JEE MAIN - Chemistry (2004 - No. 39)
In a cell that utilises the reaction Zn(s) + 2H+
(aq) $$\to$$ Zn2+(aq) + H2(g) addition of H2SO4 to cathode compartment, will
lower the E and shift equilibrium to the left
increases the E and shift equilibrium to the left
increase the E and shift equilibrium to the right
Lower the E and shift equilibrium to the right
Explanation
$$Zn\left( s \right) + 2{H^ + } + \left( {aq} \right)\,\,\rightleftharpoons\,\,Z{n^{2 + }}\left( {aq} \right) + {H_2}\left( g \right)$$
$${E_{cell}} = E_{cell}^ \circ - {{0.059} \over 2}\log {{\left[ {Z{n^{2 + }}} \right]\left[ {{H_2}} \right]} \over {{{\left[ {{H^ + }} \right]}^2}}}$$
Addition of $${H_2}S{O_4}$$ will increases $$\left[ {{H^ + }} \right]$$ and $${E_{cell}}$$ will also increase and the equilibrium will shift towards $$RHS$$
$${E_{cell}} = E_{cell}^ \circ - {{0.059} \over 2}\log {{\left[ {Z{n^{2 + }}} \right]\left[ {{H_2}} \right]} \over {{{\left[ {{H^ + }} \right]}^2}}}$$
Addition of $${H_2}S{O_4}$$ will increases $$\left[ {{H^ + }} \right]$$ and $${E_{cell}}$$ will also increase and the equilibrium will shift towards $$RHS$$
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