275784 In the electrolysis of a $\mathrm{CuSO}_{4}$ solution, how many grams of $\mathrm{Cu}$ are plated out on the cathode, in the time that is required to liberate 5.6 $\mathrm{L}$ of $\mathrm{O}_{2}(\mathrm{~g})$, measured at $1 \mathrm{~atm}$ and 273 . $\mathrm{K}$, at the anode?

275786 For the reaction $\mathrm{Sn}(\mathrm{s})\left \vert\mathrm{Sn}^{2+}(0.10 \mathrm{M})\right \vert$ $\mathrm{Pb}^{2+}(0.5 \mathrm{M}) \mid \mathrm{Pb}(\mathrm{s})$. What will be approximate $\mathrm{E}_{\text {cell }}$ when $\left[\mathrm{Pb}^{2+}\right]$ is $0.1 \mathrm{M}$ (given $\mathrm{E}_{\mathrm{Sn}^{2+/ \mathrm{Sn}}}^0=-0.136 \mathrm{~V}: \mathrm{E}_{\mathrm{Pb}^{2+} / \mathrm{Pb}^{\mathrm{b}}}^{\mathrm{0}}=-0.126 \mathrm{~V}$ )

275787 For the cell reaction $3 \mathrm{Sn}^{4+}+2 \mathrm{Cr} \rightarrow 3 \mathrm{Sn}^{2+}+2 \mathrm{Cr}^{3+}, \mathrm{E}_{\text {cell }}^{0}$ is $0.89 \mathrm{~V}$.
Then $\Delta \mathbf{G}^{\mathbf{0}}$ for the reaction is ....... .

275799 Calculate emf of cell at $25^{\circ} \mathrm{C}$ if value of $E_{\text {cell }}^{\circ}$ is 4
volt $\left(\right.$ Given $\frac{R T}{F}$ in $\left.10=0.06\right)$
Cell notation : $\left.\mathbf{M}\left \vert\mathbf{M}_{0.01}{ }^{2+}\right \vert\right \vert_{0.0001} \mathbf{M}^{2+} \mid \mathbf{M}$

275784 In the electrolysis of a $\mathrm{CuSO}_{4}$ solution, how many grams of $\mathrm{Cu}$ are plated out on the cathode, in the time that is required to liberate 5.6 $\mathrm{L}$ of $\mathrm{O}_{2}(\mathrm{~g})$, measured at $1 \mathrm{~atm}$ and 273 . $\mathrm{K}$, at the anode?

275786 For the reaction $\mathrm{Sn}(\mathrm{s})\left \vert\mathrm{Sn}^{2+}(0.10 \mathrm{M})\right \vert$ $\mathrm{Pb}^{2+}(0.5 \mathrm{M}) \mid \mathrm{Pb}(\mathrm{s})$. What will be approximate $\mathrm{E}_{\text {cell }}$ when $\left[\mathrm{Pb}^{2+}\right]$ is $0.1 \mathrm{M}$ (given $\mathrm{E}_{\mathrm{Sn}^{2+/ \mathrm{Sn}}}^0=-0.136 \mathrm{~V}: \mathrm{E}_{\mathrm{Pb}^{2+} / \mathrm{Pb}^{\mathrm{b}}}^{\mathrm{0}}=-0.126 \mathrm{~V}$ )

275787 For the cell reaction $3 \mathrm{Sn}^{4+}+2 \mathrm{Cr} \rightarrow 3 \mathrm{Sn}^{2+}+2 \mathrm{Cr}^{3+}, \mathrm{E}_{\text {cell }}^{0}$ is $0.89 \mathrm{~V}$.
Then $\Delta \mathbf{G}^{\mathbf{0}}$ for the reaction is ....... .

275799 Calculate emf of cell at $25^{\circ} \mathrm{C}$ if value of $E_{\text {cell }}^{\circ}$ is 4
volt $\left(\right.$ Given $\frac{R T}{F}$ in $\left.10=0.06\right)$
Cell notation : $\left.\mathbf{M}\left \vert\mathbf{M}_{0.01}{ }^{2+}\right \vert\right \vert_{0.0001} \mathbf{M}^{2+} \mid \mathbf{M}$

275784 In the electrolysis of a $\mathrm{CuSO}_{4}$ solution, how many grams of $\mathrm{Cu}$ are plated out on the cathode, in the time that is required to liberate 5.6 $\mathrm{L}$ of $\mathrm{O}_{2}(\mathrm{~g})$, measured at $1 \mathrm{~atm}$ and 273 . $\mathrm{K}$, at the anode?

