Final answer:
The ratio of [NO3–] to [NH4+] at 298 K can be determined using the Nernst equation. The Nernst equation is given by: E = E° – (0.0592/n) log(Q). Where E is the cell potential, E° is the standard cell potential, n is the number of electrons transferred, and Q is the reaction quotient.
Step-by-step explanation:
The ratio of [NO3–] to [NH4+] at 298 K can be determined using the Nernst equation. The Nernst equation is given by:
E = E° – (0.0592/n) log(Q)
Where E is the cell potential, E° is the standard cell potential, n is the number of electrons transferred, and Q is the reaction quotient.
In this case, the reaction quotient Q can be expressed as:
Q = [NO3–] / [NH4+]
We know that E = 0 because the reaction is at equilibrium. Substituting E = 0 and E° = –0.2710 V into the Nernst equation, we can solve for the ratio [NO3–] / [NH4+].