Effect of Concentration on emf of cell - Nernst Equation
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CHXII03:ELECTROCHEMISTRY

329986 The potential of hydrogen electrode is\({\rm{ - 118 mV}}\). The \({{\rm{H}}^{\rm{ + }}}\) concentration of the solution is

1 \({\rm{1}}{{\rm{0}}^{{\rm{ - 4}}}}\,\,{\rm{M}}\)
2 \({\rm{2}}\,\,{\rm{M}}\)
3 \({\rm{0}}{\rm{.01}}\,\,{\rm{M}}\)
4 \({\rm{1}}\,\,{\rm{M}}\)
CHXII03:ELECTROCHEMISTRY

329987 Emf of the cell
\(\left. {{\rm{Ni}}} \right \vert \left. {{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}\left( {{\rm{0}}{\rm{.1M}}} \right)} \right\vert \left. {{\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}\left( {{\rm{1}}{\rm{.0M}}} \right)} \right \vert {\rm{Au}}\) will be
\({\rm{E}}_{\left. {{\rm{Ni}}} \right \vert {\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}}^{\rm{^\circ }}{\rm{ = 0}}{\rm{.25,}}\,\,{\rm{E}}_{\left. {{\rm{Au}}} \right \vert {\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}}^{\rm{^\circ }}{\rm{ = - 0}}{\rm{.15V}}\)

1 \({\rm{ - 1}}{\rm{.7795}}\,\,{\rm{V}}\)
2 \({\rm{ + 1}}{\rm{.7795}}\,\,{\rm{V}}\)
3 \({\rm{1}}{\rm{.75}}\,\,{\rm{V}}\)
4 \({\rm{ + 0}}{\rm{.7795}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

329988 The cell,
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right\vert \left. {{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right \vert {\rm{Cu(E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 1}}{\rm{.10V)}}\), was allowed to be completely discharged at 298 K. The relative concentration of \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{,}}\left[ {\frac{{{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}}}{{{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}}}} \right]\) is

1 \({\rm{9}}{\rm{.65 \times 1}}{{\rm{0}}^{\rm{4}}}\)
2 \({\rm{1}}{{\rm{0}}^{{\rm{37}}{\rm{.3}}}}\)
3 antilog (24.08)
4 37.3
CHXII03:ELECTROCHEMISTRY

329989 The electrode potential becomes equal to standard electrode potential when reactants and products concentration ratio is

1 Greater than 1
2 Less than 1
3 Equal to 1
4 None of the above
CHXII03:ELECTROCHEMISTRY

329990 The oxidation potential of \({\rm{0}}{\rm{.05}}\,\,{\rm{M}}\,\,{{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\) is

1 \({\rm{ - 2 \times 0}}{\rm{.0591}}\)
2 \({\rm{ - 0}}{\rm{.01 \times 0}}{\rm{.0591}}\)
3 \({\rm{ - 2}}{\rm{.321 \times 0}}{\rm{.0591}}\)
4 \({\rm{0}}{\rm{.0591}}\)
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

329986 The potential of hydrogen electrode is\({\rm{ - 118 mV}}\). The \({{\rm{H}}^{\rm{ + }}}\) concentration of the solution is

1 \({\rm{1}}{{\rm{0}}^{{\rm{ - 4}}}}\,\,{\rm{M}}\)
2 \({\rm{2}}\,\,{\rm{M}}\)
3 \({\rm{0}}{\rm{.01}}\,\,{\rm{M}}\)
4 \({\rm{1}}\,\,{\rm{M}}\)
CHXII03:ELECTROCHEMISTRY

329987 Emf of the cell
\(\left. {{\rm{Ni}}} \right \vert \left. {{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}\left( {{\rm{0}}{\rm{.1M}}} \right)} \right\vert \left. {{\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}\left( {{\rm{1}}{\rm{.0M}}} \right)} \right \vert {\rm{Au}}\) will be
\({\rm{E}}_{\left. {{\rm{Ni}}} \right \vert {\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}}^{\rm{^\circ }}{\rm{ = 0}}{\rm{.25,}}\,\,{\rm{E}}_{\left. {{\rm{Au}}} \right \vert {\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}}^{\rm{^\circ }}{\rm{ = - 0}}{\rm{.15V}}\)

1 \({\rm{ - 1}}{\rm{.7795}}\,\,{\rm{V}}\)
2 \({\rm{ + 1}}{\rm{.7795}}\,\,{\rm{V}}\)
3 \({\rm{1}}{\rm{.75}}\,\,{\rm{V}}\)
4 \({\rm{ + 0}}{\rm{.7795}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

329988 The cell,
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right\vert \left. {{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right \vert {\rm{Cu(E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 1}}{\rm{.10V)}}\), was allowed to be completely discharged at 298 K. The relative concentration of \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{,}}\left[ {\frac{{{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}}}{{{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}}}} \right]\) is

1 \({\rm{9}}{\rm{.65 \times 1}}{{\rm{0}}^{\rm{4}}}\)
2 \({\rm{1}}{{\rm{0}}^{{\rm{37}}{\rm{.3}}}}\)
3 antilog (24.08)
4 37.3
CHXII03:ELECTROCHEMISTRY

