Which of the following metals behaves as the weakest reducing agent?
$E^\circ_{(\text{Li}^+/\text{Li})} = -3.05 \text{ V}$, $E^\circ_{(\text{Au}^{3+}/\text{Au})} = 1.40 \text{ V}$, $E^\circ_{(\text{Ag}^+/\text{Ag})} = 0.80 \text{ V}$, $E^\circ_{(\text{Mg}^{2+}/\text{Mg})} = -2.36 \text{ V}$

Give the symbolic representation of the following half-cells (electrodes):
$(i)$ $2H^{+}_{(aq)} + 2e^- \to H_{2_{(g)}}$
$(ii)$ $Br_{2_{(aq)}} + 2e^- \to 2Br^{-}_{(aq)}$
$(iii)$ $2Br^{-}_{(aq)} \to Br_{2_{(aq)}} + 2e^-$

Write the equation relating thermodynamics and electrochemistry.

The standard electrode potentials for $Ag^{+}/Ag$,$Hg_2^{2+}/2Hg$,$Cu^{2+}/Cu$,and $Mg^{2+}/Mg$ are $0.80 \, V$,$0.79 \, V$,$0.34 \, V$,and $-2.37 \, V$ respectively. If an aqueous solution containing $1 \, M$ concentration of each of these metal ions is electrolyzed,what is the correct order of metal deposition at the cathode as the voltage is increased?

When a $Zn$ piece is kept in a $CuSO_4$ solution,the copper gets precipitated because the standard reduction potential of zinc is

The standard electrode potentials of two half-cells are given as: $Ni^{2+}_{(aq)} + 2e^{-} \rightarrow Ni_{(s)}$; $E^o = -0.25 \ V$ and $Zn^{2+}_{(aq)} + 2e^{-} \rightarrow Zn_{(s)}$; $E^o = -0.76 \ V$. What is the standard $emf$ of the cell formed by connecting these two half-cells in $volt$?