275892 The emf of a galvanic cell constituted with the electrodes $\mathrm{Zn}^{2+} \mid \mathrm{Zn}(-0.76 \mathrm{~V})$ and $\mathrm{Fe}^{2+} \mid \mathrm{Fe}(-0.41$ $\mathrm{V})$ is

275895 Given that the standard reduction potentials for $\mathrm{M}^{+} / \mathrm{M}$ and $\mathrm{N}^{+} / \mathrm{N}$ electrodes at $298 \mathrm{~K}$ are 0.52 $\mathrm{V}$ and $0.25 \mathrm{~V}$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$\mathbf{M}\left \vert\mathbf{M}^{+} \ \vert \mathbf{N}^{+}\right \vert \mathbf{N}$

275898 In a cell that utilizes the reaction
$\mathbf{Z n}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
addition of $\mathrm{H}_{2} \mathrm{SO}_{4}$ to cathode compartment will.

275900 $\mathrm{Zn}(\mathrm{s})+\mathrm{Cl}_{2}(1 \mathrm{~atm}) \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{Cl}^{-} ; \mathrm{E}^{\circ}=2.0 \mathrm{~V}$.
To increase the e.m.f. of the above cell

275901 The reduction potential of an electrode can be increased by

275892 The emf of a galvanic cell constituted with the electrodes $\mathrm{Zn}^{2+} \mid \mathrm{Zn}(-0.76 \mathrm{~V})$ and $\mathrm{Fe}^{2+} \mid \mathrm{Fe}(-0.41$ $\mathrm{V})$ is

275895 Given that the standard reduction potentials for $\mathrm{M}^{+} / \mathrm{M}$ and $\mathrm{N}^{+} / \mathrm{N}$ electrodes at $298 \mathrm{~K}$ are 0.52 $\mathrm{V}$ and $0.25 \mathrm{~V}$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$\mathbf{M}\left \vert\mathbf{M}^{+} \ \vert \mathbf{N}^{+}\right \vert \mathbf{N}$

275898 In a cell that utilizes the reaction
$\mathbf{Z n}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
addition of $\mathrm{H}_{2} \mathrm{SO}_{4}$ to cathode compartment will.

275900 $\mathrm{Zn}(\mathrm{s})+\mathrm{Cl}_{2}(1 \mathrm{~atm}) \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{Cl}^{-} ; \mathrm{E}^{\circ}=2.0 \mathrm{~V}$.
To increase the e.m.f. of the above cell

275901 The reduction potential of an electrode can be increased by

275892 The emf of a galvanic cell constituted with the electrodes $\mathrm{Zn}^{2+} \mid \mathrm{Zn}(-0.76 \mathrm{~V})$ and $\mathrm{Fe}^{2+} \mid \mathrm{Fe}(-0.41$ $\mathrm{V})$ is

275895 Given that the standard reduction potentials for $\mathrm{M}^{+} / \mathrm{M}$ and $\mathrm{N}^{+} / \mathrm{N}$ electrodes at $298 \mathrm{~K}$ are 0.52 $\mathrm{V}$ and $0.25 \mathrm{~V}$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$\mathbf{M}\left \vert\mathbf{M}^{+} \ \vert \mathbf{N}^{+}\right \vert \mathbf{N}$

275898 In a cell that utilizes the reaction
$\mathbf{Z n}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
addition of $\mathrm{H}_{2} \mathrm{SO}_{4}$ to cathode compartment will.

275900 $\mathrm{Zn}(\mathrm{s})+\mathrm{Cl}_{2}(1 \mathrm{~atm}) \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{Cl}^{-} ; \mathrm{E}^{\circ}=2.0 \mathrm{~V}$.
To increase the e.m.f. of the above cell

275901 The reduction potential of an electrode can be increased by

275892 The emf of a galvanic cell constituted with the electrodes $\mathrm{Zn}^{2+} \mid \mathrm{Zn}(-0.76 \mathrm{~V})$ and $\mathrm{Fe}^{2+} \mid \mathrm{Fe}(-0.41$ $\mathrm{V})$ is

275895 Given that the standard reduction potentials for $\mathrm{M}^{+} / \mathrm{M}$ and $\mathrm{N}^{+} / \mathrm{N}$ electrodes at $298 \mathrm{~K}$ are 0.52 $\mathrm{V}$ and $0.25 \mathrm{~V}$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$\mathbf{M}\left \vert\mathbf{M}^{+} \ \vert \mathbf{N}^{+}\right \vert \mathbf{N}$

275898 In a cell that utilizes the reaction
$\mathbf{Z n}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
addition of $\mathrm{H}_{2} \mathrm{SO}_{4}$ to cathode compartment will.

275900 $\mathrm{Zn}(\mathrm{s})+\mathrm{Cl}_{2}(1 \mathrm{~atm}) \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{Cl}^{-} ; \mathrm{E}^{\circ}=2.0 \mathrm{~V}$.
To increase the e.m.f. of the above cell

275901 The reduction potential of an electrode can be increased by

275892 The emf of a galvanic cell constituted with the electrodes $\mathrm{Zn}^{2+} \mid \mathrm{Zn}(-0.76 \mathrm{~V})$ and $\mathrm{Fe}^{2+} \mid \mathrm{Fe}(-0.41$ $\mathrm{V})$ is

275895 Given that the standard reduction potentials for $\mathrm{M}^{+} / \mathrm{M}$ and $\mathrm{N}^{+} / \mathrm{N}$ electrodes at $298 \mathrm{~K}$ are 0.52 $\mathrm{V}$ and $0.25 \mathrm{~V}$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$\mathbf{M}\left \vert\mathbf{M}^{+} \ \vert \mathbf{N}^{+}\right \vert \mathbf{N}$

275898 In a cell that utilizes the reaction
$\mathbf{Z n}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
addition of $\mathrm{H}_{2} \mathrm{SO}_{4}$ to cathode compartment will.

275900 $\mathrm{Zn}(\mathrm{s})+\mathrm{Cl}_{2}(1 \mathrm{~atm}) \rightarrow \mathrm{Zn}^{2+}+2 \mathrm{Cl}^{-} ; \mathrm{E}^{\circ}=2.0 \mathrm{~V}$.
To increase the e.m.f. of the above cell

275901 The reduction potential of an electrode can be increased by