Electrochemical Cells or Galvanic Cells
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CHXII03:ELECTROCHEMISTRY

330062 What will be the emf of the following concentration cell at \({\rm{25^\circ C}}\)?
\(\left. {{\rm{A}}{{\rm{g}}_{\left( {\rm{s}} \right)}}} \right \vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.05M)}}} \right \vert {\rm{A}}{{\rm{g}}_{{\rm{(s)}}}}\)

1 0.828 V
2 0.0413 V
3 \({\rm{ - 0}}{\rm{.0413}}\,\,{\rm{V}}\)
4 \({\rm{ - 0}}{\rm{.828}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330063 For the electrochemical cell,
\(\mathrm{Ag}^{+} \vert \mathrm{AgCl} \vert \mathrm{KCl} \vert \vert \mathrm{AgNO}_{3} \mid \mathrm{Ag}^{+}\), the overall cell reaction is

1 \(\mathrm{Ag}^{+}+\mathrm{KCl} \longrightarrow \mathrm{AgCl}(s)+\mathrm{K}^{+}\)
2 \(\mathrm{Ag}+\mathrm{AgCl} \longrightarrow 2 \mathrm{Ag}+\dfrac{1}{2} \mathrm{Cl}_{2}\)
3 \(\mathrm{AgCl}(s) \longrightarrow \mathrm{Ag}^{+}+\mathrm{Cl}^{-}\)
4 \(\mathrm{Ag}^{+}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AgCl}(\mathrm{s})\)
CHXII03:ELECTROCHEMISTRY

330064 Standard electrode potential for \({\rm{S}}{{\rm{n}}^{{\rm{4 + }}}}{\rm{/S}}{{\rm{n}}^{{\rm{2 + }}}}\) couple is \({\rm{ + 0}}{\rm{.15}}\,\,{\rm{V}}\) and that for the \({\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}\) couple is \({\rm{ - 0}}{\rm{.74}}\,\,{\rm{V}}\). These two couple in their standard state are connected to make a cell. The cell potential will be

1 \({\rm{ + 0}}{\rm{.18}}\,\,{\rm{V}}\)
2 \({\rm{ + 0}}{\rm{.89}}\,\,{\rm{V}}\)
3 \({\rm{ + 1}}{\rm{.83}}\,\,{\rm{V}}\)
4 \({\rm{ + 1}}{\rm{.19}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330065 The oxidation potential of a hydrogen electrode at \({\rm{pH = 10}}\,\,{\rm{and}}\,\,{{\rm{p}}_{{{\rm{H}}_{\rm{2}}}}}{\rm{ = 1}}\,\,{\rm{atm}}\) is

1 \({\rm{ - 0}}{\rm{.59}}\,\,{\rm{V}}\)
2 \({\rm{0}}{\rm{.00}}\,\,{\rm{V}}\)
3 \({\rm{ + 0}}{\rm{.59}}\,\,{\rm{V}}\)
4 \({\rm{0}}{\rm{.059}}\,\,{\rm{V}}\)
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CHXII03:ELECTROCHEMISTRY

330062 What will be the emf of the following concentration cell at \({\rm{25^\circ C}}\)?
\(\left. {{\rm{A}}{{\rm{g}}_{\left( {\rm{s}} \right)}}} \right \vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.05M)}}} \right \vert {\rm{A}}{{\rm{g}}_{{\rm{(s)}}}}\)

1 0.828 V
2 0.0413 V
3 \({\rm{ - 0}}{\rm{.0413}}\,\,{\rm{V}}\)
4 \({\rm{ - 0}}{\rm{.828}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330063 For the electrochemical cell,
\(\mathrm{Ag}^{+} \vert \mathrm{AgCl} \vert \mathrm{KCl} \vert \vert \mathrm{AgNO}_{3} \mid \mathrm{Ag}^{+}\), the overall cell reaction is

