275763 The standard reduction potentials at $298 \mathrm{~K}$ for the following half cell reactions are given below:
$\begin{aligned}
& \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Zn}(\mathrm{s}),-0.762 \mathrm{~V} \\
& \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightleftharpoons \mathrm{Cr}(\mathrm{s}),-0.74 \mathrm{~V} \\
& 2 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g}),+\mathbf{0 . 0 0 V} \\
& \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightleftharpoons \mathrm{Fe}^{2+}(\mathrm{aq}),+0.77 \mathrm{~V}
\end{aligned}$
Which one of the following is the strongest reducing agent?

275776 Using the data given below find out the strongest reducing agent?
$\begin{array}{ll}
\mathrm{E}_{\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} / \mathrm{Cr}^{3+}}^{\mathrm{o}}=1.33 \mathrm{~V} & \mathrm{E}_{\mathrm{Cl}_{2} / \mathrm{Cl}^{-}}^{\mathrm{o}}=1.36 \mathrm{~V} \\
\mathrm{E}_{\mathrm{MnO}_{4}^{-} / \mathrm{Mn}^{2+}}^{\mathrm{o}}=1.51 \mathrm{~V} & \mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.74 \mathrm{~V}
\end{array}$

275779 Given below are two statements.
Statement I : The $\mathrm{E}^{0}$ value of $\mathrm{Ce}^{4+} / \mathrm{Ce}^{3+}$ is $1.74 \mathrm{~V}$.
Statement II : $\mathrm{Ce}$ is more stable in $\mathrm{Ce}^{4+}$ state than $\mathrm{Ce}^{3+}$ state.
In the light of the above statements, choose the most appropriate answer from the options given below.

275832 The standard reduction potential of $\mathrm{Pb}$ and $\mathrm{Zn}$ electrodes are $-0.126 \mathrm{~V}$ and $-0.763 \mathrm{~V}$ respectively. The cell equation will be:

275763 The standard reduction potentials at $298 \mathrm{~K}$ for the following half cell reactions are given below:
$\begin{aligned}
& \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Zn}(\mathrm{s}),-0.762 \mathrm{~V} \\
& \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightleftharpoons \mathrm{Cr}(\mathrm{s}),-0.74 \mathrm{~V} \\
& 2 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g}),+\mathbf{0 . 0 0 V} \\
& \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightleftharpoons \mathrm{Fe}^{2+}(\mathrm{aq}),+0.77 \mathrm{~V}
\end{aligned}$
Which one of the following is the strongest reducing agent?

275776 Using the data given below find out the strongest reducing agent?
$\begin{array}{ll}
\mathrm{E}_{\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} / \mathrm{Cr}^{3+}}^{\mathrm{o}}=1.33 \mathrm{~V} & \mathrm{E}_{\mathrm{Cl}_{2} / \mathrm{Cl}^{-}}^{\mathrm{o}}=1.36 \mathrm{~V} \\
\mathrm{E}_{\mathrm{MnO}_{4}^{-} / \mathrm{Mn}^{2+}}^{\mathrm{o}}=1.51 \mathrm{~V} & \mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.74 \mathrm{~V}
\end{array}$

275779 Given below are two statements.
Statement I : The $\mathrm{E}^{0}$ value of $\mathrm{Ce}^{4+} / \mathrm{Ce}^{3+}$ is $1.74 \mathrm{~V}$.
Statement II : $\mathrm{Ce}$ is more stable in $\mathrm{Ce}^{4+}$ state than $\mathrm{Ce}^{3+}$ state.
In the light of the above statements, choose the most appropriate answer from the options given below.

275832 The standard reduction potential of $\mathrm{Pb}$ and $\mathrm{Zn}$ electrodes are $-0.126 \mathrm{~V}$ and $-0.763 \mathrm{~V}$ respectively. The cell equation will be:

275763 The standard reduction potentials at $298 \mathrm{~K}$ for the following half cell reactions are given below:
$\begin{aligned}
& \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Zn}(\mathrm{s}),-0.762 \mathrm{~V} \\
& \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightleftharpoons \mathrm{Cr}(\mathrm{s}),-0.74 \mathrm{~V} \\
& 2 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g}),+\mathbf{0 . 0 0 V} \\
& \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightleftharpoons \mathrm{Fe}^{2+}(\mathrm{aq}),+0.77 \mathrm{~V}
\end{aligned}$
Which one of the following is the strongest reducing agent?

275776 Using the data given below find out the strongest reducing agent?
$\begin{array}{ll}
\mathrm{E}_{\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} / \mathrm{Cr}^{3+}}^{\mathrm{o}}=1.33 \mathrm{~V} & \mathrm{E}_{\mathrm{Cl}_{2} / \mathrm{Cl}^{-}}^{\mathrm{o}}=1.36 \mathrm{~V} \\
\mathrm{E}_{\mathrm{MnO}_{4}^{-} / \mathrm{Mn}^{2+}}^{\mathrm{o}}=1.51 \mathrm{~V} & \mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.74 \mathrm{~V}
\end{array}$

275779 Given below are two statements.
Statement I : The $\mathrm{E}^{0}$ value of $\mathrm{Ce}^{4+} / \mathrm{Ce}^{3+}$ is $1.74 \mathrm{~V}$.
Statement II : $\mathrm{Ce}$ is more stable in $\mathrm{Ce}^{4+}$ state than $\mathrm{Ce}^{3+}$ state.
In the light of the above statements, choose the most appropriate answer from the options given below.

275832 The standard reduction potential of $\mathrm{Pb}$ and $\mathrm{Zn}$ electrodes are $-0.126 \mathrm{~V}$ and $-0.763 \mathrm{~V}$ respectively. The cell equation will be:

275763 The standard reduction potentials at $298 \mathrm{~K}$ for the following half cell reactions are given below:
$\begin{aligned}
& \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Zn}(\mathrm{s}),-0.762 \mathrm{~V} \\
& \mathrm{Cr}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightleftharpoons \mathrm{Cr}(\mathrm{s}),-0.74 \mathrm{~V} \\
& 2 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g}),+\mathbf{0 . 0 0 V} \\
& \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightleftharpoons \mathrm{Fe}^{2+}(\mathrm{aq}),+0.77 \mathrm{~V}
\end{aligned}$
Which one of the following is the strongest reducing agent?

275776 Using the data given below find out the strongest reducing agent?
$\begin{array}{ll}
\mathrm{E}_{\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} / \mathrm{Cr}^{3+}}^{\mathrm{o}}=1.33 \mathrm{~V} & \mathrm{E}_{\mathrm{Cl}_{2} / \mathrm{Cl}^{-}}^{\mathrm{o}}=1.36 \mathrm{~V} \\
\mathrm{E}_{\mathrm{MnO}_{4}^{-} / \mathrm{Mn}^{2+}}^{\mathrm{o}}=1.51 \mathrm{~V} & \mathrm{E}_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{0}=-0.74 \mathrm{~V}
\end{array}$

275779 Given below are two statements.
Statement I : The $\mathrm{E}^{0}$ value of $\mathrm{Ce}^{4+} / \mathrm{Ce}^{3+}$ is $1.74 \mathrm{~V}$.
Statement II : $\mathrm{Ce}$ is more stable in $\mathrm{Ce}^{4+}$ state than $\mathrm{Ce}^{3+}$ state.
In the light of the above statements, choose the most appropriate answer from the options given below.

275832 The standard reduction potential of $\mathrm{Pb}$ and $\mathrm{Zn}$ electrodes are $-0.126 \mathrm{~V}$ and $-0.763 \mathrm{~V}$ respectively. The cell equation will be: