Question
Consider the following reactions
$${\text{(i)}}C{d^{2 + }}\left( {aq} \right) + 2{e^ - } \to $$ $$Cd\left( s \right),{E^ \circ } = - 0.40\,V$$
$${\text{(ii)}}A{g^ + }\left( {aq} \right) + {e^ - } \to $$ $$Ag\left( s \right),{E^ \circ } = 0.80\,V$$
For the galvanic cell involving the above reactions. Which of the following is not correct ?
A.
Molar concentration of the cation in the cathodic compartment changes faster than that of the cation in the anodic compartment.
B.
$${E_{cell}}$$ increase when $$C{d^{2 + }}$$ solution is diluted.
C.
Twice as many electrons pass through the cadmium electrode as through silver electrode.
D.
$${E_{cell}}$$ decreases when $$A{g^ + }$$ solution is diluted.
Answer :
Twice as many electrons pass through the cadmium electrode as through silver electrode.
Solution :
$$\eqalign{
& Cd\left( s \right) + 2A{g^ + }\left( {aq} \right) \to C{d^{2 + }}\left( {aq} \right) + Ag\left( s \right), \cr
& {E_{cell}} = E_{cell}^ \circ - \frac{{0.059}}{2}{\text{log}}\frac{{\left[ {C{d^{2 + }}} \right]}}{{{{\left[ {A{g^ + }} \right]}^2}}} \cr} $$