Question 1
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C. (The equation is balanced.)
Pb(
s) + Br
2(
l) → Pb
2+(
aq) + 2 Br⁻(
aq)
| Pb2+(aq) + 2 e⁻ → Pb(s) | E° = -0.13 V |
| Br2(l) + 2 e⁻ → 2 Br⁻(aq) | E° = +1.07 V |
◦ -0.60 V
◦ -1.20 V
◦ -0.94 V
◦ +0.94 V
◦ +1.20 V
Question 2
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.)
Sn(
s) + 2Ag⁺(
aq) → Sn
2+(
aq) + 2Ag(
s)
| Sn2+(aq) + 2 e⁻ → Sn(s) | E° = -0.14 V |
| Ag⁺(aq) + e⁻ → Ag(s) | E° = +0.80 V |
◦ +1.08 V
◦ -1.08 V
◦ +0.94 V
◦ +1.74 V
◦ -1.74 V
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