What is the concentration of Cu2+(aq)in the following cell at 25 °C if the cell voltage is 1.253 V? Zn(s)∣ Zn2+ (aq,0.125 M) Cu2+(?)∣ Cu(s) Cu2+(aq)+ 2 e- → Cu(s)E° = 0.340 V Zn2+(aq)+ 2 e- → Zn(s)E° = -0.763 V

A) 0.6 M B) 1 × 10-2 M C) 1 × 10-6 M D) 9 × 10-4 M E) 4 × 10-4 M A) 0.6 M B) 1 × 10-2 M C) 1 × 10-6 M D) 9 × 10-4 M E) 4 × 10-4 M

What is E° of the spontaneous cell made from the Zn2+(aq)/Zn(s)(-0.76 V)and Br2(l)/2 Br-(aq)(1.07 V)half cells?

A) -1.83 V B) 0.31 V C) 1.83 V D) -0.31 V E) -0.76 V A) -1.83 V B) 0.31 V C) 1.83 V D) -0.31 V E) -0.76 V

Determine E°cell for the reaction: Pb(s)+ Zn2+(aq)→ Pb2+(aq)+ Zn(s). The half reactions are: Pb2+(aq)+ 2 e- → Pb(s)E° = -0.125 V Zn2+(aq)+ 2 e- → Zn(s)E° = -0.763 V

A) 0.638 V B) -0.638 V C) 0.888 V D) -1.276 V E) -0.888 V A) 0.638 V B) -0.638 V C) 0.888 V D) -1.276 V E) -0.888 V

Consider the cell: Ni(s)∣ Ni2+ (aq,?M) Cu2+ (aq,0.136 M)∣ Cu(s) Ni2+(aq)/Ni(s) E° = -0.257 V Cu2+(aq)/Cu(s) E° = 0.340 V The measured potential of the cell is 0.621 V.What is [Ni2+] at 25 °C?

A) 2 × 10-2 M B) 1 M C) 4 × 10-42 M D) 0.05 M E) 0.4 M A) 2 × 10-2 M B) 1 M C) 4 × 10-42 M D) 0.05 M E) 0.4 M

Two cells containing solutions of AgNO3(aq)and CuSO4(aq),respectively,were connected in series and electrolyzed.The cathode in the AgNO3(aq)cell was found to gain 1.078 grams in weight.How much had the cathode in the other cell gained?

A) 0.127 g B) 0.6354 g C) 3.175 g D) 0.318 g E) 0.254 g A) 0.127 g B) 0.6354 g C) 3.175 g D) 0.318 g E) 0.254 g

Determine E°cell at 25 °C for the following reaction: Pb2+(aq)+ Cu(s)→ Cu2+(aq)+ Pb(s) The half-reactions are: Pb2+(aq)+ 2 e- → Pb(s)E° = -0.125 V Cu2+(aq)+ 2 e- → Cu(s)E° = +0.337 V

A) 0.212 V B) -0.462 V C) 0.462 V D) -0.212 V E) 0.424 V A) 0.212 V B) -0.462 V C) 0.462 V D) -0.212 V E) 0.424 V

Consider the following standard reduction potentials: Ni2+(aq)+ 2 e- → Ni(s)E° = -0.26 V I2(s)+ 2 e- → 2 I-(aq)E° = +0.54 V Under standard conditions:

A) Ni2+(aq)is a stronger oxidizing agent than I2(s),and I-(aq)is a stronger reducing agent than Ni(s) B) I2(s)is a stronger oxidizing agent than Ni2+(aq),and Ni(s)is a stronger reducing agent than I-(aq) C) Ni(s)is a stronger oxidizing agent than I-(aq),and Ni2+(aq)is a stronger reducing agent than I2(s) D) I-(aq)is a stronger oxidizing agent than Ni(s),and I2(s)is a stronger reducing agent than Ni2+(aq) A) Ni2+(aq)is a stronger oxidizing agent than I2(s),and I-(aq)is a stronger reducing agent than Ni(s) B) I2(s)is a stronger oxidizing agent than Ni2+(aq),and Ni(s)is a stronger reducing agent than I-(aq) C) Ni(s)is a stronger oxidizing agent than I-(aq),and Ni2+(aq)is a stronger reducing agent than I2(s) D) I-(aq)is a stronger oxidizing agent than Ni(s),and I2(s)is a stronger reducing agent than Ni2+(aq)

