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2 Ag(s) + Cu?+ (aq) → 2 Ag* (aq) + Cu(s) Half-Reaction Standard Reduction Potential, E (V) Ag+ (aq) + e -→ Ag(s) +0.80 Cu²+ (ag) + 2 e → Cu(s) +0.34 The reaction represented by the equation above serves as the basis for the construction of an electrochemical cell. The table gives the reduction half-reactions and their respective standard reduction potentials. Based on the overall reaction, which type of electrochemical cell was constructed, and why? A A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 + 0.34=+1.14 V. B A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 - 0.34= +0,46 V. 96,500 (-0,46) = 44 kJ /mol and its operation requires a potential smaller than 0.46 V to be supplied. C An electrolytic cell, because AG = 1,000 An electrolytic cell, because AG 2 x 96,500 (-0.40) 89 kJ/mol and its operation requires a potential greater than 0.46 V to be supplied. D 1,000

2 Ag(s) + Cu?+ (aq) → 2 Ag* (aq) + Cu(s) Half-Reaction Standard Reduction Potential, E (V) Ag+ (aq) + e -→ Ag(s) +0.80 Cu²+ (ag) + 2 e → Cu(s) +0.34 The reaction represented by the equation above serves as the basis for the construction of an electrochemical cell. The table gives the reduction half-reactions and their respective standard reduction potentials. Based on the overall reaction, which type of electrochemical cell was constructed, and why? A A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 + 0.34=+1.14 V. B A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 - 0.34= +0,46 V. 96,500 (-0,46) = 44 kJ /mol and its operation requires a potential smaller than 0.46 V to be supplied. C An electrolytic cell, because AG = 1,000 An electrolytic cell, because AG 2 x 96,500 (-0.40) 89 kJ/mol and its operation requires a potential greater than 0.46 V to be supplied. D 1,000

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2 Ag(s) + Cu?+ (aq) → 2 Ag* (aq) + Cu( s) Half-Reaction Standard Reduction Potential, E" (V) Ag+ (aq) + e -→ Ag(s) Cu?+ (ag) + 2 e → Cu(s) +0.80 +0.34 The reaction represented by the equation above serves as the basis for the construction of an electrochemical cell. The table gives the reduction half-reactions and their respective standard reduction potentials. Based on the overall reaction, which type of electrochemical cell was constructed, and why? A A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 + 0.34 =+1.14 V. B A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 - 0.34 = +0,46 V. 96,500 x (-0.46) 44 kJ /mol.. and its operation requires a potential smaller than 0.46 V to be supplied. An electrolytic cell, because AG = 1,000 2 x 96,500 x (-0.46) An electrolytic cell, because AG = = 89 kJ /mol and its operation requires a potential greater than 0.46 V to be supplied. D 1,000
Transcribed Image Text:2 Ag(s) + Cu?+ (aq) → 2 Ag* (aq) + Cu( s) Half-Reaction Standard Reduction Potential, E" (V) Ag+ (aq) + e -→ Ag(s) Cu?+ (ag) + 2 e → Cu(s) +0.80 +0.34 The reaction represented by the equation above serves as the basis for the construction of an electrochemical cell. The table gives the reduction half-reactions and their respective standard reduction potentials. Based on the overall reaction, which type of electrochemical cell was constructed, and why? A A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 + 0.34 =+1.14 V. B A galvanic or voltaic cell, because the standard reduction potentials for the two half-reactions are positive and E = 0.80 - 0.34 = +0,46 V. 96,500 x (-0.46) 44 kJ /mol.. and its operation requires a potential smaller than 0.46 V to be supplied. An electrolytic cell, because AG = 1,000 2 x 96,500 x (-0.46) An electrolytic cell, because AG = = 89 kJ /mol and its operation requires a potential greater than 0.46 V to be supplied. D 1,000
2 H2(g) + O2(g) → 2 H2O(1) = -474 kJ/moln AG rzn Half-Reaction Standard Reduction Potential (V) Electrode ? Cathode O2(g) + 4 H+(aq) + 4 e- → 2 H,O(!) 0.00 Anode 2 H*(ag) + 2 e → H2(g) The operation of a hydrogen fuel cell under standard conditions relies on the chemical reaction represented above. The table provides the relevant reduction half-reactions and the standard reduction potentials. Based on the information given, which of the following equations can be used to calculate the standard reduction potential, in volts, of the half-reaction occurring at the cathode? E" rea(cathode) = (00) A E red (cathode) = 474,000 4x 96,500 B 4 x 96,500 E red (cathode)= 474 E" red(cathode) = -(00.500) D -474,000
Transcribed Image Text:2 H2(g) + O2(g) → 2 H2O(1) = -474 kJ/moln AG rzn Half-Reaction Standard Reduction Potential (V) Electrode ? Cathode O2(g) + 4 H+(aq) + 4 e- → 2 H,O(!) 0.00 Anode 2 H*(ag) + 2 e → H2(g) The operation of a hydrogen fuel cell under standard conditions relies on the chemical reaction represented above. The table provides the relevant reduction half-reactions and the standard reduction potentials. Based on the information given, which of the following equations can be used to calculate the standard reduction potential, in volts, of the half-reaction occurring at the cathode? E" rea(cathode) = (00) A E red (cathode) = 474,000 4x 96,500 B 4 x 96,500 E red (cathode)= 474 E" red(cathode) = -(00.500) D -474,000
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