🤓 Based on our data, we think this question is relevant for Professor Bindell's class at UCF.
To solve for equilibrium constant, K:
Step 1. Calculate 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 = 0.46 V
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)