Given, standard reduction potentials for half reactions: A+e−→A−;E0=−ve B+e−→B−;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. E∘cell=SRP of substance reduced−SRP of substance oxidised
(SRP - Standard reduction potential)