Electrochemical Cells or Galvanic Cells
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CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes
2 Potential difference develops between two different electrolytes
3 Potential difference develops between electrode and electrolyte
4 All of the above
CHXII03:ELECTROCHEMISTRY

330076 \({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} {F_2} + 2e \to 2{F^ - }{\mkern 1mu} {\mkern 1mu} is{\mkern 1mu} {\mkern 1mu} \,\,2.8{\mkern 1mu} {\mkern 1mu} V,{\mkern 1mu} {\mkern 1mu} \)
\({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} \frac{1}{2}{F_2} + e \to {F^ - }{\mkern 1mu} {\mkern 1mu} is\)

1 – 1.4 V
2 – 2.8 V
3 2.8 V
4 1.4 V
CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.
2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.
3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly
4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly
CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Zn,}}\,\,{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}{\rm{/Ni}}\,\,{\rm{and}}\,\,{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}\)\({\rm{are}}\,\,{\rm{ - 0}}{\rm{.76,}}\,\,{\rm{ - 0}}{\rm{.23}}\,\,{\rm{and}}\,\,{\rm{ - 0}}{\rm{.44}}\,\,{\rm{V}}\) respectively. The reaction \(X + {Y^{2 + }} \to {X^2} + Y\) will be spontaneous when

1 \({\rm{X = Zn,Y = Ni}}\)
2 \({\rm{X = Ni,Y = Fe}}\)
3 \({\rm{X = Ni,Y = Zn}}\)
4 \({\rm{X = Fe,Y = Zn}}\)
CHXII03:ELECTROCHEMISTRY

330079 Consider the following \({{\rm{E}}^{\rm{o}}}\) values:
\({\rm{E}}_{{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}{\rm{/F}}{{\rm{e}}^{{\rm{2 + }}}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.77}}\,\,{\rm{V}}\)
\({\rm{E}}_{{\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Sn}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.14}}\,\,{\rm{V}}\)
Under standard conditions the potential for the reaction
\({\rm{Sn}}\left( s \right) + 2F{e^{3 + }}\left( {aq} \right) \to 2F{e^{2 + }}\left( {sq} \right) + S{n^{2 + }}\left( {aq} \right)\) is

1 0.91 V
2 0.63 V
3 1.40 V
4 1.68 V
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes
2 Potential difference develops between two different electrolytes
3 Potential difference develops between electrode and electrolyte
4 All of the above
CHXII03:ELECTROCHEMISTRY

330076 \({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} {F_2} + 2e \to 2{F^ - }{\mkern 1mu} {\mkern 1mu} is{\mkern 1mu} {\mkern 1mu} \,\,2.8{\mkern 1mu} {\mkern 1mu} V,{\mkern 1mu} {\mkern 1mu} \)
\({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} \frac{1}{2}{F_2} + e \to {F^ - }{\mkern 1mu} {\mkern 1mu} is\)

1 – 1.4 V
2 – 2.8 V
3 2.8 V
4 1.4 V
CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.
2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.
3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly
4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly
CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Zn,}}\,\,{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}{\rm{/Ni}}\,\,{\rm{and}}\,\,{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}\)\({\rm{are}}\,\,{\rm{ - 0}}{\rm{.76,}}\,\,{\rm{ - 0}}{\rm{.23}}\,\,{\rm{and}}\,\,{\rm{ - 0}}{\rm{.44}}\,\,{\rm{V}}\) respectively. The reaction \(X + {Y^{2 + }} \to {X^2} + Y\) will be spontaneous when

1 \({\rm{X = Zn,Y = Ni}}\)
2 \({\rm{X = Ni,Y = Fe}}\)
3 \({\rm{X = Ni,Y = Zn}}\)
4 \({\rm{X = Fe,Y = Zn}}\)
CHXII03:ELECTROCHEMISTRY

330079 Consider the following \({{\rm{E}}^{\rm{o}}}\) values:
\({\rm{E}}_{{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}{\rm{/F}}{{\rm{e}}^{{\rm{2 + }}}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.77}}\,\,{\rm{V}}\)
\({\rm{E}}_{{\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Sn}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.14}}\,\,{\rm{V}}\)
Under standard conditions the potential for the reaction
\({\rm{Sn}}\left( s \right) + 2F{e^{3 + }}\left( {aq} \right) \to 2F{e^{2 + }}\left( {sq} \right) + S{n^{2 + }}\left( {aq} \right)\) is

1 0.91 V
2 0.63 V
3 1.40 V
4 1.68 V
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CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes
2 Potential difference develops between two different electrolytes
3 Potential difference develops between electrode and electrolyte
4 All of the above
CHXII03:ELECTROCHEMISTRY

330076 \({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} {F_2} + 2e \to 2{F^ - }{\mkern 1mu} {\mkern 1mu} is{\mkern 1mu} {\mkern 1mu} \,\,2.8{\mkern 1mu} {\mkern 1mu} V,{\mkern 1mu} {\mkern 1mu} \)
\({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} \frac{1}{2}{F_2} + e \to {F^ - }{\mkern 1mu} {\mkern 1mu} is\)

1 – 1.4 V
2 – 2.8 V
3 2.8 V
4 1.4 V
CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.
2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.
3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly
4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly
CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Zn,}}\,\,{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}{\rm{/Ni}}\,\,{\rm{and}}\,\,{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}\)\({\rm{are}}\,\,{\rm{ - 0}}{\rm{.76,}}\,\,{\rm{ - 0}}{\rm{.23}}\,\,{\rm{and}}\,\,{\rm{ - 0}}{\rm{.44}}\,\,{\rm{V}}\) respectively. The reaction \(X + {Y^{2 + }} \to {X^2} + Y\) will be spontaneous when

1 \({\rm{X = Zn,Y = Ni}}\)
2 \({\rm{X = Ni,Y = Fe}}\)
3 \({\rm{X = Ni,Y = Zn}}\)
4 \({\rm{X = Fe,Y = Zn}}\)
CHXII03:ELECTROCHEMISTRY

330079 Consider the following \({{\rm{E}}^{\rm{o}}}\) values:
\({\rm{E}}_{{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}{\rm{/F}}{{\rm{e}}^{{\rm{2 + }}}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.77}}\,\,{\rm{V}}\)
\({\rm{E}}_{{\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Sn}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.14}}\,\,{\rm{V}}\)
Under standard conditions the potential for the reaction
\({\rm{Sn}}\left( s \right) + 2F{e^{3 + }}\left( {aq} \right) \to 2F{e^{2 + }}\left( {sq} \right) + S{n^{2 + }}\left( {aq} \right)\) is

1 0.91 V
2 0.63 V
3 1.40 V
4 1.68 V
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CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes
2 Potential difference develops between two different electrolytes
3 Potential difference develops between electrode and electrolyte
4 All of the above
CHXII03:ELECTROCHEMISTRY

330076 \({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} {F_2} + 2e \to 2{F^ - }{\mkern 1mu} {\mkern 1mu} is{\mkern 1mu} {\mkern 1mu} \,\,2.8{\mkern 1mu} {\mkern 1mu} V,{\mkern 1mu} {\mkern 1mu} \)
\({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} \frac{1}{2}{F_2} + e \to {F^ - }{\mkern 1mu} {\mkern 1mu} is\)

1 – 1.4 V
2 – 2.8 V
3 2.8 V
4 1.4 V
CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.
2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.
3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly
4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly
CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Zn,}}\,\,{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}{\rm{/Ni}}\,\,{\rm{and}}\,\,{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}\)\({\rm{are}}\,\,{\rm{ - 0}}{\rm{.76,}}\,\,{\rm{ - 0}}{\rm{.23}}\,\,{\rm{and}}\,\,{\rm{ - 0}}{\rm{.44}}\,\,{\rm{V}}\) respectively. The reaction \(X + {Y^{2 + }} \to {X^2} + Y\) will be spontaneous when

1 \({\rm{X = Zn,Y = Ni}}\)
2 \({\rm{X = Ni,Y = Fe}}\)
3 \({\rm{X = Ni,Y = Zn}}\)
4 \({\rm{X = Fe,Y = Zn}}\)
CHXII03:ELECTROCHEMISTRY

330079 Consider the following \({{\rm{E}}^{\rm{o}}}\) values:
\({\rm{E}}_{{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}{\rm{/F}}{{\rm{e}}^{{\rm{2 + }}}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.77}}\,\,{\rm{V}}\)
\({\rm{E}}_{{\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Sn}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.14}}\,\,{\rm{V}}\)
Under standard conditions the potential for the reaction
\({\rm{Sn}}\left( s \right) + 2F{e^{3 + }}\left( {aq} \right) \to 2F{e^{2 + }}\left( {sq} \right) + S{n^{2 + }}\left( {aq} \right)\) is

1 0.91 V
2 0.63 V
3 1.40 V
4 1.68 V
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes
2 Potential difference develops between two different electrolytes
3 Potential difference develops between electrode and electrolyte
4 All of the above
CHXII03:ELECTROCHEMISTRY

330076 \({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} {F_2} + 2e \to 2{F^ - }{\mkern 1mu} {\mkern 1mu} is{\mkern 1mu} {\mkern 1mu} \,\,2.8{\mkern 1mu} {\mkern 1mu} V,{\mkern 1mu} {\mkern 1mu} \)
\({E^o}{\mkern 1mu} {\mkern 1mu} for{\mkern 1mu} {\mkern 1mu} \frac{1}{2}{F_2} + e \to {F^ - }{\mkern 1mu} {\mkern 1mu} is\)

1 – 1.4 V
2 – 2.8 V
3 2.8 V
4 1.4 V
CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.
2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.
3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly
4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly
CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Zn,}}\,\,{\rm{N}}{{\rm{i}}^{{\rm{2 + }}}}{\rm{/Ni}}\,\,{\rm{and}}\,\,{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}}{\rm{/Fe}}\)\({\rm{are}}\,\,{\rm{ - 0}}{\rm{.76,}}\,\,{\rm{ - 0}}{\rm{.23}}\,\,{\rm{and}}\,\,{\rm{ - 0}}{\rm{.44}}\,\,{\rm{V}}\) respectively. The reaction \(X + {Y^{2 + }} \to {X^2} + Y\) will be spontaneous when

1 \({\rm{X = Zn,Y = Ni}}\)
2 \({\rm{X = Ni,Y = Fe}}\)
3 \({\rm{X = Ni,Y = Zn}}\)
4 \({\rm{X = Fe,Y = Zn}}\)
CHXII03:ELECTROCHEMISTRY

330079 Consider the following \({{\rm{E}}^{\rm{o}}}\) values:
\({\rm{E}}_{{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}{\rm{/F}}{{\rm{e}}^{{\rm{2 + }}}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.77}}\,\,{\rm{V}}\)
\({\rm{E}}_{{\rm{S}}{{\rm{n}}^{{\rm{2 + }}}}{\rm{/Sn}}}^{\rm{o}}{\rm{ = + 0}}{\rm{.14}}\,\,{\rm{V}}\)
Under standard conditions the potential for the reaction
\({\rm{Sn}}\left( s \right) + 2F{e^{3 + }}\left( {aq} \right) \to 2F{e^{2 + }}\left( {sq} \right) + S{n^{2 + }}\left( {aq} \right)\) is

1 0.91 V
2 0.63 V
3 1.40 V
4 1.68 V