275824 The voltage of the cell consisting of $\mathrm{Li}(\mathrm{s})$ and $F_{2}(g)$ electrodes is $5.92 \mathrm{~V}$ at standard condition at $298 \mathrm{~K}$. What is the voltage if the electrolyte consists of $2 \mathrm{M} \mathrm{LiF}$.
(In 2=0.693, $\mathrm{R}=\mathbf{8 . 3 1 4} \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ and $\mathrm{F}=\mathbf{9 6 5 0 0}$ $\left(\right.$ mol $^{-1}$ )

275826 The $\mathrm{E}_{\text {red }}^{\circ}$ of $\mathrm{Ag}, \mathrm{Cu}, \mathrm{Co}$ and $\mathrm{Zn}$ are 0.799, 0.337, $-0.277,-0.762 \mathrm{~V}$ respectively, which of the following cells will have maximum cell emf ?

275828 What will be the $\mathrm{E}_{\text {cell }}$ for the given cell?
$\mathrm{Zn}\left \vert\mathrm{Zn}^{2+}(0.1 \mathrm{M})\right \vert\left \vert\mathrm{Cu}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Cu}$
Given : $\mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{0}=0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{cu}}^{0}=0.34 \mathrm{~V}$
Also predict whether the reaction is spontaneous or non-spontaneous.

275829 What will be the half-cell potential of a hydrogen electrode acting as an anode and dipped in a solution of $\mathbf{p H}=\mathbf{2}$ ?

275824 The voltage of the cell consisting of $\mathrm{Li}(\mathrm{s})$ and $F_{2}(g)$ electrodes is $5.92 \mathrm{~V}$ at standard condition at $298 \mathrm{~K}$. What is the voltage if the electrolyte consists of $2 \mathrm{M} \mathrm{LiF}$.
(In 2=0.693, $\mathrm{R}=\mathbf{8 . 3 1 4} \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ and $\mathrm{F}=\mathbf{9 6 5 0 0}$ $\left(\right.$ mol $^{-1}$ )

275826 The $\mathrm{E}_{\text {red }}^{\circ}$ of $\mathrm{Ag}, \mathrm{Cu}, \mathrm{Co}$ and $\mathrm{Zn}$ are 0.799, 0.337, $-0.277,-0.762 \mathrm{~V}$ respectively, which of the following cells will have maximum cell emf ?

275828 What will be the $\mathrm{E}_{\text {cell }}$ for the given cell?
$\mathrm{Zn}\left \vert\mathrm{Zn}^{2+}(0.1 \mathrm{M})\right \vert\left \vert\mathrm{Cu}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Cu}$
Given : $\mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{0}=0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{cu}}^{0}=0.34 \mathrm{~V}$
Also predict whether the reaction is spontaneous or non-spontaneous.

275829 What will be the half-cell potential of a hydrogen electrode acting as an anode and dipped in a solution of $\mathbf{p H}=\mathbf{2}$ ?

275824 The voltage of the cell consisting of $\mathrm{Li}(\mathrm{s})$ and $F_{2}(g)$ electrodes is $5.92 \mathrm{~V}$ at standard condition at $298 \mathrm{~K}$. What is the voltage if the electrolyte consists of $2 \mathrm{M} \mathrm{LiF}$.
(In 2=0.693, $\mathrm{R}=\mathbf{8 . 3 1 4} \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ and $\mathrm{F}=\mathbf{9 6 5 0 0}$ $\left(\right.$ mol $^{-1}$ )

275826 The $\mathrm{E}_{\text {red }}^{\circ}$ of $\mathrm{Ag}, \mathrm{Cu}, \mathrm{Co}$ and $\mathrm{Zn}$ are 0.799, 0.337, $-0.277,-0.762 \mathrm{~V}$ respectively, which of the following cells will have maximum cell emf ?

275828 What will be the $\mathrm{E}_{\text {cell }}$ for the given cell?
$\mathrm{Zn}\left \vert\mathrm{Zn}^{2+}(0.1 \mathrm{M})\right \vert\left \vert\mathrm{Cu}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Cu}$
Given : $\mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{0}=0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{cu}}^{0}=0.34 \mathrm{~V}$
Also predict whether the reaction is spontaneous or non-spontaneous.

275829 What will be the half-cell potential of a hydrogen electrode acting as an anode and dipped in a solution of $\mathbf{p H}=\mathbf{2}$ ?

275824 The voltage of the cell consisting of $\mathrm{Li}(\mathrm{s})$ and $F_{2}(g)$ electrodes is $5.92 \mathrm{~V}$ at standard condition at $298 \mathrm{~K}$. What is the voltage if the electrolyte consists of $2 \mathrm{M} \mathrm{LiF}$.
(In 2=0.693, $\mathrm{R}=\mathbf{8 . 3 1 4} \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ and $\mathrm{F}=\mathbf{9 6 5 0 0}$ $\left(\right.$ mol $^{-1}$ )

275826 The $\mathrm{E}_{\text {red }}^{\circ}$ of $\mathrm{Ag}, \mathrm{Cu}, \mathrm{Co}$ and $\mathrm{Zn}$ are 0.799, 0.337, $-0.277,-0.762 \mathrm{~V}$ respectively, which of the following cells will have maximum cell emf ?

275828 What will be the $\mathrm{E}_{\text {cell }}$ for the given cell?
$\mathrm{Zn}\left \vert\mathrm{Zn}^{2+}(0.1 \mathrm{M})\right \vert\left \vert\mathrm{Cu}^{2+}(0.01 \mathrm{M})\right \vert \mathrm{Cu}$
Given : $\mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{0}=0.76 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{cu}}^{0}=0.34 \mathrm{~V}$
Also predict whether the reaction is spontaneous or non-spontaneous.

275829 What will be the half-cell potential of a hydrogen electrode acting as an anode and dipped in a solution of $\mathbf{p H}=\mathbf{2}$ ?