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Question

Given three reactions:
Reaction 1 :
A (aq.)An+ (aq.)+ne
E=+2 V

Reaction 2:
B (aq.)Bn+ (aq.)+ne
E=3 V

Reaction 3:
Cn+ (aq.)+neC (aq.)
E=+4 V

The correct decreasing order of the tendency of the species A, B and C to get oxidised is:

A
A>B>C
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B
C>B>A
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C
A>C>B
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D
B>C>A
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Solution

The correct option is A A>B>C
For any reaction if Ecell>0, the forward reaction is spontaneous. If Ecell<0, the backward reaction is spontaneous.

For Reaction 1 :
A (aq.)An+ (aq.)+ne
E=+2 V
Oxidation is spontaneous

Reaction 2:
B (aq.)Bn+ (aq.)+ne
E=3 V
Backward reaction i.e. reduction is spontaneous
Reaction 3:
Cn+ (aq.)+neC (aq.)
E=+4 V
Forward reaction i.e. reduction is spontaneous

So, tendency of A is the highest for oxidation.
Between reaction 2 and reaction 3:
In reaction 2, E for backward reaction (reduction reaction) is +3V , whereas for reaction 3 E for reduction is +4V
So, C has the highest tendency to get reduced, and thus the least tendency to get oxidised.
Correct decreasing order is:
A>B>C

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