The Nernst equation for a half-cell reaction at 298 K is:

Full form: $E = E^{\circ} - \dfrac{RT}{nF} \ln Q$. At 298 K with $\log_{10}$, the constants collapse to $\dfrac{0.0592}{n}$, often rounded to $\dfrac{0.059}{n}$. Here $n$ is the number of electrons exchanged in the half-cell, and $Q$ is the reaction quotient. The negative sign matters: when $Q > 1$ (products dominate), $E$ is below $E^{\circ}$. Option B has the wrong sign; option D scrambles where $n$ goes.