275886 Consider the helf-cell reduction reaction
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{0}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{0}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\mathbf{0}}$ for the reaction, $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275887 $\mathrm{H}_{2}$ gas is liberated at cathode and anode both by electrolysis of the following solution except in-

275888 A quantity of electrical charge brings about the deposition of $4.5 \mathrm{~g} \mathrm{Al}$ from $\mathrm{Al}^{3+}$ at the cathode will also produce the following volume at (STP) of $\mathrm{H}_{2}(\mathrm{~g})$ from $\mathrm{H}^{+}$at the cathode-

275890 An electrochemical cell has two half cell reactions as
$\mathrm{A}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{A}$;
$\mathbf{E}_{\mathrm{A}^{2+} / \mathrm{A}}^{\mathbf{0}}=\mathbf{0 . 3 4 \mathrm { V }}$
$\mathrm{X} \rightarrow \mathrm{X}^{2+}+2 \mathrm{e}^{-}$;
$\mathbf{E}_{\mathbf{x}^{2+} / \mathbf{x}}^{0}=-2.37 \mathrm{~V}$
The cell voltage will be

275893 Consider the half-cell reduction reaction,
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{\circ}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{\circ}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\circ}$ for the reaction $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275886 Consider the helf-cell reduction reaction
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{0}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{0}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\mathbf{0}}$ for the reaction, $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275887 $\mathrm{H}_{2}$ gas is liberated at cathode and anode both by electrolysis of the following solution except in-

275888 A quantity of electrical charge brings about the deposition of $4.5 \mathrm{~g} \mathrm{Al}$ from $\mathrm{Al}^{3+}$ at the cathode will also produce the following volume at (STP) of $\mathrm{H}_{2}(\mathrm{~g})$ from $\mathrm{H}^{+}$at the cathode-

275890 An electrochemical cell has two half cell reactions as
$\mathrm{A}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{A}$;
$\mathbf{E}_{\mathrm{A}^{2+} / \mathrm{A}}^{\mathbf{0}}=\mathbf{0 . 3 4 \mathrm { V }}$
$\mathrm{X} \rightarrow \mathrm{X}^{2+}+2 \mathrm{e}^{-}$;
$\mathbf{E}_{\mathbf{x}^{2+} / \mathbf{x}}^{0}=-2.37 \mathrm{~V}$
The cell voltage will be

275893 Consider the half-cell reduction reaction,
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{\circ}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{\circ}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\circ}$ for the reaction $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275886 Consider the helf-cell reduction reaction
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{0}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{0}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\mathbf{0}}$ for the reaction, $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275887 $\mathrm{H}_{2}$ gas is liberated at cathode and anode both by electrolysis of the following solution except in-

275888 A quantity of electrical charge brings about the deposition of $4.5 \mathrm{~g} \mathrm{Al}$ from $\mathrm{Al}^{3+}$ at the cathode will also produce the following volume at (STP) of $\mathrm{H}_{2}(\mathrm{~g})$ from $\mathrm{H}^{+}$at the cathode-

275890 An electrochemical cell has two half cell reactions as
$\mathrm{A}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{A}$;
$\mathbf{E}_{\mathrm{A}^{2+} / \mathrm{A}}^{\mathbf{0}}=\mathbf{0 . 3 4 \mathrm { V }}$
$\mathrm{X} \rightarrow \mathrm{X}^{2+}+2 \mathrm{e}^{-}$;
$\mathbf{E}_{\mathbf{x}^{2+} / \mathbf{x}}^{0}=-2.37 \mathrm{~V}$
The cell voltage will be

275893 Consider the half-cell reduction reaction,
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{\circ}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{\circ}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\circ}$ for the reaction $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275886 Consider the helf-cell reduction reaction
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{0}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{0}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\mathbf{0}}$ for the reaction, $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275887 $\mathrm{H}_{2}$ gas is liberated at cathode and anode both by electrolysis of the following solution except in-

275888 A quantity of electrical charge brings about the deposition of $4.5 \mathrm{~g} \mathrm{Al}$ from $\mathrm{Al}^{3+}$ at the cathode will also produce the following volume at (STP) of $\mathrm{H}_{2}(\mathrm{~g})$ from $\mathrm{H}^{+}$at the cathode-

275890 An electrochemical cell has two half cell reactions as
$\mathrm{A}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{A}$;
$\mathbf{E}_{\mathrm{A}^{2+} / \mathrm{A}}^{\mathbf{0}}=\mathbf{0 . 3 4 \mathrm { V }}$
$\mathrm{X} \rightarrow \mathrm{X}^{2+}+2 \mathrm{e}^{-}$;
$\mathbf{E}_{\mathbf{x}^{2+} / \mathbf{x}}^{0}=-2.37 \mathrm{~V}$
The cell voltage will be

275893 Consider the half-cell reduction reaction,
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{\circ}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{\circ}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\circ}$ for the reaction $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275886 Consider the helf-cell reduction reaction
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{0}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{0}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\mathbf{0}}$ for the reaction, $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively

275887 $\mathrm{H}_{2}$ gas is liberated at cathode and anode both by electrolysis of the following solution except in-

275888 A quantity of electrical charge brings about the deposition of $4.5 \mathrm{~g} \mathrm{Al}$ from $\mathrm{Al}^{3+}$ at the cathode will also produce the following volume at (STP) of $\mathrm{H}_{2}(\mathrm{~g})$ from $\mathrm{H}^{+}$at the cathode-

275890 An electrochemical cell has two half cell reactions as
$\mathrm{A}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{A}$;
$\mathbf{E}_{\mathrm{A}^{2+} / \mathrm{A}}^{\mathbf{0}}=\mathbf{0 . 3 4 \mathrm { V }}$
$\mathrm{X} \rightarrow \mathrm{X}^{2+}+2 \mathrm{e}^{-}$;
$\mathbf{E}_{\mathbf{x}^{2+} / \mathbf{x}}^{0}=-2.37 \mathrm{~V}$
The cell voltage will be

275893 Consider the half-cell reduction reaction,
$\mathrm{Mn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}, \mathrm{E}^{\circ}=-1.18 \mathrm{~V}$
$\mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{3+}+\mathrm{e}^{-}, \mathrm{E}^{\circ}=-1.51 \mathrm{~V}$
The $\mathrm{E}^{\circ}$ for the reaction $3 \mathrm{Mn}^{2+} \rightarrow \mathrm{Mn}^{0}+2 \mathrm{Mn}^{3+}$, and possibility of the forward reaction are respectively