275933 Calculate the reduction potential of a half-cell containing of platinum electrode immersed in 2.0 $\mathrm{M} \mathrm{Fe}^{2+}$ and $0.02 \mathrm{MFe}^{3+}$.
$\text { Given : } \begin{array}{r}
\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.771 \mathrm{~V} . \\
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}
\end{array}$

275934 The emf of the cell
$\mathrm{Ni}\left \vert\mathrm{Ni}^{2+}(\mathbf{1 . 0} \mathrm{M}) \ \vert \mathrm{Au}^{3+}(1.0 \mathrm{M})\right \vert \mathrm{Au}$
$\text { is }\left[\mathrm{E}_{\left(\mathrm{Ni}^{2+} / \mathrm{Ni}\right)}^{0}=-0.25 \mathrm{~V} \text { and } \mathrm{E}_{\left(\mathrm{Au}^{3+} / \mathrm{Au}\right)}^{0}=+1.5 \mathrm{~V}\right]$

275935 How long it will take to deposit $1.0 \mathrm{~g}$ of chromium when a current of 1.25 A flows through a solution of chromium (III) sulphate?
(Molar mass of $\mathrm{Cr}=\mathbf{5 2}$ )

275936 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 $V$. The equilibrium constant for the reaction of the cell is

275938 If the solution of copper sulphate in which a copper rod is immersed, is diluted 100 times, what is the change in electrode potential (Reduction)?

275933 Calculate the reduction potential of a half-cell containing of platinum electrode immersed in 2.0 $\mathrm{M} \mathrm{Fe}^{2+}$ and $0.02 \mathrm{MFe}^{3+}$.
$\text { Given : } \begin{array}{r}
\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.771 \mathrm{~V} . \\
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}
\end{array}$

275934 The emf of the cell
$\mathrm{Ni}\left \vert\mathrm{Ni}^{2+}(\mathbf{1 . 0} \mathrm{M}) \ \vert \mathrm{Au}^{3+}(1.0 \mathrm{M})\right \vert \mathrm{Au}$
$\text { is }\left[\mathrm{E}_{\left(\mathrm{Ni}^{2+} / \mathrm{Ni}\right)}^{0}=-0.25 \mathrm{~V} \text { and } \mathrm{E}_{\left(\mathrm{Au}^{3+} / \mathrm{Au}\right)}^{0}=+1.5 \mathrm{~V}\right]$

275935 How long it will take to deposit $1.0 \mathrm{~g}$ of chromium when a current of 1.25 A flows through a solution of chromium (III) sulphate?
(Molar mass of $\mathrm{Cr}=\mathbf{5 2}$ )

275936 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 $V$. The equilibrium constant for the reaction of the cell is

275938 If the solution of copper sulphate in which a copper rod is immersed, is diluted 100 times, what is the change in electrode potential (Reduction)?

275933 Calculate the reduction potential of a half-cell containing of platinum electrode immersed in 2.0 $\mathrm{M} \mathrm{Fe}^{2+}$ and $0.02 \mathrm{MFe}^{3+}$.
$\text { Given : } \begin{array}{r}
\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.771 \mathrm{~V} . \\
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}
\end{array}$

275934 The emf of the cell
$\mathrm{Ni}\left \vert\mathrm{Ni}^{2+}(\mathbf{1 . 0} \mathrm{M}) \ \vert \mathrm{Au}^{3+}(1.0 \mathrm{M})\right \vert \mathrm{Au}$
$\text { is }\left[\mathrm{E}_{\left(\mathrm{Ni}^{2+} / \mathrm{Ni}\right)}^{0}=-0.25 \mathrm{~V} \text { and } \mathrm{E}_{\left(\mathrm{Au}^{3+} / \mathrm{Au}\right)}^{0}=+1.5 \mathrm{~V}\right]$

275935 How long it will take to deposit $1.0 \mathrm{~g}$ of chromium when a current of 1.25 A flows through a solution of chromium (III) sulphate?
(Molar mass of $\mathrm{Cr}=\mathbf{5 2}$ )

275936 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 $V$. The equilibrium constant for the reaction of the cell is

275938 If the solution of copper sulphate in which a copper rod is immersed, is diluted 100 times, what is the change in electrode potential (Reduction)?

275933 Calculate the reduction potential of a half-cell containing of platinum electrode immersed in 2.0 $\mathrm{M} \mathrm{Fe}^{2+}$ and $0.02 \mathrm{MFe}^{3+}$.
$\text { Given : } \begin{array}{r}
\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.771 \mathrm{~V} . \\
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}
\end{array}$

275934 The emf of the cell
$\mathrm{Ni}\left \vert\mathrm{Ni}^{2+}(\mathbf{1 . 0} \mathrm{M}) \ \vert \mathrm{Au}^{3+}(1.0 \mathrm{M})\right \vert \mathrm{Au}$
$\text { is }\left[\mathrm{E}_{\left(\mathrm{Ni}^{2+} / \mathrm{Ni}\right)}^{0}=-0.25 \mathrm{~V} \text { and } \mathrm{E}_{\left(\mathrm{Au}^{3+} / \mathrm{Au}\right)}^{0}=+1.5 \mathrm{~V}\right]$

275935 How long it will take to deposit $1.0 \mathrm{~g}$ of chromium when a current of 1.25 A flows through a solution of chromium (III) sulphate?
(Molar mass of $\mathrm{Cr}=\mathbf{5 2}$ )

275936 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 $V$. The equilibrium constant for the reaction of the cell is

275938 If the solution of copper sulphate in which a copper rod is immersed, is diluted 100 times, what is the change in electrode potential (Reduction)?

275933 Calculate the reduction potential of a half-cell containing of platinum electrode immersed in 2.0 $\mathrm{M} \mathrm{Fe}^{2+}$ and $0.02 \mathrm{MFe}^{3+}$.
$\text { Given : } \begin{array}{r}
\mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{0}=0.771 \mathrm{~V} . \\
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}
\end{array}$

275934 The emf of the cell
$\mathrm{Ni}\left \vert\mathrm{Ni}^{2+}(\mathbf{1 . 0} \mathrm{M}) \ \vert \mathrm{Au}^{3+}(1.0 \mathrm{M})\right \vert \mathrm{Au}$
$\text { is }\left[\mathrm{E}_{\left(\mathrm{Ni}^{2+} / \mathrm{Ni}\right)}^{0}=-0.25 \mathrm{~V} \text { and } \mathrm{E}_{\left(\mathrm{Au}^{3+} / \mathrm{Au}\right)}^{0}=+1.5 \mathrm{~V}\right]$

275935 How long it will take to deposit $1.0 \mathrm{~g}$ of chromium when a current of 1.25 A flows through a solution of chromium (III) sulphate?
(Molar mass of $\mathrm{Cr}=\mathbf{5 2}$ )

275936 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 $V$. The equilibrium constant for the reaction of the cell is

275938 If the solution of copper sulphate in which a copper rod is immersed, is diluted 100 times, what is the change in electrode potential (Reduction)?