275909 In a galvanic cell the following reaction takes place at $298 \mathrm{~K}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{Fe}^{2+} \rightarrow 2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}$
Given that : $\mathrm{E}^{\mathrm{o}}\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}, \mathrm{H}^{+}, \mathrm{Cr}^{3+} / \mathrm{Pt}\right)=1.33 \mathrm{~V}$
$\mathrm{E}^{\mathrm{o}}\left(\mathrm{Fe}^{3+}, \mathrm{Fe}^{2+} / \mathrm{Pt}\right)=\mathbf{0 . 7 7} \mathrm{V}$
The standard e.m.f. of the cell is

275910 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is $\mathbf{0 . 5 9}$ $V$. The equilibrium constant for the redox reaction of the cell is

275911 The standard redox potentials for the reactions $\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}$ and $\mathrm{Mn}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}$ are $1.18 \mathrm{~V}$ and $1.51 \mathrm{~V}$ respectively. What is the redox potential for the reaction $\mathrm{Mn}^{3+}+3 \mathrm{e}^{-} \rightarrow$ Mn?

275912 The standard reduction potential for $\mathrm{Fe}^{2+} / \mathrm{Fe}$ and $\mathrm{Sn}^{2+} / \mathrm{Sn}$ electrodes are -0.44 and $-0.14 \mathrm{~V}$ respectively. For the cell reaction, $\mathrm{Fe}^{2+}+\mathrm{Sn} \rightarrow$ $\mathrm{Fe}+\mathrm{Sn}^{2+}$ the standard emf is

275909 In a galvanic cell the following reaction takes place at $298 \mathrm{~K}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{Fe}^{2+} \rightarrow 2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}$
Given that : $\mathrm{E}^{\mathrm{o}}\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}, \mathrm{H}^{+}, \mathrm{Cr}^{3+} / \mathrm{Pt}\right)=1.33 \mathrm{~V}$
$\mathrm{E}^{\mathrm{o}}\left(\mathrm{Fe}^{3+}, \mathrm{Fe}^{2+} / \mathrm{Pt}\right)=\mathbf{0 . 7 7} \mathrm{V}$
The standard e.m.f. of the cell is

275910 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is $\mathbf{0 . 5 9}$ $V$. The equilibrium constant for the redox reaction of the cell is

275911 The standard redox potentials for the reactions $\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}$ and $\mathrm{Mn}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}$ are $1.18 \mathrm{~V}$ and $1.51 \mathrm{~V}$ respectively. What is the redox potential for the reaction $\mathrm{Mn}^{3+}+3 \mathrm{e}^{-} \rightarrow$ Mn?

275912 The standard reduction potential for $\mathrm{Fe}^{2+} / \mathrm{Fe}$ and $\mathrm{Sn}^{2+} / \mathrm{Sn}$ electrodes are -0.44 and $-0.14 \mathrm{~V}$ respectively. For the cell reaction, $\mathrm{Fe}^{2+}+\mathrm{Sn} \rightarrow$ $\mathrm{Fe}+\mathrm{Sn}^{2+}$ the standard emf is

275909 In a galvanic cell the following reaction takes place at $298 \mathrm{~K}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{Fe}^{2+} \rightarrow 2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}$
Given that : $\mathrm{E}^{\mathrm{o}}\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}, \mathrm{H}^{+}, \mathrm{Cr}^{3+} / \mathrm{Pt}\right)=1.33 \mathrm{~V}$
$\mathrm{E}^{\mathrm{o}}\left(\mathrm{Fe}^{3+}, \mathrm{Fe}^{2+} / \mathrm{Pt}\right)=\mathbf{0 . 7 7} \mathrm{V}$
The standard e.m.f. of the cell is

275910 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is $\mathbf{0 . 5 9}$ $V$. The equilibrium constant for the redox reaction of the cell is

275911 The standard redox potentials for the reactions $\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}$ and $\mathrm{Mn}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}$ are $1.18 \mathrm{~V}$ and $1.51 \mathrm{~V}$ respectively. What is the redox potential for the reaction $\mathrm{Mn}^{3+}+3 \mathrm{e}^{-} \rightarrow$ Mn?

275912 The standard reduction potential for $\mathrm{Fe}^{2+} / \mathrm{Fe}$ and $\mathrm{Sn}^{2+} / \mathrm{Sn}$ electrodes are -0.44 and $-0.14 \mathrm{~V}$ respectively. For the cell reaction, $\mathrm{Fe}^{2+}+\mathrm{Sn} \rightarrow$ $\mathrm{Fe}+\mathrm{Sn}^{2+}$ the standard emf is

275909 In a galvanic cell the following reaction takes place at $298 \mathrm{~K}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+14 \mathrm{H}^{+}+6 \mathrm{Fe}^{2+} \rightarrow 2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}$
Given that : $\mathrm{E}^{\mathrm{o}}\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}, \mathrm{H}^{+}, \mathrm{Cr}^{3+} / \mathrm{Pt}\right)=1.33 \mathrm{~V}$
$\mathrm{E}^{\mathrm{o}}\left(\mathrm{Fe}^{3+}, \mathrm{Fe}^{2+} / \mathrm{Pt}\right)=\mathbf{0 . 7 7} \mathrm{V}$
The standard e.m.f. of the cell is

275910 The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is $\mathbf{0 . 5 9}$ $V$. The equilibrium constant for the redox reaction of the cell is

275911 The standard redox potentials for the reactions $\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}$ and $\mathrm{Mn}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}$ are $1.18 \mathrm{~V}$ and $1.51 \mathrm{~V}$ respectively. What is the redox potential for the reaction $\mathrm{Mn}^{3+}+3 \mathrm{e}^{-} \rightarrow$ Mn?

275912 The standard reduction potential for $\mathrm{Fe}^{2+} / \mathrm{Fe}$ and $\mathrm{Sn}^{2+} / \mathrm{Sn}$ electrodes are -0.44 and $-0.14 \mathrm{~V}$ respectively. For the cell reaction, $\mathrm{Fe}^{2+}+\mathrm{Sn} \rightarrow$ $\mathrm{Fe}+\mathrm{Sn}^{2+}$ the standard emf is