1 \(\mathrm{Ag}^{+}+\mathrm{KCl} \longrightarrow \mathrm{AgCl}(s)+\mathrm{K}^{+}\)
2 \(\mathrm{Ag}+\mathrm{AgCl} \longrightarrow 2 \mathrm{Ag}+\dfrac{1}{2} \mathrm{Cl}_{2}\)
3 \(\mathrm{AgCl}(s) \longrightarrow \mathrm{Ag}^{+}+\mathrm{Cl}^{-}\)
4 \(\mathrm{Ag}^{+}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AgCl}(\mathrm{s})\)
CHXII03:ELECTROCHEMISTRY

330064 Standard electrode potential for \({\rm{S}}{{\rm{n}}^{{\rm{4 + }}}}{\rm{/S}}{{\rm{n}}^{{\rm{2 + }}}}\) couple is \({\rm{ + 0}}{\rm{.15}}\,\,{\rm{V}}\) and that for the \({\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}\) couple is \({\rm{ - 0}}{\rm{.74}}\,\,{\rm{V}}\). These two couple in their standard state are connected to make a cell. The cell potential will be

1 \({\rm{ + 0}}{\rm{.18}}\,\,{\rm{V}}\)
2 \({\rm{ + 0}}{\rm{.89}}\,\,{\rm{V}}\)
3 \({\rm{ + 1}}{\rm{.83}}\,\,{\rm{V}}\)
4 \({\rm{ + 1}}{\rm{.19}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330065 The oxidation potential of a hydrogen electrode at \({\rm{pH = 10}}\,\,{\rm{and}}\,\,{{\rm{p}}_{{{\rm{H}}_{\rm{2}}}}}{\rm{ = 1}}\,\,{\rm{atm}}\) is

1 \({\rm{ - 0}}{\rm{.59}}\,\,{\rm{V}}\)
2 \({\rm{0}}{\rm{.00}}\,\,{\rm{V}}\)
3 \({\rm{ + 0}}{\rm{.59}}\,\,{\rm{V}}\)
4 \({\rm{0}}{\rm{.059}}\,\,{\rm{V}}\)
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CHXII03:ELECTROCHEMISTRY

330062 What will be the emf of the following concentration cell at \({\rm{25^\circ C}}\)?
\(\left. {{\rm{A}}{{\rm{g}}_{\left( {\rm{s}} \right)}}} \right \vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.05M)}}} \right \vert {\rm{A}}{{\rm{g}}_{{\rm{(s)}}}}\)

1 0.828 V
2 0.0413 V
3 \({\rm{ - 0}}{\rm{.0413}}\,\,{\rm{V}}\)
4 \({\rm{ - 0}}{\rm{.828}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330063 For the electrochemical cell,
\(\mathrm{Ag}^{+} \vert \mathrm{AgCl} \vert \mathrm{KCl} \vert \vert \mathrm{AgNO}_{3} \mid \mathrm{Ag}^{+}\), the overall cell reaction is

1 \(\mathrm{Ag}^{+}+\mathrm{KCl} \longrightarrow \mathrm{AgCl}(s)+\mathrm{K}^{+}\)
2 \(\mathrm{Ag}+\mathrm{AgCl} \longrightarrow 2 \mathrm{Ag}+\dfrac{1}{2} \mathrm{Cl}_{2}\)
3 \(\mathrm{AgCl}(s) \longrightarrow \mathrm{Ag}^{+}+\mathrm{Cl}^{-}\)
4 \(\mathrm{Ag}^{+}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AgCl}(\mathrm{s})\)
CHXII03:ELECTROCHEMISTRY

330064 Standard electrode potential for \({\rm{S}}{{\rm{n}}^{{\rm{4 + }}}}{\rm{/S}}{{\rm{n}}^{{\rm{2 + }}}}\) couple is \({\rm{ + 0}}{\rm{.15}}\,\,{\rm{V}}\) and that for the \({\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}\) couple is \({\rm{ - 0}}{\rm{.74}}\,\,{\rm{V}}\). These two couple in their standard state are connected to make a cell. The cell potential will be

