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Byju's Answer
Standard XII
Chemistry
Nernst Equation
Refer to the ...
Question

Refer to the following experimental data.

Half ReactionEo
I. Mg→Mg2++2e−2.37V
II. Mn→Mn2++2e−1.03V
III. H2→2H++2e−0.00V
IV. Cu→Cu2++2e−-0.16V
What will be the standard reduction potential for the reaction: Mg+Mn2+→Mg2++Mn?

A
-0.16V
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B
-1.34V
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C
1.03V
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D
1.34V
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Solution

The correct option is D 1.34V
Eocell=EoC−EoA
EoMg2+/Mg=−2.37V (more −ve reduction potential)
EoMn2+/Mn=−1.03V (less −ve reduction potential)
Eocell=−10.3−(−2.37)=1.34V

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Q.
Half ReactionEo
I. Mg→Mg2++2e−2.37V
II. Mn→Mn2++2e−1.03V
III. H2→2H++2e−0.00V
IV. Cu→Cu2++2e−-0.16V

From the above experimental data what will be the standard reduction potential which represents spontaneous process?
Q. Refer to the following experimental data.
Half ReactionEo
I. Mg→Mg2++2e−2.37V
II. Mn→Mn2++2e−1.03V
III. H2→2H++2e−0.00V
IV. Cu→Cu2++2e−-0.16V
Which of the following reactions is spontaneous?
Q.
Half ReactionEo
I. Mg→Mg2++2e−2.37V
II. Mn→Mn2++2e−1.03V
III. H2→2H++2e−0.00V
IV. Cu→Cu2++2e−-0.16V
From the above experimental data which of the following represents a spontaneous process?
Q. Rank the following elements by increasing ease of oxidation with most easily oxidized LAST:
Cd,Cu,Ni,Fe

Standard Reduction Potentials at 25∘C
Half-ReactionE∘(V)
F2+2e−→2F−2.87
Ag2+e−→Ag+1.99
Co3++e−→Co2+1.82
H2O2+2H++2e−→2H2O1.78
MnO−4+4H++3e−→MnO2+2H2O1.68
2e−+2H++IO−4→IO−3+H2O1.60
MnO−4+8H++5e−→Mn2++4H2O1.51
Au3++3e−→Au1.50
Cl2+2e−→2Cl−1.36
O2+4H++4e−→2H2O1.23
MnO2+4H++2e−→Mn2++2H2O1.21
Br2+2e−→2Br−1.09
NO−3+4H++3e−→NO+2H2O0.96
ClO2+e−→ClO20.954
2Hg2++2e−→Hg2+20.91
Ag++e−→Ag0.80
Hg2+2+2e−→2Hg0.80
Fe3++e−→Fe2+0.77
O2+2H++2e−→H2O20.68
MnO−4+e−→MnO2−40.56
I2+2e−→2I−0.54
Cu++e−→Cu0.52
O2+2H2O+4e−→4OH−0.40
Cu2++2e−→Cu0.34
AgCl+e−→Ag+Cl−0.22
Cu2++e−→Cu+0.16
2H++2e−→H20.00
Fe3++3e−→Fe−0.036
Pb2++2e−→Pb−0.13
Ni2++2e−→Ni−0.23
Cd2++2e−→Cd−0.40
Fe2++2e−→Fe−0.44
Cr3++e−→Cr2+−0.50
Cr3++3e−→Cr−0.73
Zn2++2e−→Zn−0.76
2H2O+2e−→H2+2OH−−0.83
Mn2++2e−→Mn−1.18
Al3++3e−→Al−1.66
H2+2e−→2H−−2.23
Mg2++2e−→Mg−2.37
Na++e−→Na−2.71
Ca2++2e−→Ca−2.76
Ba2++2e−→Ba−2.90
K++e−→K−2.92
Li++e−→Li−3.05

Q. Find the △G∘ of a galvanic cell with Ag and Al.
Standard Reduction Potentials at 25∘C
Half-ReactionE∘(V)
F2+2e−→2F−2.87
Ag2+e−→Ag+1.99
Co3++e−→Co2+1.82
H2O2+2H++2e−→2H2O1.78
MnO−4+4H++3e−→MnO2+2H2O1.68
2e−+2H++IO−4→IO−3+H2O1.60
MnO−4+8H++5e−→Mn2++4H2O1.51
Au3++3e−→Au1.50
Cl2+2e−→2Cl−1.36
O2+4H++4e−→2H2O1.23
MnO2+4H++2e−→Mn2++2H2O1.21
Br2+2e−→2Br−1.09
NO−3+4H++3e−→NO+2H2O0.96
ClO2+e−→ClO20.954
2Hg2++2e−→Hg2+20.91
Ag++e−→Ag0.80
Hg2+2+2e−→2Hg0.80
Fe3++e−→Fe2+0.77
O2+2H++2e−→H2O20.68
MnO−4+e−→MnO2−40.56
I2+2e−→2I−0.54
Cu++e−→Cu0.52
O2+2H2O+4e−→4OH−0.40
Cu2++2e−→Cu0.34
AgCl+e−→Ag+Cl−0.22
Cu2++e−→Cu+0.16
2H++2e−→H20.00
Fe3++3e−→Fe−0.036
Pb2++2e−→Pb−0.13
Ni2++2e−→Ni−0.23
Cd2++2e−→Cd−0.40
Fe2++2e−→Fe−0.44
Cr3++e−→Cr2+−0.50
Cr3++3e−→Cr−0.73
Zn2++2e−→Zn−0.76
2H2O+2e−→H2+2OH−−0.83
Mn2++2e−→Mn−1.18
Al3++3e−→Al−1.66
H2+2e−→2H−−2.23
Mg2++2e−→Mg−2.37
Na++e−→Na−2.71
Ca2++2e−→Ca−2.76
Ba2++2e−→Ba−2.90
K++e−→K−2.92
Li++e−→Li−3.05

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