If the $\Delta G^o$ for the cell reaction $AgCl_{(s)} + \frac{1}{2} H_{2(g)} \rightarrow Ag_{(s)} + H^+ + Cl^-$ is $-21.52 \, kJ$,what will be the $\Delta G^o$ for the reaction $2AgCl_{(s)} + H_{2(g)} \rightarrow 2Ag_{(s)} + 2H^+ + 2Cl^-$ (in $, kJ$)?

All the energy released from the reaction $X \rightarrow Y, \Delta_{r}G^0 = -193 \ kJ \ mol^{-1}$ is used for oxidizing $M^{+}$ as $M^{+} \rightarrow M^{3+} + 2e^-, E^0 = -0.25 \ V$. Under standard conditions,the number of moles of $M^{+}$ oxidized when one mole of $X$ is converted to $Y$ is $\left[F = 96500 \ C \ mol^{-1}\right]$.

At $298 \, K$, the standard Gibbs free energy of formation for $H_2O_{(l)}$, $CO_{2(g)}$, and $C_5H_{12(g)}$ are $-237.2$, $-394.4$, and $-8.2 \, kJ \, mol^{-1}$ respectively. What is the potential of a pentane-oxygen fuel cell in $V$?

Consider the following electrochemical cell at standard condition: $Au_{(s)} | QH_2, Q | NH_4X(0.01 \ M) || Ag^{+}(1 \ M) | Ag_{(s)}$. Given $E_{\text{cell}} = +0.4 \ V$. The couple $QH_2 / Q$ represents the quinhydrone electrode,and the half-cell reaction is given as: $Q + 2e^- + 2H^+ \rightarrow QH_2$ with $E^o_{Q/QH_2} = +0.7 \ V$. Given: $E^o_{Ag^+/Ag} = +0.8 \ V$ and $\frac{2.303 \ RT}{F} = 0.06 \ V$. The $pK_b$ value of the ammonium halide salt $(NH_4X)$ used here is $.........$ (nearest integer).

What are the uses of standard half-cell potential?

During electrolysis of aqueous $NaOH$,$4 \ g$ of $O_2$ gas is liberated at $NTP$ at the anode. The volume of $H_2$ gas liberated at the cathode in $litres$ is $..............$