For the cell reaction,$Zn + Cu^{2+} \to Zn^{2+} + Cu,$ the cell representation is:

The standard Gibbs free energy change ($\Delta G^{\circ}$ in $kJ \, mol^{-1}$),in a $Daniell$ cell $(E^{\circ}_{cell} = 1.1 \, V)$,when $2 \, moles$ of $Zn_{(s)}$ is oxidised at $298 \, K$,is closest to

Standard electrode potentials for a few half cells are mentioned below:
$E^0_{Cu^{2+}/Cu} = 0.34 \ V, E^0_{Zn^{2+}/Zn} = -0.76 \ V$
$E^0_{Ag^{+}/Ag} = 0.80 \ V, E^0_{Mg^{2+}/Mg} = -2.37 \ V$
Which one of the following cells gives the most negative value of $\Delta G^0$?

In a galvanic cell,the salt bridge is used to:

Write a note on hydrogen-oxygen fuel cell.

Which of the following net cell reactions takes place in a galvanic cell containing a copper electrode and a standard hydrogen electrode $(SHE)$? Given: $E^{\circ}(Cu^{2+}_{(aq)} \mid Cu_{(s)}) = +0.34 \ V$.