The overall reaction 2Co³⁺(aq)+ 2Cl^-(aq)$\rarr$ 2Co²⁺(aq)+ Cl₂(g)has the standard cell voltage E°_cell= 0.46 V.Given E° = 1.36 V for the reaction Cl₂(g)+ 2e^- $\rarr$2Cl^-(aq), calculate the standard reduction potential for the following the half reaction at 25°C: Co³⁺ + e^- $\rarr$ Co²⁺

Question

Quizplus · Accepted Answer

We can use the equation: 
E°cell = E°cathode - E°anode 
where E°cathode is the standard reduction potential for the cathode half-reaction and E°anode is the standard reduction potential for the anode half-reaction.

In this case, we know: 
E°cell = 0.46 V 
E°anode = -1.36 V (from the given reduction potential for Cl2)

To find E°cathode, we can rearrange the equation: 
E°cathode = E°cell + E°anode 
E°cathode = 0.46 V + (-1.36 V) 
E°cathode = -0.90 V

Therefore, the answer is choice A) 1.82 V, which is the reduction potential for the half-reaction: 
Co3+ + e- --> Co2+ 
(Note that the given equation in the question is not a half-reaction, but a balanced overall equation that involves both a cathode and an anode half-reaction.)

The Overall Reaction 2Co3+(aq)+ 2Cl-(aq) →\rarr→ 2Co2+(aq)+ Cl2(g)has the Standard Cell Voltage E°cell= 0

The Overall Reaction 2Co³⁺(aq)+ 2Cl^-(aq) $\rarr$ 2Co²⁺(aq)+ Cl₂(g)has the Standard Cell Voltage E°_cell= 0