$A$ galvanic cell consists of a copper electrode and a standard hydrogen electrode. If $E^0_{(Cu^{2+}(aq)|Cu(s))} = +0.34 \text{ V}$, identify the reaction taking place at the positive electrode during the working of the cell.

Which of the following will have a standard oxidation potential less than $SHE$?

Consider the following relations for $EMF$ of an electrochemical cell:
$(i)$ $EMF$ of cell = (Oxidation potential of anode) $-$ (Reduction potential of cathode)
$(ii)$ $EMF$ of cell = (Oxidation potential of anode) $+$ (Reduction potential of cathode)
$(iii)$ $EMF$ of cell = (Reduction potential of anode) $+$ (Reduction potential of cathode)
$(iv)$ $EMF$ of cell = (Oxidation potential of anode) $-$ (Oxidation potential of cathode)
Which of the above relations are correct?

Which one of the following metals cannot evolve $H_2$ from acids,$H_2O$,or from its compounds?

The $E^0_{cell}$ of the cell $Al(s)|Al^{3+}(1M)||Pb^{2+}(1M)|Pb(s)$ is $1.5 \text{ V}$. If $E^0_{Pb^{2+}/Pb}$ is $-0.14 \text{ V}$, then $E^0_{Al^{3+}/Al}$ will be: (in $\text{ V}$)

Among the following metals,the strongest reducing agent is