275879 $\mathrm{Cu}^{+}(\mathrm{aq})$ is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction:
$\mathrm{Cu}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})$
Choose correct $\mathrm{E}^{0}$ for above reaction if
$\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathbf{0}}=\mathbf{0 . 3 4} \mathrm{V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}^{+}}^{\mathbf{0}}=\mathbf{0 . 1 5} \mathrm{V}$

275880 Which of the following will give $\mathrm{H}_{2(\mathrm{~g})}$ at cathode and $\mathrm{O}_{2(\mathrm{~g})}$ at anode on electrolysis using platinum electrodes?

275882 The standard emf of the cell $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Ag}^{+}\right \vert \mathrm{Ag}$ is $1.56 \mathrm{~V}$. If the standard reduction potential of $\mathrm{Ag}$ is $0.8 \mathrm{~V}$, the standard oxidation potential of $\mathrm{Zn}$ is

275885 A hydrogen gas electrode is made by dipping platinum wire in a solution of $\mathrm{HCl}$ of $\mathrm{pH}=10$ and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of electrode would be

275879 $\mathrm{Cu}^{+}(\mathrm{aq})$ is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction:
$\mathrm{Cu}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})$
Choose correct $\mathrm{E}^{0}$ for above reaction if
$\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathbf{0}}=\mathbf{0 . 3 4} \mathrm{V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}^{+}}^{\mathbf{0}}=\mathbf{0 . 1 5} \mathrm{V}$

275880 Which of the following will give $\mathrm{H}_{2(\mathrm{~g})}$ at cathode and $\mathrm{O}_{2(\mathrm{~g})}$ at anode on electrolysis using platinum electrodes?

275882 The standard emf of the cell $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Ag}^{+}\right \vert \mathrm{Ag}$ is $1.56 \mathrm{~V}$. If the standard reduction potential of $\mathrm{Ag}$ is $0.8 \mathrm{~V}$, the standard oxidation potential of $\mathrm{Zn}$ is

275885 A hydrogen gas electrode is made by dipping platinum wire in a solution of $\mathrm{HCl}$ of $\mathrm{pH}=10$ and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of electrode would be

275879 $\mathrm{Cu}^{+}(\mathrm{aq})$ is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction:
$\mathrm{Cu}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})$
Choose correct $\mathrm{E}^{0}$ for above reaction if
$\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathbf{0}}=\mathbf{0 . 3 4} \mathrm{V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}^{+}}^{\mathbf{0}}=\mathbf{0 . 1 5} \mathrm{V}$

275880 Which of the following will give $\mathrm{H}_{2(\mathrm{~g})}$ at cathode and $\mathrm{O}_{2(\mathrm{~g})}$ at anode on electrolysis using platinum electrodes?

275882 The standard emf of the cell $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Ag}^{+}\right \vert \mathrm{Ag}$ is $1.56 \mathrm{~V}$. If the standard reduction potential of $\mathrm{Ag}$ is $0.8 \mathrm{~V}$, the standard oxidation potential of $\mathrm{Zn}$ is

275885 A hydrogen gas electrode is made by dipping platinum wire in a solution of $\mathrm{HCl}$ of $\mathrm{pH}=10$ and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of electrode would be

275879 $\mathrm{Cu}^{+}(\mathrm{aq})$ is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction:
$\mathrm{Cu}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})$
Choose correct $\mathrm{E}^{0}$ for above reaction if
$\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}}^{\mathbf{0}}=\mathbf{0 . 3 4} \mathrm{V}$ and $\mathrm{E}_{\mathrm{Cu}^{2+} / \mathrm{Cu}^{+}}^{\mathbf{0}}=\mathbf{0 . 1 5} \mathrm{V}$

275880 Which of the following will give $\mathrm{H}_{2(\mathrm{~g})}$ at cathode and $\mathrm{O}_{2(\mathrm{~g})}$ at anode on electrolysis using platinum electrodes?

275882 The standard emf of the cell $\mathrm{Zn}\left \vert\mathrm{Zn}^{2+} \ \vert \mathrm{Ag}^{+}\right \vert \mathrm{Ag}$ is $1.56 \mathrm{~V}$. If the standard reduction potential of $\mathrm{Ag}$ is $0.8 \mathrm{~V}$, the standard oxidation potential of $\mathrm{Zn}$ is

275885 A hydrogen gas electrode is made by dipping platinum wire in a solution of $\mathrm{HCl}$ of $\mathrm{pH}=10$ and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of electrode would be