(aq, 1.0 M)  | Ca(s)  The standard reduction potentials are given follows:
Zn2+(aq)  + 2 e− → Zn(s) ; E° = -0.76 V
Ca2+(aq)  + 2 e− → Ca(s) ; E° = -2.87 V

Accepted Answer

A)   The standard cell potential is -3.63 V.
B)   The standard cell potential is -2.11 V.
C)   The standard cell potential is -2.11 V..
D)   The standard cell potential is -3.63 V..
E)   The standard cell potential is 2.11 V.F) A) and C)
G) B) and D)

Question 15

Which of the following is true for a product-favored reaction at equilibrium?

Accepted Answer

A)   ΔrG° cell > 0
B)   ΔrG° > 0; E°cell 
C)   ΔrG° cell 
D)   ΔrG° > 0; E°cell > 0
E)   ΔrG° > 0; E°cell = 0F) None of the above
G) B) and E)

Question 16

Balance the following half-reaction occurring in an acidic solution. 
NO3-(aq)  → NO(aq)

Accepted Answer

A)   NO3-(aq)  + 4 H+(aq)  + 3 e− → NO(g)  + 2 H2O(l) 
B)   NO3-(aq)  + 2 H2O(l)  + 3 e− → NO(g)  + 4 H+(aq) 
C)   NO3-(aq)  + 4 H+(aq)  → NO(g)  + 2 H2O(l)  + 3 e−
D)   NO3-(aq)  + 3 e− → NO(g)  + 4 H+(aq)  + 2 H2O(l) 
E)   NO3-(aq)  + 4 H+(aq) → NO(g)  + 2 H2O(l) F) A) and E)
G) A) and D)

Question 17

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is 
Co3+(aq)  + e− → Co2+(aq) ?

Accepted Answer

A)   Pt(s)  | H2(g)  | H+(aq)  || Co3+(aq) , Co2+(aq)  | Pt(s) 
B)   Pt(s)  | H2(g)  | H+(aq)  || Co3+(aq) , Co2+(aq) 
C)   Co2+(aq) , Co3+(aq)  || H+(aq)  | H2(g)  | Pt(s) 
D)   Pt(s) | Co2+(aq) , Co3+(aq)  || H+(aq)  | H2(g)  | Pt(s) 
E)   H2(g)  | H+(aq)  || Co2+(aq) , Co3+(aq) F) All of the above
G) A) and C)

Question 18

The standard reduction potentials are as follows: Cr3+(aq)  + 3 e- → Cr(s) ; E° = -0.74 V
Fe2+(aq)  + 2 e- → Fe(s) ; E° = -0.41 V
Calculate the standard Gibbs free energy change for the following reaction.
2 Cr(s)  + 3 Fe2+ → 3 Fe(s)  + 2 Cr3+(aq)

Accepted Answer

A)   191 kJ
B)   63.7 kJ
C)   -504 kJ
D)   -191 kJ
E)   1060 kJF) A) and C)
G) A) and E)

Question 19

Which of the following statements is true concerning the voltaic cell shown below?

Accepted Answer

A)   The Zn anode mass decreases as the cell discharges.
B)   The Zn cathode mass increases as the cell discharges.
C)   The Zn cathode mass decreases as the cell discharges.
D)   The Zn anode mass increases as the cell discharges.
E)   The mass of the Zn electrode neither increases nor decreases as the cell discharges.F) All of the above
G) D) and E)

Question 20

According to the cell notation below, which of the following species is undergoing reduction? 
Ni | Ni2+(aq)  || Mn2+(aq)  | MnO2(s)  | Pt(s)

Accepted Answer

A)   Mn2+(aq) 
B)   Ni2+(aq) 
C)   Ni(s) 
D)   MnO2(s) 
E)   Pt(s) F) B) and E)
G) A) and E)

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn²⁺(aq, 1.0 M) || Ca²⁺(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn²⁺(aq) + 2 e− → Zn(s) ; E° = -0.76 V Ca²⁺(aq) + 2 e− → Ca(s) ; E° = -2.87 V

Correct Answer
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Correct Answer
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Calculate Δ_rG° for the disproportionation reaction of copper(I) ion (Cu⁺) at 25 °C. 2 Cu⁺(aq) → Cu²⁺(aq) + Cu(s) The standard reduction potentials are as follows: Cu⁺(aq) + e^- → Cu(s) E° = +0.518 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.337 V

Correct Answer
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The standard reduction potentials are as follows: Cr³⁺(aq) + 3 e^- → Cr(s) ; E° = -0.74 V Fe²⁺(aq) + 2 e^- → Fe(s) ; E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe²⁺ → 3 Fe(s) + 2 Cr³⁺(aq)

Correct Answer
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Which of the following statements is true concerning the voltaic cell shown below?

