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Question

In a cell that utilises the reactions,


Zn(s)+2H+(aq)Zn2+(aq)+H2(g) addition of H2SO4 to cathode compartment will:

A
increase the E and shift equilibrium to the left
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B
lower the E and shift equilibrium to the right
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C
increase the E and shift equilibrium to the right
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D
lower the E and shift equilibrium to the left
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Solution

The correct option is C increase the E and shift equilibrium to the right
Zn(s)+2H+(aq)Zn2+(aq)+H2(g) addition of H2SO4

As we add H2SO4 in solution, conc. of hydrogen ion increases and according to the principal, reaction moves forward.

According to nernst equation,

E=Eo(0.0591/n)logQ

Ecell=Eocell+0.0592log[H+]2PH2×[Zn2+]

Addition of H2SO4 will increase [H+] and thus Ecell will be more and equilibrium will be shifted to right.

So, the correct option is C

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