# 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:

.

$\overline{){\mathbf{∆}}{\mathbf{G}}{\mathbf{°}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{°}}}_{{\mathbf{cell}}}}$

$\overline{){\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{anode}}}}$

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 = 0.46 V

###### 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)