Correct Answer
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Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? Fe³⁺(aq) + Co(s) → Fe²⁺(aq) + Co²⁺(aq)

Correct Answer
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Correct Answer
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If ?_rG° for the following reaction is -22.2 kJ/mol-rxn, calculate $E _ { \text {cell } } ^ { \circ }$ for the following reaction: Cu²⁺(aq) + 2 Ag(s) + 2 Cl^-(aq) ? Cu(s) + 2 AgCl(s)

Correct Answer
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Correct Answer
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Which of the following statements concerning voltaic cells is not true?

Correct Answer
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Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

Correct Answer
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Which of the following equations represents the Nernst equation?

Correct Answer
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Balance the following half-reaction occurring in an acidic solution. NO₃^-(aq) → NO(aq)

Correct Answer
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The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn⁴⁺(aq, 1.0 M) , Sn²⁺(aq, 1.0 M) || Cu²⁺(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

Correct Answer
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What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

Correct Answer
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Which of the following is true for a product-favored reaction at equilibrium?

Correct Answer
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Correct Answer
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The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( $\ell$ ), to produce solid sodium.

Correct Answer
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According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

Correct Answer
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Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq) ?

Correct Answer
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Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn2+(aq, 1.0 M) || Ca2+(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn2+(aq) + 2 e− → Zn(s) ; E° = -0.76 V Ca2+(aq) + 2 e− → Ca(s) ; E° = -2.87 V

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Calculate ΔrG° for the disproportionation reaction of copper(I) ion (Cu+) at 25 °C. 2 Cu+(aq) → Cu2+(aq) + Cu(s) The standard reduction potentials are as follows: Cu+(aq) + e- → Cu(s) E° = +0.518 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.337 V

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The standard reduction potentials are as follows: Cr3+(aq) + 3 e- → Cr(s) ; E° = -0.74 V Fe2+(aq) + 2 e- → Fe(s) ; E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe2+ → 3 Fe(s) + 2 Cr3+(aq)

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Which of the following statements is true concerning the voltaic cell shown below?

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Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? Fe3+(aq) + Co(s) → Fe2+(aq) + Co2+(aq)

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If ?rG° for the following reaction is -22.2 kJ/mol-rxn, calculate Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ for the following reaction: Cu2+(aq) + 2 Ag(s) + 2 Cl-(aq) ? Cu(s) + 2 AgCl(s)

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Which of the following statements concerning voltaic cells is not true?

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Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

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Which of the following equations represents the Nernst equation?

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Balance the following half-reaction occurring in an acidic solution. NO3-(aq) → NO(aq)

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The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn4+(aq, 1.0 M) , Sn2+(aq, 1.0 M) || Cu2+(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

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What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

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Which of the following is true for a product-favored reaction at equilibrium?

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Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Sn2+(aq, 0.350 M) , Sn4+(aq, 0.020 M) | Pt(s) The standard reduction potentials are as follows: Sn4+(aq) + 2 e- → Sn2+(s) E° = +0.15 V 2 H+(aq) + 2 e- → H2(g) E° = 0.00 V

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The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( ℓ\ellℓ ), to produce solid sodium.

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According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni2+(aq) || Mn2+(aq) | MnO2(s) | Pt(s)

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Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co3+(aq) + e− → Co2+(aq) ?

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Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn²⁺(aq, 1.0 M) || Ca²⁺(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn²⁺(aq) + 2 e− → Zn(s) ; E° = -0.76 V Ca²⁺(aq) + 2 e− → Ca(s) ; E° = -2.87 V

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Correct Answer
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Calculate Δ_rG° for the disproportionation reaction of copper(I) ion (Cu⁺) at 25 °C. 2 Cu⁺(aq) → Cu²⁺(aq) + Cu(s) The standard reduction potentials are as follows: Cu⁺(aq) + e^- → Cu(s) E° = +0.518 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.337 V

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The standard reduction potentials are as follows: Cr³⁺(aq) + 3 e^- → Cr(s) ; E° = -0.74 V Fe²⁺(aq) + 2 e^- → Fe(s) ; E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe²⁺ → 3 Fe(s) + 2 Cr³⁺(aq)

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Correct Answer
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Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? Fe³⁺(aq) + Co(s) → Fe²⁺(aq) + Co²⁺(aq)

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Correct Answer
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If ?_rG° for the following reaction is -22.2 kJ/mol-rxn, calculate $E _ { \text {cell } } ^ { \circ }$ for the following reaction: Cu²⁺(aq) + 2 Ag(s) + 2 Cl^-(aq) ? Cu(s) + 2 AgCl(s)

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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Balance the following half-reaction occurring in an acidic solution. NO₃^-(aq) → NO(aq)

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The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn⁴⁺(aq, 1.0 M) , Sn²⁺(aq, 1.0 M) || Cu²⁺(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( $\ell$ ), to produce solid sodium.

Correct Answer
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According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

Correct Answer
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Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq) ?

Correct Answer
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