Exam 19: Electrochemistry

What is the concentration of Cu²⁺(aq)in the following cell at 25 °C if the cell voltage is 1.253 V? Zn(s)∣ Zn²⁺ (aq,0.125 M) Cu²⁺(?)∣ Cu(s) Cu²⁺(aq)+ 2 e^- → Cu(s)E° = 0.340 V Zn²⁺(aq)+ 2 e^- → Zn(s)E° = -0.763 V

(Multiple Choice)

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Question 61

Choose the INCORRECT statement.

(Multiple Choice)

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Question 62

What is E° of the spontaneous cell made from the Zn²⁺(aq)^/Zn(s)(-0.76 V)and Br₂(l)_/2 Br^-(aq)(1.07 V)half cells?

(Multiple Choice)

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Question 63

Choose the INCORRECT completion of the following sentence: "In the electrolysis of water...

(Multiple Choice)

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Question 64

Determine E°_cell for the reaction: Pb(s)+ Zn²⁺(aq)→ Pb²⁺(aq)+ Zn(s). The half reactions are: Pb²⁺(aq)+ 2 e^- → Pb(s)E° = -0.125 V Zn²+(aq)+ 2 e^- → Zn(s)E° = -0.763 V

(Multiple Choice)

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Question 65

What is the standard cell potential if the Gibbs energy is -2108 kJ in the reaction: C₃H₈(g)+ O₂(g)→ CO₂(g)+ H₂O(l)(not balanced)?

(Multiple Choice)

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Question 66

Consider the cell: Ni(s)∣ Ni²⁺ (aq,?M) Cu²⁺ (aq,0.136 M)∣ Cu(s) Ni²⁺(aq)/Ni(s) E° = -0.257 V Cu²⁺(aq)/Cu(s) E° = 0.340 V The measured potential of the cell is 0.621 V.What is [Ni^2+] at 25 °C?

(Multiple Choice)

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Question 67

Two cells containing solutions of AgNO₃(aq)and CuSO₄(aq),respectively,were connected in series and electrolyzed.The cathode in the AgNO₃(aq)cell was found to gain 1.078 grams in weight.How much had the cathode in the other cell gained?

(Multiple Choice)

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Question 68

What is K_eqat 25 °C of the spontaneous cell made from Ag⁺(aq)/Ag(s)(0.80 V)and Cl₂(g)/Cl^-(aq)(1.36 V)half cells?

(Multiple Choice)

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Question 69

Given that E°_red = -1.66 V for Al³⁺(aq)/Al(s)at 25 °C,find E° and E for the concentration cell expressed using shorthand notation below: Al(s)∣ Al³⁺(aq,1.0 × 10^-5 mol L^-1)∣∣ Al³⁺(aq,0.100 mol L^-1)∣ Al(s)

(Multiple Choice)

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Question 70

Primary batteries' cell reactions cannot be reversed.

(True/False)

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Question 71

Determine E°_cell at 25 °C for the following reaction: Pb²⁺(aq)+ Cu(s)→ Cu²⁺(aq)+ Pb(s) The half-reactions are: Pb²⁺(aq)+ 2 e^- → Pb(s)E° = -0.125 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = +0.337 V

(Multiple Choice)

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Question 72

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni²⁺(aq)∣∣ Cl₂(g)∣ Cl^-(aq)∣ C(s)

(Multiple Choice)

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Question 73

How long would it take to deposit 15.0 g copper metal at the cathode of an electrolysis cell running with a current of 150 mA?