329989 The electrode potential becomes equal to standard electrode potential when reactants and products concentration ratio is

1 Greater than 1
2 Less than 1
3 Equal to 1
4 None of the above
CHXII03:ELECTROCHEMISTRY

329990 The oxidation potential of \({\rm{0}}{\rm{.05}}\,\,{\rm{M}}\,\,{{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\) is

1 \({\rm{ - 2 \times 0}}{\rm{.0591}}\)
2 \({\rm{ - 0}}{\rm{.01 \times 0}}{\rm{.0591}}\)
3 \({\rm{ - 2}}{\rm{.321 \times 0}}{\rm{.0591}}\)
4 \({\rm{0}}{\rm{.0591}}\)
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CHXII03:ELECTROCHEMISTRY

329986 The potential of hydrogen electrode is\({\rm{ - 118 mV}}\). The \({{\rm{H}}^{\rm{ + }}}\) concentration of the solution is

1 \({\rm{1}}{{\rm{0}}^{{\rm{ - 4}}}}\,\,{\rm{M}}\)
2 \({\rm{2}}\,\,{\rm{M}}\)
3 \({\rm{0}}{\rm{.01}}\,\,{\rm{M}}\)
4 \({\rm{1}}\,\,{\rm{M}}\)
CHXII03:ELECTROCHEMISTRY

329987 Emf of the cell
\(\left. {{\rm{Ni}}} \right \vert \left. {{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}\left( {{\rm{0}}{\rm{.1M}}} \right)} \right\vert \left. {{\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}\left( {{\rm{1}}{\rm{.0M}}} \right)} \right \vert {\rm{Au}}\) will be
\({\rm{E}}_{\left. {{\rm{Ni}}} \right \vert {\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}}^{\rm{^\circ }}{\rm{ = 0}}{\rm{.25,}}\,\,{\rm{E}}_{\left. {{\rm{Au}}} \right \vert {\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}}^{\rm{^\circ }}{\rm{ = - 0}}{\rm{.15V}}\)

1 \({\rm{ - 1}}{\rm{.7795}}\,\,{\rm{V}}\)
2 \({\rm{ + 1}}{\rm{.7795}}\,\,{\rm{V}}\)
3 \({\rm{1}}{\rm{.75}}\,\,{\rm{V}}\)
4 \({\rm{ + 0}}{\rm{.7795}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

329988 The cell,
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right\vert \left. {{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right \vert {\rm{Cu(E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 1}}{\rm{.10V)}}\), was allowed to be completely discharged at 298 K. The relative concentration of \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{,}}\left[ {\frac{{{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}}}{{{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}}}} \right]\) is

1 \({\rm{9}}{\rm{.65 \times 1}}{{\rm{0}}^{\rm{4}}}\)
2 \({\rm{1}}{{\rm{0}}^{{\rm{37}}{\rm{.3}}}}\)
3 antilog (24.08)
4 37.3
CHXII03:ELECTROCHEMISTRY

329989 The electrode potential becomes equal to standard electrode potential when reactants and products concentration ratio is

1 Greater than 1
2 Less than 1
3 Equal to 1
4 None of the above
CHXII03:ELECTROCHEMISTRY

329990 The oxidation potential of \({\rm{0}}{\rm{.05}}\,\,{\rm{M}}\,\,{{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\) is

1 \({\rm{ - 2 \times 0}}{\rm{.0591}}\)
2 \({\rm{ - 0}}{\rm{.01 \times 0}}{\rm{.0591}}\)
3 \({\rm{ - 2}}{\rm{.321 \times 0}}{\rm{.0591}}\)
4 \({\rm{0}}{\rm{.0591}}\)
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CHXII03:ELECTROCHEMISTRY

329986 The potential of hydrogen electrode is\({\rm{ - 118 mV}}\). The \({{\rm{H}}^{\rm{ + }}}\) concentration of the solution is

1 \({\rm{1}}{{\rm{0}}^{{\rm{ - 4}}}}\,\,{\rm{M}}\)
2 \({\rm{2}}\,\,{\rm{M}}\)
3 \({\rm{0}}{\rm{.01}}\,\,{\rm{M}}\)
4 \({\rm{1}}\,\,{\rm{M}}\)
CHXII03:ELECTROCHEMISTRY

329987 Emf of the cell
\(\left. {{\rm{Ni}}} \right \vert \left. {{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}\left( {{\rm{0}}{\rm{.1M}}} \right)} \right\vert \left. {{\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}\left( {{\rm{1}}{\rm{.0M}}} \right)} \right \vert {\rm{Au}}\) will be
\({\rm{E}}_{\left. {{\rm{Ni}}} \right \vert {\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}}^{\rm{^\circ }}{\rm{ = 0}}{\rm{.25,}}\,\,{\rm{E}}_{\left. {{\rm{Au}}} \right \vert {\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}}^{\rm{^\circ }}{\rm{ = - 0}}{\rm{.15V}}\)

