Four metals $A$,$B$,$C$,and $D$ have Standard Reduction Potential $(SRP)$ values of $-3.05 \ V$,$-1.66 \ V$,$-0.40 \ V$,and $0.80 \ V$ respectively. Which is the strongest reducing agent?

The $E^{\circ}$ of $Ce^{4+} / Ce^{3+} = 1.6 \ V$ and $Fe^{3+} / Fe^{2+} = 0.77 \ V$. The $E^{\circ}$ of the reaction where $Fe^{3+}$ oxidises $Ce^{3+}$ is:

Which from the following is the correct relationship between standard Gibbs energy change and standard cell potential?

The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

The values of $E^0$ for metals $A$,$B$,and $C$ are $0.34 \ V$,$-0.80 \ V$,and $-0.46 \ V$ respectively. State the correct order for their ability to act as reducing agents.

Which of the following is the strongest oxidising agent?