(Multiple Choice)

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Question 74

Consider the following standard reduction potentials: Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.26 V I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Under standard conditions:

(Multiple Choice)

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Question 75

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ → Ag(s)+ (aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 mol L^-1 and 2.22 mol L^-1,respectively.The cell emf is ________ V.

(Multiple Choice)

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Question 76

Choose the INCORRECT statement.

(Multiple Choice)

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Question 77

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s)∣ Zn²⁺(aq)∣∣ Ni²⁺(aq)∣ Ni(s)

(Multiple Choice)

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Question 78

What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe²⁺(aq)+ F₂(g)→ 2 Fe³⁺(aq)+ 2 F^-(aq)

(Multiple Choice)

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Question 79

A voltaic cell is constructed with two -Zn electrodes,where the half-reaction is (aq)+ → Zn(s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 mol L^-1 and 1.11 × Mol L^-1,respectively.The cell emf is ________ V.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 127

Exam 19: Electrochemistry

What is the concentration of Cu2+(aq)in the following cell at 25 °C if the cell voltage is 1.253 V? Zn(s)∣ Zn2+ (aq,0.125 M) Cu2+(?)∣ Cu(s) Cu2+(aq)+ 2 e- → Cu(s)E° = 0.340 V Zn2+(aq)+ 2 e- → Zn(s)E° = -0.763 V

Choose the INCORRECT statement.

What is E° of the spontaneous cell made from the Zn2+(aq)/Zn(s)(-0.76 V)and Br2(l)/2 Br-(aq)(1.07 V)half cells?

Choose the INCORRECT completion of the following sentence: "In the electrolysis of water...

Determine E°cell for the reaction: Pb(s)+ Zn2+(aq)→ Pb2+(aq)+ Zn(s). The half reactions are: Pb2+(aq)+ 2 e- → Pb(s)E° = -0.125 V Zn2+(aq)+ 2 e- → Zn(s)E° = -0.763 V

What is the standard cell potential if the Gibbs energy is -2108 kJ in the reaction: C3H8(g)+ O2(g)→ CO2(g)+ H2O(l)(not balanced)?

Consider the cell: Ni(s)∣ Ni2+ (aq,?M) Cu2+ (aq,0.136 M)∣ Cu(s) Ni2+(aq)/Ni(s) E° = -0.257 V Cu2+(aq)/Cu(s) E° = 0.340 V The measured potential of the cell is 0.621 V.What is [Ni2+] at 25 °C?

Two cells containing solutions of AgNO3(aq)and CuSO4(aq),respectively,were connected in series and electrolyzed.The cathode in the AgNO3(aq)cell was found to gain 1.078 grams in weight.How much had the cathode in the other cell gained?

What is Keq at 25 °C of the spontaneous cell made from Ag+(aq)/Ag(s)(0.80 V)and Cl2(g)/Cl-(aq)(1.36 V)half cells?

Given that E°red = -1.66 V for Al3+(aq)/Al(s)at 25 °C,find E° and E for the concentration cell expressed using shorthand notation below: Al(s)∣ Al3+(aq,1.0 × 10-5 mol L-1)∣∣ Al3+(aq,0.100 mol L-1)∣ Al(s)

Primary batteries' cell reactions cannot be reversed.

Determine E°cell at 25 °C for the following reaction: Pb2+(aq)+ Cu(s)→ Cu2+(aq)+ Pb(s) The half-reactions are: Pb2+(aq)+ 2 e- → Pb(s)E° = -0.125 V Cu2+(aq)+ 2 e- → Cu(s)E° = +0.337 V

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni2+(aq)∣∣ Cl2(g)∣ Cl-(aq)∣ C(s)

How long would it take to deposit 15.0 g copper metal at the cathode of an electrolysis cell running with a current of 150 mA?

