# Problem: Using the standard reduction potentials listed in Appendix E in the textbook, calculate the equilibrium constant for each of the following reactions at 298 K.3Ce4+(aq) + Bi(s) + H2O(l)  →  3Ce3+(aq) + BiO+(aq) + 2H+(aq)

###### FREE Expert Solution
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###### FREE Expert Solution

Step 1:

3Ce4+ (aq) + 3 e-  3Ce3+(aq)                     E° = +1.61 V       E°  reduction  cathode

BiO+ (aq) + 2H+ (aq) + 3e Bi(s) + H2O(l)  E° = 0.32 V         E°  oxidation  anode

Step 2

cell = 1.29 V

Step 3

3Ce4+ (aq) + 3 e-  3Ce3+(aq)

Bi(s) + H2O(l) → BiO+ (aq) + 2H+ (aq) + 3e-

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3Ce4+ (aq) +Bi(s) + H2O(l)  3Ce3+(aq) + BiO+(aq) + 2H+(aq)

n = 3

93% (494 ratings)
###### Problem Details

Using the standard reduction potentials listed in Appendix E in the textbook, calculate the equilibrium constant for each of the following reactions at 298 K.

3Ce4+(aq) + Bi(s) + H2O(l)  →  3Ce3+(aq) + BiO+(aq) + 2H+(aq)

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