2 Ag(s) + Cu?+ (aq) → 2 Ag* (aq) + Cu( s)Half-ReactionStandard Reduction Potential, E" (V)Ag+ (aq) + e -→ Ag(s)Cu?+ (ag) + 2 e → Cu(s)+0.80+0.34The 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 reductionpotentials. Based on the overall reaction, which type of electrochemical cell was constructed, and why?AA 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.BA 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 =1,0002 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.D1,000 2 H2(g) + O2(g) → 2 H2O(1)= -474 kJ/molnAGrznHalf-ReactionStandard Reduction Potential (V)Electrode?CathodeO2(g) + 4 H+(aq) + 4 e- → 2 H,O(!)0.00Anode2 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 reductionpotentials. 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)AE red (cathode) =474,0004x 96,500B4 x 96,500E red (cathode)=474E" red(cathode) = -(00.500)D-474,000

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

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

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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