275816 For the following transformation, the reduction half reaction is
$\mathrm{Sn}^{2+}+2 \mathrm{Hg}^{2+} \rightarrow \mathrm{Sn}^{4+}+\mathbf{H g}_{2}^{2+}$

275831 Calculate the standard free energy change for the reaction
$2 \mathrm{Ag}+2 \mathrm{H}^{+} \longrightarrow \mathrm{H}_{2}+2 \mathrm{Ag}^{+}$
$\mathrm{E}^{\circ}$ for $\mathrm{Ag}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}$ is $0.80 \mathrm{~V}$.

275836 The electrode potential, $\mathbf{E}^{\mathbf{0}}$, for the reduction of $\mathrm{MnO}_{4}^{-}$to $\mathrm{Mn}^{2+}$ in acidic medium is $+1.51 \mathrm{~V}$. Which of the following metal (s) will be oxidised? The reduction reaction and standard electrode potentials for $\mathrm{Zn}^{2+}, \mathbf{A g}^{+}$, and $\mathbf{A u}^{+}$are given as
$\begin{aligned}
& \mathrm{Zn}_{(\mathrm{aq})}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}_{(\mathrm{s})}, \mathrm{E}^{0}=-0.762 \mathrm{~V} \\
& \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Ag}_{(\mathrm{s})} \mathrm{E}^{\mathbf{0}}=+0.80 \mathrm{~V} \\
& \mathrm{Au}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Au}_{(\mathrm{s})}, \mathrm{E}^{0}=+1.69 \mathrm{~V}
\end{aligned}$

275841 The reaction is spontaneous if the cell potential is :

275816 For the following transformation, the reduction half reaction is
$\mathrm{Sn}^{2+}+2 \mathrm{Hg}^{2+} \rightarrow \mathrm{Sn}^{4+}+\mathbf{H g}_{2}^{2+}$

275831 Calculate the standard free energy change for the reaction
$2 \mathrm{Ag}+2 \mathrm{H}^{+} \longrightarrow \mathrm{H}_{2}+2 \mathrm{Ag}^{+}$
$\mathrm{E}^{\circ}$ for $\mathrm{Ag}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}$ is $0.80 \mathrm{~V}$.

275836 The electrode potential, $\mathbf{E}^{\mathbf{0}}$, for the reduction of $\mathrm{MnO}_{4}^{-}$to $\mathrm{Mn}^{2+}$ in acidic medium is $+1.51 \mathrm{~V}$. Which of the following metal (s) will be oxidised? The reduction reaction and standard electrode potentials for $\mathrm{Zn}^{2+}, \mathbf{A g}^{+}$, and $\mathbf{A u}^{+}$are given as
$\begin{aligned}
& \mathrm{Zn}_{(\mathrm{aq})}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}_{(\mathrm{s})}, \mathrm{E}^{0}=-0.762 \mathrm{~V} \\
& \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Ag}_{(\mathrm{s})} \mathrm{E}^{\mathbf{0}}=+0.80 \mathrm{~V} \\
& \mathrm{Au}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Au}_{(\mathrm{s})}, \mathrm{E}^{0}=+1.69 \mathrm{~V}
\end{aligned}$

275841 The reaction is spontaneous if the cell potential is :

275816 For the following transformation, the reduction half reaction is
$\mathrm{Sn}^{2+}+2 \mathrm{Hg}^{2+} \rightarrow \mathrm{Sn}^{4+}+\mathbf{H g}_{2}^{2+}$

275831 Calculate the standard free energy change for the reaction
$2 \mathrm{Ag}+2 \mathrm{H}^{+} \longrightarrow \mathrm{H}_{2}+2 \mathrm{Ag}^{+}$
$\mathrm{E}^{\circ}$ for $\mathrm{Ag}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}$ is $0.80 \mathrm{~V}$.

275836 The electrode potential, $\mathbf{E}^{\mathbf{0}}$, for the reduction of $\mathrm{MnO}_{4}^{-}$to $\mathrm{Mn}^{2+}$ in acidic medium is $+1.51 \mathrm{~V}$. Which of the following metal (s) will be oxidised? The reduction reaction and standard electrode potentials for $\mathrm{Zn}^{2+}, \mathbf{A g}^{+}$, and $\mathbf{A u}^{+}$are given as
$\begin{aligned}
& \mathrm{Zn}_{(\mathrm{aq})}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}_{(\mathrm{s})}, \mathrm{E}^{0}=-0.762 \mathrm{~V} \\
& \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Ag}_{(\mathrm{s})} \mathrm{E}^{\mathbf{0}}=+0.80 \mathrm{~V} \\
& \mathrm{Au}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Au}_{(\mathrm{s})}, \mathrm{E}^{0}=+1.69 \mathrm{~V}
\end{aligned}$

275841 The reaction is spontaneous if the cell potential is :

275816 For the following transformation, the reduction half reaction is
$\mathrm{Sn}^{2+}+2 \mathrm{Hg}^{2+} \rightarrow \mathrm{Sn}^{4+}+\mathbf{H g}_{2}^{2+}$

275831 Calculate the standard free energy change for the reaction
$2 \mathrm{Ag}+2 \mathrm{H}^{+} \longrightarrow \mathrm{H}_{2}+2 \mathrm{Ag}^{+}$
$\mathrm{E}^{\circ}$ for $\mathrm{Ag}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}$ is $0.80 \mathrm{~V}$.

275836 The electrode potential, $\mathbf{E}^{\mathbf{0}}$, for the reduction of $\mathrm{MnO}_{4}^{-}$to $\mathrm{Mn}^{2+}$ in acidic medium is $+1.51 \mathrm{~V}$. Which of the following metal (s) will be oxidised? The reduction reaction and standard electrode potentials for $\mathrm{Zn}^{2+}, \mathbf{A g}^{+}$, and $\mathbf{A u}^{+}$are given as
$\begin{aligned}
& \mathrm{Zn}_{(\mathrm{aq})}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}_{(\mathrm{s})}, \mathrm{E}^{0}=-0.762 \mathrm{~V} \\
& \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Ag}_{(\mathrm{s})} \mathrm{E}^{\mathbf{0}}=+0.80 \mathrm{~V} \\
& \mathrm{Au}_{(\mathrm{aq})}^{+}+\mathrm{e}^{-} \rightleftharpoons \mathrm{Au}_{(\mathrm{s})}, \mathrm{E}^{0}=+1.69 \mathrm{~V}
\end{aligned}$

275841 The reaction is spontaneous if the cell potential is :