| (i) \[C{{d}^{2+}}\left( aq \right)+2{{e}^{-}}\xrightarrow{{}}Cd\left( s \right),E{}^\circ =-0.40V\] |
| (ii) \[A{{g}^{+}}(aq)+{{e}^{-}}\xrightarrow{{}}Ag(s),E{}^\circ =0.80V\] |
| 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.
Correct Answer: C
Solution :
[c] \[Cd(s)+2A{{g}^{+}}\left( aq \right)\xrightarrow{{}}C{{d}^{2+}}(aq)+Ag(s),\] \[{{E}_{cell}}=E_{cell}^{{}^\circ }-\frac{0.059}{2}\log \frac{[C{{d}^{2+}}]}{{{[A{{g}^{+}}]}^{2}}}\]
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