Question

Calculate E o cell for the reaction: AgCl(s) + NO(g) → Ag(s) + Cl-(aq) + NO3-(aq) (in acidic solution) Use the fact that the reduction potential for nitrate(aq) to give NO(g) is +0.96 V and for AgCl(s) it is +0.22 V. You should give your answer with 1 digit before the decimal point and to 2 decimal places. Do NOT include units..... Also - do not use scientific notation!

Answer 1

Answer:

-0.74

Explanation:

Let's consider the following redox reaction.

AgCl(s) + NO(g) → Ag(s) + Cl⁻(aq) + NO₃⁻(aq)

We can identify the oxidation and reduction half-reactions.

Reduction (cathode): 1 e⁻ + AgCl(s) → Ag(s) + Cl⁻(aq)

Oxidation (anode): 2 H₂O(l) + NO(g) → NO₃⁻(aq) + 4H⁺(aq) + 3 e⁻

The standard cell potential (E°) is equal to the difference between the standard reduction potential of the cathode and the standard reduction potential of the anode.

E° = E°red,cat - Ered,an = 0.22 V - 0.96 V = -0.74 V