If the standard $emf$ of the cell $Zn_{(s)} | Zn_{(1 \ M)}^{+2} || Ag_{(1 \ M)}^{+1} | Ag_{(s)}$ is $1.55 \ V$, what is the electrical work done under standard conditions (in $kJ$)?

If $\Lambda _{NaCl}^{o}=126\,S\,cm^{2}mol^{-1}$,$\Lambda _{KBr}^{o}=152\,S\,cm^{2}mol^{-1}$,and $\Lambda _{KCl}^{o}=150\,S\,cm^{2}mol^{-1}$,then find $\Lambda ^{o}_{NaBr}$ in $S\,cm^{2}mol^{-1}$.

$A$ metal used in storage batteries is

$A$ solution containing $1 \ mol \ L^{-1}$ of each $Cu(NO_3)_2, AgNO_3, Hg_2(NO_3)_2$ and $Mg(NO_3)_2$ is being electrolysed using inert electrodes. The standard reduction potentials are $E^0_{Ag^{+}/Ag} = +0.80 \ V, E^0_{Hg_2^{2+}/Hg} = +0.79 \ V, E^0_{Cu^{2+}/Cu} = +0.34 \ V, E^0_{Mg^{2+}/Mg} = -2.37 \ V$. With increasing voltage,the sequence of deposition of metals on the cathode will be:

$A$ galvanic cell has an electrical potential of $1.1 \ V$. If an opposing potential of $1.1 \ V$ is applied to this cell,what will happen to the cell reaction and the current flowing through the cell?

Hydrogen-oxygen fuel cells are used in spacecraft to supply: