275811 One litre solution of $\mathbf{M g C l}_{2}$ is electrolysed completely by passing a current of $1 \mathrm{~A}$ for 16 min $5 \mathrm{sec}$. The original concentration of $\mathbf{M g C l}_{2}$ solution was
(Atomic mass of $\mathrm{Mg}=24$ )

275812 The $\mathbf{E}^{0}$ values of the following half cells are given: $\left(25^{\circ} \mathrm{C}\right) \quad \mathrm{E}^{\mathbf{o}}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+0.771 \mathrm{~V}$
$\mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})-0.447 \mathrm{~V}$
The $\Delta \mathrm{G}^{\mathrm{o}}$ of $\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})$

275814 If one mole electrons is passed through the solutions of $\mathrm{AlCl}_{3}, \mathrm{AgNO}_{3}$ and $\mathrm{MgSO}_{4}$, in what ratio $\mathrm{Al}, \mathrm{Ag}$ and $\mathrm{Mg}$ will be deposited all the electrodes?

275808 Given, that $\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{0}=+1.23 \mathrm{~V}$;
$\mathrm{E}_{\mathrm{s}_{2} \mathrm{O}_{8}^{2-/} / \mathrm{SO}_{4}^{2-}}^{\Theta}=\mathbf{2 . 0 5} \mathrm{V}$;
$\mathrm{E}_{\mathrm{Br}_{2} / \mathbf{B r}^{-}}^{\ominus}=+1.09 \mathrm{~V}$,
$\mathrm{E}_{\mathrm{Au}^{3+} / \mathrm{Au}}^{\Theta}=+\mathbf{1 . 4 V}$
The strongest oxidising agent is

275813 $\quad \mathrm{Zn}_{\text {(s) }}\left \vert\mathbf{Z n}_{\text {(aq) }}^{2+}(1 \mathrm{M}) \ \vert \mathrm{Ni}_{\text {(aq) }}^{2+}(1 \mathrm{M})\right \vert \mathbf{N i}_{\text {(s) }}$
Which is incorrect for the above given cell?

275811 One litre solution of $\mathbf{M g C l}_{2}$ is electrolysed completely by passing a current of $1 \mathrm{~A}$ for 16 min $5 \mathrm{sec}$. The original concentration of $\mathbf{M g C l}_{2}$ solution was
(Atomic mass of $\mathrm{Mg}=24$ )

275812 The $\mathbf{E}^{0}$ values of the following half cells are given: $\left(25^{\circ} \mathrm{C}\right) \quad \mathrm{E}^{\mathbf{o}}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+0.771 \mathrm{~V}$
$\mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})-0.447 \mathrm{~V}$
The $\Delta \mathrm{G}^{\mathrm{o}}$ of $\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})$

275814 If one mole electrons is passed through the solutions of $\mathrm{AlCl}_{3}, \mathrm{AgNO}_{3}$ and $\mathrm{MgSO}_{4}$, in what ratio $\mathrm{Al}, \mathrm{Ag}$ and $\mathrm{Mg}$ will be deposited all the electrodes?

275808 Given, that $\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{0}=+1.23 \mathrm{~V}$;
$\mathrm{E}_{\mathrm{s}_{2} \mathrm{O}_{8}^{2-/} / \mathrm{SO}_{4}^{2-}}^{\Theta}=\mathbf{2 . 0 5} \mathrm{V}$;
$\mathrm{E}_{\mathrm{Br}_{2} / \mathbf{B r}^{-}}^{\ominus}=+1.09 \mathrm{~V}$,
$\mathrm{E}_{\mathrm{Au}^{3+} / \mathrm{Au}}^{\Theta}=+\mathbf{1 . 4 V}$
The strongest oxidising agent is

275813 $\quad \mathrm{Zn}_{\text {(s) }}\left \vert\mathbf{Z n}_{\text {(aq) }}^{2+}(1 \mathrm{M}) \ \vert \mathrm{Ni}_{\text {(aq) }}^{2+}(1 \mathrm{M})\right \vert \mathbf{N i}_{\text {(s) }}$
Which is incorrect for the above given cell?

275811 One litre solution of $\mathbf{M g C l}_{2}$ is electrolysed completely by passing a current of $1 \mathrm{~A}$ for 16 min $5 \mathrm{sec}$. The original concentration of $\mathbf{M g C l}_{2}$ solution was
(Atomic mass of $\mathrm{Mg}=24$ )

275812 The $\mathbf{E}^{0}$ values of the following half cells are given: $\left(25^{\circ} \mathrm{C}\right) \quad \mathrm{E}^{\mathbf{o}}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+0.771 \mathrm{~V}$
$\mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})-0.447 \mathrm{~V}$
The $\Delta \mathrm{G}^{\mathrm{o}}$ of $\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})$

275814 If one mole electrons is passed through the solutions of $\mathrm{AlCl}_{3}, \mathrm{AgNO}_{3}$ and $\mathrm{MgSO}_{4}$, in what ratio $\mathrm{Al}, \mathrm{Ag}$ and $\mathrm{Mg}$ will be deposited all the electrodes?

