Electrochemical Series and Applications
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CHXII03:ELECTROCHEMISTRY

330094 Consider the cell potentials \({\rm{E}}_{\left. {{\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}} \right \vert {\rm{Mg}}}^{\rm{o}}{\rm{ = - 2}}{\rm{.37V}}\,\,{\rm{and}}\,\,{\rm{E}}_{\left. {{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}} \right \vert {\rm{Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.04V}}\). The best reducing agent would be

1 \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\)
2 \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\)
3 \({\rm{Fe}}\)
4 \({\rm{Mg}}\)
CHXII03:ELECTROCHEMISTRY

330095 The standard electrode potentials \(\left( {{\rm{E}}_{{{\rm{M}}^{\rm{ + }}}{\rm{/M}}}^{\rm{o}}} \right)\) of four metals \({\rm{A}},{\mkern 1mu} {\mkern 1mu} {\rm{B}},{\mkern 1mu} {\mkern 1mu} {\rm{C}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{D}}{\mkern 1mu} {\mkern 1mu} {\rm{are}}{\mkern 1mu} {\mkern 1mu} {\rm{ - }}{\mkern 1mu} {\mkern 1mu} {\rm{1}}.{\rm{2}}{\mkern 1mu} {\mkern 1mu} {\rm{V}},\)
\({\rm{0}}.{\rm{6}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}.{\rm{0}}.{\rm{85}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{ - 0}}.{\rm{076}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively. The sequence of deposition of metals on applying potential is :

1 D, A, B, C
2 C, B, D, A
3 A, D, C, A
4 A, C, B, D
JEE - 2014
CHXII03:ELECTROCHEMISTRY

330096 How many of the following can displace copper from its salt solution?
\({\mathrm{\mathrm{Zn}, \mathrm{Fe}, \mathrm{Pb}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}}}\)

1 6
2 3
3 1
4 4
CHXII03:ELECTROCHEMISTRY

330097 If a spoon of copper metal is placed in a solution of ferrous sulphate

1 No reaction will take place
2 Cu and Fe will precipitate
3 Iron will precipitate
4 Cu will precipitate out
CHXII03:ELECTROCHEMISTRY

330098 From the electrochemical series, it can be included that:

1 \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\) will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
2 Ag metal reacts spontaneously with \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\)
3 Zn metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
4 Ag metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

330094 Consider the cell potentials \({\rm{E}}_{\left. {{\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}} \right \vert {\rm{Mg}}}^{\rm{o}}{\rm{ = - 2}}{\rm{.37V}}\,\,{\rm{and}}\,\,{\rm{E}}_{\left. {{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}} \right \vert {\rm{Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.04V}}\). The best reducing agent would be

1 \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\)
2 \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\)
3 \({\rm{Fe}}\)
4 \({\rm{Mg}}\)
CHXII03:ELECTROCHEMISTRY

330095 The standard electrode potentials \(\left( {{\rm{E}}_{{{\rm{M}}^{\rm{ + }}}{\rm{/M}}}^{\rm{o}}} \right)\) of four metals \({\rm{A}},{\mkern 1mu} {\mkern 1mu} {\rm{B}},{\mkern 1mu} {\mkern 1mu} {\rm{C}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{D}}{\mkern 1mu} {\mkern 1mu} {\rm{are}}{\mkern 1mu} {\mkern 1mu} {\rm{ - }}{\mkern 1mu} {\mkern 1mu} {\rm{1}}.{\rm{2}}{\mkern 1mu} {\mkern 1mu} {\rm{V}},\)
\({\rm{0}}.{\rm{6}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}.{\rm{0}}.{\rm{85}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{ - 0}}.{\rm{076}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively. The sequence of deposition of metals on applying potential is :

1 D, A, B, C
2 C, B, D, A
3 A, D, C, A
4 A, C, B, D
JEE - 2014
CHXII03:ELECTROCHEMISTRY

330096 How many of the following can displace copper from its salt solution?
\({\mathrm{\mathrm{Zn}, \mathrm{Fe}, \mathrm{Pb}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}}}\)

