275843 Consider the single electrode process $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$ catalysed by platinum black electrode in $\mathrm{HCl}$ electrolyte. The potential of the electrode is $-0.059 \mathrm{~V}$. SHE. What is the concentration of the acid in the hydrogen half cell if the $\mathrm{H}_{2}$ pressure is 1 bar ? $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$

275844 Consider the following electrode processes of a cell,
$\mathrm{Cl}^{-} \rightarrow \frac{1}{2} \mathrm{Cl}_{2}+\mathrm{e}^{-}$
$\left[\mathrm{MCl}+\mathrm{e}^{-} \rightarrow \mathrm{M}+\mathrm{Cl}^{-}\right]$
If EMF of this cell is $-1.140 \mathrm{~V}$ and $E^{\circ}$ value of the cell is $-0.55 \mathrm{~V}$ at $298 \mathrm{~K}$, the value of the equilibrium constant of the sparingly soluble salt $\mathrm{MCl}$ is in the order of

275845 What is the standard potential of the $\mathrm{Tl}^{3} / \mathrm{TI}$ electrode?
$\mathrm{Tl}^{3+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Tl}^{+}, \mathrm{E}^{0}=1.26 \mathrm{~V}$
$\mathrm{Tl}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Tl}, \mathrm{E}^{0}=-\mathbf{0 . 3 3 6 \mathrm { V }}$

275846 Which option is incorrect for the working cell?
$\mathbf{P t}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{C l}_{\left(\mathrm{c}_{1}\right)}^{-} \vert \vert \mathbf{C l}_{\left(\mathfrak{c}_{2}\right)}^{-}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{P t}$
1 bar 1 bar

275843 Consider the single electrode process $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$ catalysed by platinum black electrode in $\mathrm{HCl}$ electrolyte. The potential of the electrode is $-0.059 \mathrm{~V}$. SHE. What is the concentration of the acid in the hydrogen half cell if the $\mathrm{H}_{2}$ pressure is 1 bar ? $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$

275844 Consider the following electrode processes of a cell,
$\mathrm{Cl}^{-} \rightarrow \frac{1}{2} \mathrm{Cl}_{2}+\mathrm{e}^{-}$
$\left[\mathrm{MCl}+\mathrm{e}^{-} \rightarrow \mathrm{M}+\mathrm{Cl}^{-}\right]$
If EMF of this cell is $-1.140 \mathrm{~V}$ and $E^{\circ}$ value of the cell is $-0.55 \mathrm{~V}$ at $298 \mathrm{~K}$, the value of the equilibrium constant of the sparingly soluble salt $\mathrm{MCl}$ is in the order of

275845 What is the standard potential of the $\mathrm{Tl}^{3} / \mathrm{TI}$ electrode?
$\mathrm{Tl}^{3+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Tl}^{+}, \mathrm{E}^{0}=1.26 \mathrm{~V}$
$\mathrm{Tl}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Tl}, \mathrm{E}^{0}=-\mathbf{0 . 3 3 6 \mathrm { V }}$

275846 Which option is incorrect for the working cell?
$\mathbf{P t}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{C l}_{\left(\mathrm{c}_{1}\right)}^{-} \vert \vert \mathbf{C l}_{\left(\mathfrak{c}_{2}\right)}^{-}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{P t}$
1 bar 1 bar

275843 Consider the single electrode process $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$ catalysed by platinum black electrode in $\mathrm{HCl}$ electrolyte. The potential of the electrode is $-0.059 \mathrm{~V}$. SHE. What is the concentration of the acid in the hydrogen half cell if the $\mathrm{H}_{2}$ pressure is 1 bar ? $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$

275844 Consider the following electrode processes of a cell,
$\mathrm{Cl}^{-} \rightarrow \frac{1}{2} \mathrm{Cl}_{2}+\mathrm{e}^{-}$
$\left[\mathrm{MCl}+\mathrm{e}^{-} \rightarrow \mathrm{M}+\mathrm{Cl}^{-}\right]$
If EMF of this cell is $-1.140 \mathrm{~V}$ and $E^{\circ}$ value of the cell is $-0.55 \mathrm{~V}$ at $298 \mathrm{~K}$, the value of the equilibrium constant of the sparingly soluble salt $\mathrm{MCl}$ is in the order of

275845 What is the standard potential of the $\mathrm{Tl}^{3} / \mathrm{TI}$ electrode?
$\mathrm{Tl}^{3+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Tl}^{+}, \mathrm{E}^{0}=1.26 \mathrm{~V}$
$\mathrm{Tl}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Tl}, \mathrm{E}^{0}=-\mathbf{0 . 3 3 6 \mathrm { V }}$

275846 Which option is incorrect for the working cell?
$\mathbf{P t}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{C l}_{\left(\mathrm{c}_{1}\right)}^{-} \vert \vert \mathbf{C l}_{\left(\mathfrak{c}_{2}\right)}^{-}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{P t}$
1 bar 1 bar

275843 Consider the single electrode process $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$ catalysed by platinum black electrode in $\mathrm{HCl}$ electrolyte. The potential of the electrode is $-0.059 \mathrm{~V}$. SHE. What is the concentration of the acid in the hydrogen half cell if the $\mathrm{H}_{2}$ pressure is 1 bar ? $4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{H}_{2}$

275844 Consider the following electrode processes of a cell,
$\mathrm{Cl}^{-} \rightarrow \frac{1}{2} \mathrm{Cl}_{2}+\mathrm{e}^{-}$
$\left[\mathrm{MCl}+\mathrm{e}^{-} \rightarrow \mathrm{M}+\mathrm{Cl}^{-}\right]$
If EMF of this cell is $-1.140 \mathrm{~V}$ and $E^{\circ}$ value of the cell is $-0.55 \mathrm{~V}$ at $298 \mathrm{~K}$, the value of the equilibrium constant of the sparingly soluble salt $\mathrm{MCl}$ is in the order of

275845 What is the standard potential of the $\mathrm{Tl}^{3} / \mathrm{TI}$ electrode?
$\mathrm{Tl}^{3+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Tl}^{+}, \mathrm{E}^{0}=1.26 \mathrm{~V}$
$\mathrm{Tl}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Tl}, \mathrm{E}^{0}=-\mathbf{0 . 3 3 6 \mathrm { V }}$

275846 Which option is incorrect for the working cell?
$\mathbf{P t}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{C l}_{\left(\mathrm{c}_{1}\right)}^{-} \vert \vert \mathbf{C l}_{\left(\mathfrak{c}_{2}\right)}^{-}\left \vert\mathbf{C l}_{2(\mathrm{~g})}\right \vert \mathbf{P t}$
1 bar 1 bar