In a cell that utilizes the reactions.
`Zn(s) + 2H^(+) (aq) rightarrow Zn^(2+)(aq) + H_(2)(g)`
addition of `H_(2)SO_(4)` to cathode compartment, will

Options

A. Lower the E and shift equilibrium to the left
B. lower the E and shift equilibrium to the right
C. increase the E and shift equilibrium to the right
D. Increase the E and shift equilibrium to the left

Answer

C

Explanation

`E_(cell)=E_(cell)^(@)-(0.0591)/(2)"log"([Zn^(2+)]xxp_(H_(2)))/([H^(+)]^(2))`
On adding `H_(2)SO_(4),[H^(+)]` will increase, therefore `E_(cell)` will increase. The equilibrium `Zn+2H^(+)hArrZn^(2+)+H_(2)` will shift towards right on increasing the concentration of `H^(+)` ions.