1 6
2 3
3 1
4 4
CHXII03:ELECTROCHEMISTRY

330097 If a spoon of copper metal is placed in a solution of ferrous sulphate

1 No reaction will take place
2 Cu and Fe will precipitate
3 Iron will precipitate
4 Cu will precipitate out
CHXII03:ELECTROCHEMISTRY

330098 From the electrochemical series, it can be included that:

1 \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\) will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
2 Ag metal reacts spontaneously with \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\)
3 Zn metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
4 Ag metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
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CHXII03:ELECTROCHEMISTRY

330094 Consider the cell potentials \({\rm{E}}_{\left. {{\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}} \right \vert {\rm{Mg}}}^{\rm{o}}{\rm{ = - 2}}{\rm{.37V}}\,\,{\rm{and}}\,\,{\rm{E}}_{\left. {{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}} \right \vert {\rm{Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.04V}}\). The best reducing agent would be

1 \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\)
2 \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\)
3 \({\rm{Fe}}\)
4 \({\rm{Mg}}\)
CHXII03:ELECTROCHEMISTRY

330095 The standard electrode potentials \(\left( {{\rm{E}}_{{{\rm{M}}^{\rm{ + }}}{\rm{/M}}}^{\rm{o}}} \right)\) of four metals \({\rm{A}},{\mkern 1mu} {\mkern 1mu} {\rm{B}},{\mkern 1mu} {\mkern 1mu} {\rm{C}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{D}}{\mkern 1mu} {\mkern 1mu} {\rm{are}}{\mkern 1mu} {\mkern 1mu} {\rm{ - }}{\mkern 1mu} {\mkern 1mu} {\rm{1}}.{\rm{2}}{\mkern 1mu} {\mkern 1mu} {\rm{V}},\)
\({\rm{0}}.{\rm{6}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}.{\rm{0}}.{\rm{85}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{ - 0}}.{\rm{076}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively. The sequence of deposition of metals on applying potential is :

1 D, A, B, C
2 C, B, D, A
3 A, D, C, A
4 A, C, B, D
JEE - 2014
CHXII03:ELECTROCHEMISTRY

330096 How many of the following can displace copper from its salt solution?
\({\mathrm{\mathrm{Zn}, \mathrm{Fe}, \mathrm{Pb}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}}}\)

1 6
2 3
3 1
4 4
CHXII03:ELECTROCHEMISTRY

330097 If a spoon of copper metal is placed in a solution of ferrous sulphate

1 No reaction will take place
2 Cu and Fe will precipitate
3 Iron will precipitate
4 Cu will precipitate out
CHXII03:ELECTROCHEMISTRY

330098 From the electrochemical series, it can be included that:

1 \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\) will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
2 Ag metal reacts spontaneously with \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\)
3 Zn metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
4 Ag metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
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CHXII03:ELECTROCHEMISTRY

330094 Consider the cell potentials \({\rm{E}}_{\left. {{\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}} \right \vert {\rm{Mg}}}^{\rm{o}}{\rm{ = - 2}}{\rm{.37V}}\,\,{\rm{and}}\,\,{\rm{E}}_{\left. {{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}} \right \vert {\rm{Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.04V}}\). The best reducing agent would be

1 \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\)
2 \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\)
3 \({\rm{Fe}}\)
4 \({\rm{Mg}}\)
CHXII03:ELECTROCHEMISTRY

330095 The standard electrode potentials \(\left( {{\rm{E}}_{{{\rm{M}}^{\rm{ + }}}{\rm{/M}}}^{\rm{o}}} \right)\) of four metals \({\rm{A}},{\mkern 1mu} {\mkern 1mu} {\rm{B}},{\mkern 1mu} {\mkern 1mu} {\rm{C}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{D}}{\mkern 1mu} {\mkern 1mu} {\rm{are}}{\mkern 1mu} {\mkern 1mu} {\rm{ - }}{\mkern 1mu} {\mkern 1mu} {\rm{1}}.{\rm{2}}{\mkern 1mu} {\mkern 1mu} {\rm{V}},\)
\({\rm{0}}.{\rm{6}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}.{\rm{0}}.{\rm{85}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{ - 0}}.{\rm{076}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively. The sequence of deposition of metals on applying potential is :

