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Question

Given, standard reduction potentials for half reactions:
A+eA;E0=ve
B+eB;E0=+ve
Which of the following statement(s) is/are true?

A
For a spontaneous process,
A will act as anode and B will act as cathode
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B
For a non-spontaneous process,
A will act as anode and B will act as cathode
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C
A is easily reduced
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D
None of the above
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Solution

The correct option is A For a spontaneous process,
A will act as anode and B will act as cathode
Standard reduction potentials (SRP) of the half cell electrodes are calculated and arranged in a series of increasing order which is known as electrochemical series.
The standard electrode potential of H+/H2 couple is zero.

A positive E0 signifies that it has high tendency to get reduced and the redox couple is a stronger oxidising agent than the H+/H2 couple.

Negative E0 signifies that it has high tendency to get oxidised and the redox couple is a stronger reducing agent than the H+/H2 couple.

Thus, A is easily oxidised to A

For a spontaneous process, E0cell should be a positive value.
Ecell=SRP of substance reducedSRP of substance oxidised
(SRP - Standard reduction potential)

Ecell=Ecathode (red)Eanode (red)
Ecell=(+ve)(ve)
Ecell=+ve

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