275808 Given, that $\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{0}=+1.23 \mathrm{~V}$;
$\mathrm{E}_{\mathrm{s}_{2} \mathrm{O}_{8}^{2-/} / \mathrm{SO}_{4}^{2-}}^{\Theta}=\mathbf{2 . 0 5} \mathrm{V}$;
$\mathrm{E}_{\mathrm{Br}_{2} / \mathbf{B r}^{-}}^{\ominus}=+1.09 \mathrm{~V}$,
$\mathrm{E}_{\mathrm{Au}^{3+} / \mathrm{Au}}^{\Theta}=+\mathbf{1 . 4 V}$
The strongest oxidising agent is

275813 $\quad \mathrm{Zn}_{\text {(s) }}\left \vert\mathbf{Z n}_{\text {(aq) }}^{2+}(1 \mathrm{M}) \ \vert \mathrm{Ni}_{\text {(aq) }}^{2+}(1 \mathrm{M})\right \vert \mathbf{N i}_{\text {(s) }}$
Which is incorrect for the above given cell?

275811 One litre solution of $\mathbf{M g C l}_{2}$ is electrolysed completely by passing a current of $1 \mathrm{~A}$ for 16 min $5 \mathrm{sec}$. The original concentration of $\mathbf{M g C l}_{2}$ solution was
(Atomic mass of $\mathrm{Mg}=24$ )

275812 The $\mathbf{E}^{0}$ values of the following half cells are given: $\left(25^{\circ} \mathrm{C}\right) \quad \mathrm{E}^{\mathbf{o}}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+0.771 \mathrm{~V}$
$\mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})-0.447 \mathrm{~V}$
The $\Delta \mathrm{G}^{\mathrm{o}}$ of $\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})$

275814 If one mole electrons is passed through the solutions of $\mathrm{AlCl}_{3}, \mathrm{AgNO}_{3}$ and $\mathrm{MgSO}_{4}$, in what ratio $\mathrm{Al}, \mathrm{Ag}$ and $\mathrm{Mg}$ will be deposited all the electrodes?

275808 Given, that $\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{0}=+1.23 \mathrm{~V}$;
$\mathrm{E}_{\mathrm{s}_{2} \mathrm{O}_{8}^{2-/} / \mathrm{SO}_{4}^{2-}}^{\Theta}=\mathbf{2 . 0 5} \mathrm{V}$;
$\mathrm{E}_{\mathrm{Br}_{2} / \mathbf{B r}^{-}}^{\ominus}=+1.09 \mathrm{~V}$,
$\mathrm{E}_{\mathrm{Au}^{3+} / \mathrm{Au}}^{\Theta}=+\mathbf{1 . 4 V}$
The strongest oxidising agent is

275813 $\quad \mathrm{Zn}_{\text {(s) }}\left \vert\mathbf{Z n}_{\text {(aq) }}^{2+}(1 \mathrm{M}) \ \vert \mathrm{Ni}_{\text {(aq) }}^{2+}(1 \mathrm{M})\right \vert \mathbf{N i}_{\text {(s) }}$
Which is incorrect for the above given cell?

275811 One litre solution of $\mathbf{M g C l}_{2}$ is electrolysed completely by passing a current of $1 \mathrm{~A}$ for 16 min $5 \mathrm{sec}$. The original concentration of $\mathbf{M g C l}_{2}$ solution was
(Atomic mass of $\mathrm{Mg}=24$ )

275812 The $\mathbf{E}^{0}$ values of the following half cells are given: $\left(25^{\circ} \mathrm{C}\right) \quad \mathrm{E}^{\mathbf{o}}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq})+0.771 \mathrm{~V}$
$\mathrm{Fe}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})-0.447 \mathrm{~V}$
The $\Delta \mathrm{G}^{\mathrm{o}}$ of $\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}(\mathrm{s})$

275814 If one mole electrons is passed through the solutions of $\mathrm{AlCl}_{3}, \mathrm{AgNO}_{3}$ and $\mathrm{MgSO}_{4}$, in what ratio $\mathrm{Al}, \mathrm{Ag}$ and $\mathrm{Mg}$ will be deposited all the electrodes?

275808 Given, that $\mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{0}=+1.23 \mathrm{~V}$;
$\mathrm{E}_{\mathrm{s}_{2} \mathrm{O}_{8}^{2-/} / \mathrm{SO}_{4}^{2-}}^{\Theta}=\mathbf{2 . 0 5} \mathrm{V}$;
$\mathrm{E}_{\mathrm{Br}_{2} / \mathbf{B r}^{-}}^{\ominus}=+1.09 \mathrm{~V}$,
$\mathrm{E}_{\mathrm{Au}^{3+} / \mathrm{Au}}^{\Theta}=+\mathbf{1 . 4 V}$
The strongest oxidising agent is

275813 $\quad \mathrm{Zn}_{\text {(s) }}\left \vert\mathbf{Z n}_{\text {(aq) }}^{2+}(1 \mathrm{M}) \ \vert \mathrm{Ni}_{\text {(aq) }}^{2+}(1 \mathrm{M})\right \vert \mathbf{N i}_{\text {(s) }}$
Which is incorrect for the above given cell?