275867 The standard electrode potentials of $\mathrm{Zn}$ and $\mathrm{Ni}$ respectively are $-0.76 \mathrm{~V}$ and $-0.25 \mathrm{~V}$. The standard emf of the spontaneous cell by coupling these under standard conditions is

275868 $\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.51 \mathrm{~V}$
$\mathrm{MnO}_{2}+4 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+2 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.23 \mathrm{~V}$ $\mathbf{E}_{\mathbf{M n O}_{4}^{-} / \mathrm{MnO}_{2}}^{\mathbf{0}}$ is

275869 Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below.
$\mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ; \mathrm{E}^{0}$
$=1.51 \mathrm{~V}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$;
$\mathrm{E}^{\mathbf{0}}=\mathbf{1 . 3 8 \mathrm { V }}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) ; \mathrm{E}^{\mathbf{0}}=\mathbf{0 . 7 7} \mathrm{V}$
$\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) ; \mathrm{E}^{0}=1.40 \mathrm{~V}$
Identify the incorrect statement regarding the quantitative estimation of gaseous $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}$

275870 The two half-cell reactions of an
electrochemical cell is given as
$\begin{aligned}
& \mathrm{Ag}^{+}+\mathrm{e}^{-} \rightarrow \mathrm{Ag} ; \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{0}=-0.3995 \mathrm{~V} \\
& \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{e}^{-} ; \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\circ}=-0.7120 \mathrm{~V}
\end{aligned}$
The value of cell EMF will be

275871 Assertion: During electrolysis of $\mathrm{CuSO}_{4}(\mathrm{aq})$ using copper electrodes, copper is dissolved at anode and deposited at cathode.
Reason: Oxidation takes place at anode and reduction at cathode.

275867 The standard electrode potentials of $\mathrm{Zn}$ and $\mathrm{Ni}$ respectively are $-0.76 \mathrm{~V}$ and $-0.25 \mathrm{~V}$. The standard emf of the spontaneous cell by coupling these under standard conditions is

275868 $\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.51 \mathrm{~V}$
$\mathrm{MnO}_{2}+4 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+2 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.23 \mathrm{~V}$ $\mathbf{E}_{\mathbf{M n O}_{4}^{-} / \mathrm{MnO}_{2}}^{\mathbf{0}}$ is

275869 Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below.
$\mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ; \mathrm{E}^{0}$
$=1.51 \mathrm{~V}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$;
$\mathrm{E}^{\mathbf{0}}=\mathbf{1 . 3 8 \mathrm { V }}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) ; \mathrm{E}^{\mathbf{0}}=\mathbf{0 . 7 7} \mathrm{V}$
$\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) ; \mathrm{E}^{0}=1.40 \mathrm{~V}$
Identify the incorrect statement regarding the quantitative estimation of gaseous $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}$

275870 The two half-cell reactions of an
electrochemical cell is given as
$\begin{aligned}
& \mathrm{Ag}^{+}+\mathrm{e}^{-} \rightarrow \mathrm{Ag} ; \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{0}=-0.3995 \mathrm{~V} \\
& \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{e}^{-} ; \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\circ}=-0.7120 \mathrm{~V}
\end{aligned}$
The value of cell EMF will be

275871 Assertion: During electrolysis of $\mathrm{CuSO}_{4}(\mathrm{aq})$ using copper electrodes, copper is dissolved at anode and deposited at cathode.
Reason: Oxidation takes place at anode and reduction at cathode.

275867 The standard electrode potentials of $\mathrm{Zn}$ and $\mathrm{Ni}$ respectively are $-0.76 \mathrm{~V}$ and $-0.25 \mathrm{~V}$. The standard emf of the spontaneous cell by coupling these under standard conditions is

275868 $\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.51 \mathrm{~V}$
$\mathrm{MnO}_{2}+4 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+2 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.23 \mathrm{~V}$ $\mathbf{E}_{\mathbf{M n O}_{4}^{-} / \mathrm{MnO}_{2}}^{\mathbf{0}}$ is

275869 Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below.
$\mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ; \mathrm{E}^{0}$
$=1.51 \mathrm{~V}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$;
$\mathrm{E}^{\mathbf{0}}=\mathbf{1 . 3 8 \mathrm { V }}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) ; \mathrm{E}^{\mathbf{0}}=\mathbf{0 . 7 7} \mathrm{V}$
$\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) ; \mathrm{E}^{0}=1.40 \mathrm{~V}$
Identify the incorrect statement regarding the quantitative estimation of gaseous $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}$

