Question

1.) For the complete balanced redox reaction below, what is the E^o_cell?

Zn(s) + 2Cu⁺(aq) ⟶ 2Cu(s) + Zn²⁺(aq)

Zn²⁺ + 2e-   Zn(s) E^o = -0.76 V

Cu⁺ + e-  Cu(s) E^o = 0.52

• A) -1.28 V
• B) +1.28 V
• C) 0.24 V
• D) -0.24 V
• E) +2.56 V

2.) For the redox reaction below, what is the E_cell if [Zn²⁺] = 0.072 M and [Cu⁺] = 1.27 M?
T = 298 K

Zn(s) + 2Cu⁺(aq) ⟶ 2Cu(s) + Zn²⁺(aq)

Half Reactions:

Zn²⁺ + 2e-   Zn(s) E^o = -0.76 V

Cu⁺ + e-  Cu(s) E^o = 0.52

• A) +1.32 V
• B) +1.28 V
• C) +1.17 V
• D) +1.22 V
• E) +1.24 V