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.Cu(s) + 2Ag+(aq)  →  Cu2+(aq) + 2Ag(s)

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FREE Expert Solution

To solve for equilibrium constant, K:


G°=-RT ln K

.

G°=-nFE°cell


-RT ln K=-nFE°cell

E°cell=E°cathode-E°anode


Step 1Calculate E°cell.

Ag+(aq) + e- → Ag(s)                        ↑ E° = 0.80 V                  cathode

Cu2+(aq) + 2 e- → Cu(s)                    E° = 0.34 V                    anode


E°cell=E°cathode-E°anodeE°cell=0.80 V -0.34 V  

  E°cell = 0.46 V

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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.

Cu(s) + 2Ag+(aq)  →  Cu2+(aq) + 2Ag(s)