1 \({\rm{ - 1}}{\rm{.7795}}\,\,{\rm{V}}\)
2 \({\rm{ + 1}}{\rm{.7795}}\,\,{\rm{V}}\)
3 \({\rm{1}}{\rm{.75}}\,\,{\rm{V}}\)
4 \({\rm{ + 0}}{\rm{.7795}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

329988 The cell,
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right\vert \left. {{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right \vert {\rm{Cu(E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 1}}{\rm{.10V)}}\), was allowed to be completely discharged at 298 K. The relative concentration of \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{,}}\left[ {\frac{{{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}}}{{{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}}}} \right]\) is

1 \({\rm{9}}{\rm{.65 \times 1}}{{\rm{0}}^{\rm{4}}}\)
2 \({\rm{1}}{{\rm{0}}^{{\rm{37}}{\rm{.3}}}}\)
3 antilog (24.08)
4 37.3
CHXII03:ELECTROCHEMISTRY

329989 The electrode potential becomes equal to standard electrode potential when reactants and products concentration ratio is

1 Greater than 1
2 Less than 1
3 Equal to 1
4 None of the above
CHXII03:ELECTROCHEMISTRY

329990 The oxidation potential of \({\rm{0}}{\rm{.05}}\,\,{\rm{M}}\,\,{{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\) is

1 \({\rm{ - 2 \times 0}}{\rm{.0591}}\)
2 \({\rm{ - 0}}{\rm{.01 \times 0}}{\rm{.0591}}\)
3 \({\rm{ - 2}}{\rm{.321 \times 0}}{\rm{.0591}}\)
4 \({\rm{0}}{\rm{.0591}}\)
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

329986 The potential of hydrogen electrode is\({\rm{ - 118 mV}}\). The \({{\rm{H}}^{\rm{ + }}}\) concentration of the solution is

1 \({\rm{1}}{{\rm{0}}^{{\rm{ - 4}}}}\,\,{\rm{M}}\)
2 \({\rm{2}}\,\,{\rm{M}}\)
3 \({\rm{0}}{\rm{.01}}\,\,{\rm{M}}\)
4 \({\rm{1}}\,\,{\rm{M}}\)
CHXII03:ELECTROCHEMISTRY

329987 Emf of the cell
\(\left. {{\rm{Ni}}} \right \vert \left. {{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}\left( {{\rm{0}}{\rm{.1M}}} \right)} \right\vert \left. {{\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}\left( {{\rm{1}}{\rm{.0M}}} \right)} \right \vert {\rm{Au}}\) will be
\({\rm{E}}_{\left. {{\rm{Ni}}} \right \vert {\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}}^{\rm{^\circ }}{\rm{ = 0}}{\rm{.25,}}\,\,{\rm{E}}_{\left. {{\rm{Au}}} \right \vert {\rm{A}}{{\rm{u}}^{{\rm{3 + }}}}}^{\rm{^\circ }}{\rm{ = - 0}}{\rm{.15V}}\)

1 \({\rm{ - 1}}{\rm{.7795}}\,\,{\rm{V}}\)
2 \({\rm{ + 1}}{\rm{.7795}}\,\,{\rm{V}}\)
3 \({\rm{1}}{\rm{.75}}\,\,{\rm{V}}\)
4 \({\rm{ + 0}}{\rm{.7795}}\,\,{\rm{V}}\)
CHXII03:ELECTROCHEMISTRY

329988 The cell,
\(\left. {{\rm{Zn}}} \right \vert \left. {{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right\vert \left. {{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{(1M)}}} \right \vert {\rm{Cu(E}}_{{\rm{cell}}}^{\rm{o}}{\rm{ = 1}}{\rm{.10V)}}\), was allowed to be completely discharged at 298 K. The relative concentration of \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\,\,{\rm{to}}\,\,{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}{\rm{,}}\left[ {\frac{{{\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}}}{{{\rm{C}}{{\rm{u}}^{{\rm{2 + }}}}}}} \right]\) is

1 \({\rm{9}}{\rm{.65 \times 1}}{{\rm{0}}^{\rm{4}}}\)
2 \({\rm{1}}{{\rm{0}}^{{\rm{37}}{\rm{.3}}}}\)
3 antilog (24.08)
4 37.3
CHXII03:ELECTROCHEMISTRY

329989 The electrode potential becomes equal to standard electrode potential when reactants and products concentration ratio is

1 Greater than 1
2 Less than 1
3 Equal to 1
4 None of the above
CHXII03:ELECTROCHEMISTRY

329990 The oxidation potential of \({\rm{0}}{\rm{.05}}\,\,{\rm{M}}\,\,{{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\) is

1 \({\rm{ - 2 \times 0}}{\rm{.0591}}\)
2 \({\rm{ - 0}}{\rm{.01 \times 0}}{\rm{.0591}}\)
3 \({\rm{ - 2}}{\rm{.321 \times 0}}{\rm{.0591}}\)
4 \({\rm{0}}{\rm{.0591}}\)