Question

In a cell that utilizes the reaction

$\text{Z}\text{n}_{(s)}\text{ + 2}{\text{H}^{+}}_{(\text{aq})} \rightarrow \text{Z}{\text{n}^{\text{2+}}}_{(\text{aq})}\text{ + }\text{H}_{2(g)},$ addition of H2SO4 to cathode compartment will :

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

Answer 1

Answer: (C)

Increase the E and shift the equilibrium to the right.

Answer 2

$\mathrm { Zn } + 2 \mathrm { H } ^ { + } { } _ { ( \mathrm { aq } ) } \longrightarrow \mathrm { Zn } ^ { 2 + } ( \mathrm { aq } ) + \mathrm { H } _ { 2 } ( \mathrm {~g} )$

$E = E^{0} - \frac{0.0591}{2}\log$Adding H2SO4 means increasing H+ and therefore Ecell will increase and reaction will shift to forward direction