Consider the following standard reduction potentials: Ni2+(aq)+ 2 e- → Ni(s)E° = -0.26 V I2(s)+ 2 e- → 2 I-(aq)E° = +0.54 V Under standard conditions:

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ → Ag(s)+ (aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 mol L-1 and 2.22 mol L-1,respectively.The cell emf is ________ V.

Choose the INCORRECT statement.

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s)∣ Zn2+(aq)∣∣ Ni2+(aq)∣ Ni(s)

What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe2+(aq)+ F2(g)→ 2 Fe3+(aq)+ 2 F-(aq)

A voltaic cell is constructed with two -Zn electrodes,where the half-reaction is (aq)+ → Zn(s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 mol L-1 and 1.11 × Mol L-1,respectively.The cell emf is ________ V.

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What is the concentration of Cu²⁺(aq)in the following cell at 25 °C if the cell voltage is 1.253 V? Zn(s)∣ Zn²⁺ (aq,0.125 M) Cu²⁺(?)∣ Cu(s) Cu²⁺(aq)+ 2 e^- → Cu(s)E° = 0.340 V Zn²⁺(aq)+ 2 e^- → Zn(s)E° = -0.763 V

What is E° of the spontaneous cell made from the Zn²⁺(aq)^/Zn(s)(-0.76 V)and Br₂(l)_/2 Br^-(aq)(1.07 V)half cells?

Determine E°_cell for the reaction: Pb(s)+ Zn²⁺(aq)→ Pb²⁺(aq)+ Zn(s). The half reactions are: Pb²⁺(aq)+ 2 e^- → Pb(s)E° = -0.125 V Zn²+(aq)+ 2 e^- → Zn(s)E° = -0.763 V

What is the standard cell potential if the Gibbs energy is -2108 kJ in the reaction: C₃H₈(g)+ O₂(g)→ CO₂(g)+ H₂O(l)(not balanced)?

Consider the cell: Ni(s)∣ Ni²⁺ (aq,?M) Cu²⁺ (aq,0.136 M)∣ Cu(s) Ni²⁺(aq)/Ni(s) E° = -0.257 V Cu²⁺(aq)/Cu(s) E° = 0.340 V The measured potential of the cell is 0.621 V.What is [Ni^2+] at 25 °C?

Two cells containing solutions of AgNO₃(aq)and CuSO₄(aq),respectively,were connected in series and electrolyzed.The cathode in the AgNO₃(aq)cell was found to gain 1.078 grams in weight.How much had the cathode in the other cell gained?

What is K_eqat 25 °C of the spontaneous cell made from Ag⁺(aq)/Ag(s)(0.80 V)and Cl₂(g)/Cl^-(aq)(1.36 V)half cells?

Given that E°_red = -1.66 V for Al³⁺(aq)/Al(s)at 25 °C,find E° and E for the concentration cell expressed using shorthand notation below: Al(s)∣ Al³⁺(aq,1.0 × 10^-5 mol L^-1)∣∣ Al³⁺(aq,0.100 mol L^-1)∣ Al(s)

Determine E°_cell at 25 °C for the following reaction: Pb²⁺(aq)+ Cu(s)→ Cu²⁺(aq)+ Pb(s) The half-reactions are: Pb²⁺(aq)+ 2 e^- → Pb(s)E° = -0.125 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = +0.337 V

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni²⁺(aq)∣∣ Cl₂(g)∣ Cl^-(aq)∣ C(s)

Consider the following standard reduction potentials: Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.26 V I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Under standard conditions:

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ → Ag(s)+ (aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 mol L^-1 and 2.22 mol L^-1,respectively.The cell emf is ________ V.

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s)∣ Zn²⁺(aq)∣∣ Ni²⁺(aq)∣ Ni(s)

What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe²⁺(aq)+ F₂(g)→ 2 Fe³⁺(aq)+ 2 F^-(aq)

A voltaic cell is constructed with two -Zn electrodes,where the half-reaction is (aq)+ → Zn(s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 mol L^-1 and 1.11 × Mol L^-1,respectively.The cell emf is ________ V.