1 \({\rm{ + 0}}{\rm{.18}}\,\,{\rm{V}}\)
2 \({\rm{ + 0}}{\rm{.89}}\,\,{\rm{V}}\)
3 \({\rm{ + 1}}{\rm{.83}}\,\,{\rm{V}}\)
4 \({\rm{ + 1}}{\rm{.19}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330065 The oxidation potential of a hydrogen electrode at \({\rm{pH = 10}}\,\,{\rm{and}}\,\,{{\rm{p}}_{{{\rm{H}}_{\rm{2}}}}}{\rm{ = 1}}\,\,{\rm{atm}}\) is

1 \({\rm{ - 0}}{\rm{.59}}\,\,{\rm{V}}\)
2 \({\rm{0}}{\rm{.00}}\,\,{\rm{V}}\)
3 \({\rm{ + 0}}{\rm{.59}}\,\,{\rm{V}}\)
4 \({\rm{0}}{\rm{.059}}\,\,{\rm{V}}\)
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CHXII03:ELECTROCHEMISTRY

330062 What will be the emf of the following concentration cell at \({\rm{25^\circ C}}\)?
\(\left. {{\rm{A}}{{\rm{g}}_{\left( {\rm{s}} \right)}}} \right \vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.01M)}}} \right\vert \left. {{\rm{AgN}}{{\rm{O}}_{\rm{3}}}{\rm{(0}}{\rm{.05M)}}} \right \vert {\rm{A}}{{\rm{g}}_{{\rm{(s)}}}}\)

1 0.828 V
2 0.0413 V
3 \({\rm{ - 0}}{\rm{.0413}}\,\,{\rm{V}}\)
4 \({\rm{ - 0}}{\rm{.828}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330063 For the electrochemical cell,
\(\mathrm{Ag}^{+} \vert \mathrm{AgCl} \vert \mathrm{KCl} \vert \vert \mathrm{AgNO}_{3} \mid \mathrm{Ag}^{+}\), the overall cell reaction is

1 \(\mathrm{Ag}^{+}+\mathrm{KCl} \longrightarrow \mathrm{AgCl}(s)+\mathrm{K}^{+}\)
2 \(\mathrm{Ag}+\mathrm{AgCl} \longrightarrow 2 \mathrm{Ag}+\dfrac{1}{2} \mathrm{Cl}_{2}\)
3 \(\mathrm{AgCl}(s) \longrightarrow \mathrm{Ag}^{+}+\mathrm{Cl}^{-}\)
4 \(\mathrm{Ag}^{+}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AgCl}(\mathrm{s})\)
CHXII03:ELECTROCHEMISTRY

330064 Standard electrode potential for \({\rm{S}}{{\rm{n}}^{{\rm{4 + }}}}{\rm{/S}}{{\rm{n}}^{{\rm{2 + }}}}\) couple is \({\rm{ + 0}}{\rm{.15}}\,\,{\rm{V}}\) and that for the \({\rm{C}}{{\rm{r}}^{{\rm{3 + }}}}{\rm{/Cr}}\) couple is \({\rm{ - 0}}{\rm{.74}}\,\,{\rm{V}}\). These two couple in their standard state are connected to make a cell. The cell potential will be

1 \({\rm{ + 0}}{\rm{.18}}\,\,{\rm{V}}\)
2 \({\rm{ + 0}}{\rm{.89}}\,\,{\rm{V}}\)
3 \({\rm{ + 1}}{\rm{.83}}\,\,{\rm{V}}\)
4 \({\rm{ + 1}}{\rm{.19}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

330065 The oxidation potential of a hydrogen electrode at \({\rm{pH = 10}}\,\,{\rm{and}}\,\,{{\rm{p}}_{{{\rm{H}}_{\rm{2}}}}}{\rm{ = 1}}\,\,{\rm{atm}}\) is

1 \({\rm{ - 0}}{\rm{.59}}\,\,{\rm{V}}\)
2 \({\rm{0}}{\rm{.00}}\,\,{\rm{V}}\)
3 \({\rm{ + 0}}{\rm{.59}}\,\,{\rm{V}}\)
4 \({\rm{0}}{\rm{.059}}\,\,{\rm{V}}\)
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