275786 For the reaction $\mathrm{Sn}(\mathrm{s})\left \vert\mathrm{Sn}^{2+}(0.10 \mathrm{M})\right \vert$ $\mathrm{Pb}^{2+}(0.5 \mathrm{M}) \mid \mathrm{Pb}(\mathrm{s})$. What will be approximate $\mathrm{E}_{\text {cell }}$ when $\left[\mathrm{Pb}^{2+}\right]$ is $0.1 \mathrm{M}$ (given $\mathrm{E}_{\mathrm{Sn}^{2+/ \mathrm{Sn}}}^0=-0.136 \mathrm{~V}: \mathrm{E}_{\mathrm{Pb}^{2+} / \mathrm{Pb}^{\mathrm{b}}}^{\mathrm{0}}=-0.126 \mathrm{~V}$ )

275787 For the cell reaction $3 \mathrm{Sn}^{4+}+2 \mathrm{Cr} \rightarrow 3 \mathrm{Sn}^{2+}+2 \mathrm{Cr}^{3+}, \mathrm{E}_{\text {cell }}^{0}$ is $0.89 \mathrm{~V}$.
Then $\Delta \mathbf{G}^{\mathbf{0}}$ for the reaction is ....... .

275799 Calculate emf of cell at $25^{\circ} \mathrm{C}$ if value of $E_{\text {cell }}^{\circ}$ is 4
volt $\left(\right.$ Given $\frac{R T}{F}$ in $\left.10=0.06\right)$
Cell notation : $\left.\mathbf{M}\left \vert\mathbf{M}_{0.01}{ }^{2+}\right \vert\right \vert_{0.0001} \mathbf{M}^{2+} \mid \mathbf{M}$

275784 In the electrolysis of a $\mathrm{CuSO}_{4}$ solution, how many grams of $\mathrm{Cu}$ are plated out on the cathode, in the time that is required to liberate 5.6 $\mathrm{L}$ of $\mathrm{O}_{2}(\mathrm{~g})$, measured at $1 \mathrm{~atm}$ and 273 . $\mathrm{K}$, at the anode?

275786 For the reaction $\mathrm{Sn}(\mathrm{s})\left \vert\mathrm{Sn}^{2+}(0.10 \mathrm{M})\right \vert$ $\mathrm{Pb}^{2+}(0.5 \mathrm{M}) \mid \mathrm{Pb}(\mathrm{s})$. What will be approximate $\mathrm{E}_{\text {cell }}$ when $\left[\mathrm{Pb}^{2+}\right]$ is $0.1 \mathrm{M}$ (given $\mathrm{E}_{\mathrm{Sn}^{2+/ \mathrm{Sn}}}^0=-0.136 \mathrm{~V}: \mathrm{E}_{\mathrm{Pb}^{2+} / \mathrm{Pb}^{\mathrm{b}}}^{\mathrm{0}}=-0.126 \mathrm{~V}$ )

275787 For the cell reaction $3 \mathrm{Sn}^{4+}+2 \mathrm{Cr} \rightarrow 3 \mathrm{Sn}^{2+}+2 \mathrm{Cr}^{3+}, \mathrm{E}_{\text {cell }}^{0}$ is $0.89 \mathrm{~V}$.
Then $\Delta \mathbf{G}^{\mathbf{0}}$ for the reaction is ....... .

275799 Calculate emf of cell at $25^{\circ} \mathrm{C}$ if value of $E_{\text {cell }}^{\circ}$ is 4
volt $\left(\right.$ Given $\frac{R T}{F}$ in $\left.10=0.06\right)$
Cell notation : $\left.\mathbf{M}\left \vert\mathbf{M}_{0.01}{ }^{2+}\right \vert\right \vert_{0.0001} \mathbf{M}^{2+} \mid \mathbf{M}$