Standard free energies of formation (in $kJ/mol$) at $298 \ K$ are $-237.2$,$-394.4$,and $-8.2$ for $H_2O_{(l)}$,$CO_{2_{(g)}}$,and pentane$_{(g)}$ respectively. The value of $E^o_{cell}$ for the pentane-oxygen fuel cell is .......... $V$.

Standard electrode potentials of $Zn$ and $Fe$ are known to be $(i) -0.76 \ V$ and $(ii) -0.44 \ V$ respectively. How does this explain that galvanization prevents rusting of iron while zinc slowly dissolves away?

$A$ hypothetical galvanic cell is $A_{(s)} | A^{+}_{(1 \ M)} || B^{+2}_{(1 \ M)} | B_{(s)}$ and the $EMF$ of the cell is positive. What is the possible cell reaction?

Which of the following hot aqueous solutions is used to dip carbon rods of $H_2 - O_2$ fuel cell?

$Cu^{+}_{(aq)}$ is unstable in solution and undergoes simultaneous oxidation and reduction,according to the reaction $2 Cu^{+}_{(aq)} \rightleftharpoons Cu^{2+}_{(aq)} + Cu_{(s)}$. Choose the correct $E^{\circ}$ for the above reaction if $E^{\circ}_{Cu^{2+}/Cu} = 0.34 \ V$ and $E^{\circ}_{Cu^{2+}/Cu^{+}} = 0.15 \ V$.

Which of the following is incorrect in a galvanic cell?