Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows:
Cu²⁺(aq) + 2 e^- ? Cu(s)
E° = +0.337 V
AgCl(s) + e^- ? Ag(s) + Cl^-(aq)
E° = +0.222 V

Question

Calculate

E _ { \text {cell } } ^ { \circ }

for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows:
Cu²⁺(aq) + 2 e^- ? Cu(s)
E° = +0.337 V
AgCl(s) + e^- ? Ag(s) + Cl^-(aq)
E° = +0.222 V

Quizplus · Accepted Answer

The cell potential is calculated by subtracting the anode potential from the cathode potential: $E _ { \text {cell } } ^ { \circ } = E _ { \text {cathode } } ^ { \circ } - E _ { \text {anode } } ^ { \circ }$. Here, the cathode is Cu with $E° = +0.337 \, \text{V}$ and the anode is AgCl with $E° = +0.222 \, \text{V}$. Thus, $E _ { \text {cell } } ^ { \circ } = 0.337 \, \text{V} - 0.222 \, \text{V} = +0.115 \, \text{V}$.

Calculate Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​

Calculate $E _ { \text {cell } } ^ { \circ }$