2 H2(g) + O2(g) → 2 H,0(1) ran = -474 kJ/mol AG Electrode Half-Reaction Standard Reduction Potentlal (V) 0,(g) + 4 H* (aq) + 4 e 2 H,0(1) 2 H*(aq) + 2 e- - H2(g) Cathode Anode 0.00 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 red (cathode) = 474 4x 06,500 E rea (cathode): -474,000 B 4x 06,500 () 96,500 E red (cathode) = 474 x96,500 D Ea(cathode) = 474.000 US O

2 H2(g) + O2(g) → 2 H,0(1) ran = -474 kJ/mol AG Electrode Half-Reaction Standard Reduction Potentlal (V) 0,(g) + 4 H* (aq) + 4 e 2 H,0(1) 2 H*(aq) + 2 e- - H2(g) Cathode Anode 0.00 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 red (cathode) = 474 4x 06,500 E rea (cathode): -474,000 B 4x 06,500 () 96,500 E red (cathode) = 474 x96,500 D Ea(cathode) = 474.000 US O

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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