1 D, A, B, C
2 C, B, D, A
3 A, D, C, A
4 A, C, B, D
JEE - 2014
CHXII03:ELECTROCHEMISTRY

330096 How many of the following can displace copper from its salt solution?
\({\mathrm{\mathrm{Zn}, \mathrm{Fe}, \mathrm{Pb}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}}}\)

1 6
2 3
3 1
4 4
CHXII03:ELECTROCHEMISTRY

330097 If a spoon of copper metal is placed in a solution of ferrous sulphate

1 No reaction will take place
2 Cu and Fe will precipitate
3 Iron will precipitate
4 Cu will precipitate out
CHXII03:ELECTROCHEMISTRY

330098 From the electrochemical series, it can be included that:

1 \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\) will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
2 Ag metal reacts spontaneously with \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\)
3 Zn metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
4 Ag metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
NEET DIGITAL LIBRARY
CHXII03:ELECTROCHEMISTRY

330094 Consider the cell potentials \({\rm{E}}_{\left. {{\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}} \right \vert {\rm{Mg}}}^{\rm{o}}{\rm{ = - 2}}{\rm{.37V}}\,\,{\rm{and}}\,\,{\rm{E}}_{\left. {{\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}} \right \vert {\rm{Fe}}}^{\rm{o}}{\rm{ = - 0}}{\rm{.04V}}\). The best reducing agent would be

1 \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\)
2 \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\)
3 \({\rm{Fe}}\)
4 \({\rm{Mg}}\)
CHXII03:ELECTROCHEMISTRY

330095 The standard electrode potentials \(\left( {{\rm{E}}_{{{\rm{M}}^{\rm{ + }}}{\rm{/M}}}^{\rm{o}}} \right)\) of four metals \({\rm{A}},{\mkern 1mu} {\mkern 1mu} {\rm{B}},{\mkern 1mu} {\mkern 1mu} {\rm{C}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{D}}{\mkern 1mu} {\mkern 1mu} {\rm{are}}{\mkern 1mu} {\mkern 1mu} {\rm{ - }}{\mkern 1mu} {\mkern 1mu} {\rm{1}}.{\rm{2}}{\mkern 1mu} {\mkern 1mu} {\rm{V}},\)
\({\rm{0}}.{\rm{6}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}.{\rm{0}}.{\rm{85}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}{\mkern 1mu} {\mkern 1mu} {\rm{and}}{\mkern 1mu} {\mkern 1mu} {\rm{ - 0}}.{\rm{076}}{\mkern 1mu} {\mkern 1mu} {\rm{V}}\) respectively. The sequence of deposition of metals on applying potential is :

1 D, A, B, C
2 C, B, D, A
3 A, D, C, A
4 A, C, B, D
JEE - 2014
CHXII03:ELECTROCHEMISTRY

330096 How many of the following can displace copper from its salt solution?
\({\mathrm{\mathrm{Zn}, \mathrm{Fe}, \mathrm{Pb}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}}}\)

1 6
2 3
3 1
4 4
CHXII03:ELECTROCHEMISTRY

330097 If a spoon of copper metal is placed in a solution of ferrous sulphate

1 No reaction will take place
2 Cu and Fe will precipitate
3 Iron will precipitate
4 Cu will precipitate out
CHXII03:ELECTROCHEMISTRY

330098 From the electrochemical series, it can be included that:

1 \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\) will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
2 Ag metal reacts spontaneously with \({\rm{Z}}{{\rm{n}}^{{\rm{2 + }}}}\)
3 Zn metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl
4 Ag metal will liberate \({{\rm{H}}_{\rm{2}}}\) from 1 M HCl