275870 The two half-cell reactions of an
electrochemical cell is given as
$\begin{aligned}
& \mathrm{Ag}^{+}+\mathrm{e}^{-} \rightarrow \mathrm{Ag} ; \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{0}=-0.3995 \mathrm{~V} \\
& \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{e}^{-} ; \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\circ}=-0.7120 \mathrm{~V}
\end{aligned}$
The value of cell EMF will be

275871 Assertion: During electrolysis of $\mathrm{CuSO}_{4}(\mathrm{aq})$ using copper electrodes, copper is dissolved at anode and deposited at cathode.
Reason: Oxidation takes place at anode and reduction at cathode.

275867 The standard electrode potentials of $\mathrm{Zn}$ and $\mathrm{Ni}$ respectively are $-0.76 \mathrm{~V}$ and $-0.25 \mathrm{~V}$. The standard emf of the spontaneous cell by coupling these under standard conditions is

275868 $\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.51 \mathrm{~V}$
$\mathrm{MnO}_{2}+4 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+2 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.23 \mathrm{~V}$ $\mathbf{E}_{\mathbf{M n O}_{4}^{-} / \mathrm{MnO}_{2}}^{\mathbf{0}}$ is

275869 Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below.
$\mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ; \mathrm{E}^{0}$
$=1.51 \mathrm{~V}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$;
$\mathrm{E}^{\mathbf{0}}=\mathbf{1 . 3 8 \mathrm { V }}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) ; \mathrm{E}^{\mathbf{0}}=\mathbf{0 . 7 7} \mathrm{V}$
$\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) ; \mathrm{E}^{0}=1.40 \mathrm{~V}$
Identify the incorrect statement regarding the quantitative estimation of gaseous $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}$

275870 The two half-cell reactions of an
electrochemical cell is given as
$\begin{aligned}
& \mathrm{Ag}^{+}+\mathrm{e}^{-} \rightarrow \mathrm{Ag} ; \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{0}=-0.3995 \mathrm{~V} \\
& \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{e}^{-} ; \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\circ}=-0.7120 \mathrm{~V}
\end{aligned}$
The value of cell EMF will be

275871 Assertion: During electrolysis of $\mathrm{CuSO}_{4}(\mathrm{aq})$ using copper electrodes, copper is dissolved at anode and deposited at cathode.
Reason: Oxidation takes place at anode and reduction at cathode.

275867 The standard electrode potentials of $\mathrm{Zn}$ and $\mathrm{Ni}$ respectively are $-0.76 \mathrm{~V}$ and $-0.25 \mathrm{~V}$. The standard emf of the spontaneous cell by coupling these under standard conditions is

275868 $\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.51 \mathrm{~V}$
$\mathrm{MnO}_{2}+4 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+2 \mathrm{H}_{2} \mathrm{O}, \mathrm{E}^{0}=1.23 \mathrm{~V}$ $\mathbf{E}_{\mathbf{M n O}_{4}^{-} / \mathrm{MnO}_{2}}^{\mathbf{0}}$ is

275869 Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below.
$\mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) ; \mathrm{E}^{0}$
$=1.51 \mathrm{~V}$
$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$;
$\mathrm{E}^{\mathbf{0}}=\mathbf{1 . 3 8 \mathrm { V }}$
$\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) ; \mathrm{E}^{\mathbf{0}}=\mathbf{0 . 7 7} \mathrm{V}$
$\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) ; \mathrm{E}^{0}=1.40 \mathrm{~V}$
Identify the incorrect statement regarding the quantitative estimation of gaseous $\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}$

275870 The two half-cell reactions of an
electrochemical cell is given as
$\begin{aligned}
& \mathrm{Ag}^{+}+\mathrm{e}^{-} \rightarrow \mathrm{Ag} ; \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{0}=-0.3995 \mathrm{~V} \\
& \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{e}^{-} ; \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^{\circ}=-0.7120 \mathrm{~V}
\end{aligned}$
The value of cell EMF will be

275871 Assertion: During electrolysis of $\mathrm{CuSO}_{4}(\mathrm{aq})$ using copper electrodes, copper is dissolved at anode and deposited at cathode.
Reason: Oxidation takes place at anode and reduction at cathode.