(a) (i) What should be the signs (positive/negative) for E^°_Cell and Δ G^° for a spontaneous redox reaction occurring under standard conditions?…

What should be the signs (positive/negative) for $\displaystyle \mathrm{E}^{\circ}{ }_{\text {Cell }}$ and $\displaystyle \Delta \mathrm{G}^{\circ}$ for a spontaneous redox reaction occurring under standard conditions?

State Faraday's first law of electrolysis.

Calculate the emf of the following cell at $\displaystyle 298$ K: $\displaystyle \mathrm{Fe}_{(\mathrm{s})}\left|\mathrm{Fe}^{2+}(0.01 \mathrm{M})\right|\left|\mathrm{H}^{+}{ }_{(1 \mathrm{M})}\right| \mathrm{H}_{2(\mathrm{~g})}(1$ bar $\displaystyle ), \mathrm{Pt}_{(\mathrm{s})}$ Given $\displaystyle \mathrm{E}^{\circ}{ }_{\text {Cell }}=0.44 \mathrm{~V}$.