A) \[Pt({{H}_{2}})|{{H}^{+}}(aq)\]
B) \[Pt|Quinhydrone|{{H}^{+}}(aq)\]
C) \[Ag|A{{g}^{+}}(aq)\]
D) \[Ag,\,\,AgCl|C{{l}^{-}}(aq)\]
Correct Answer: D
Solution :
(a) \[\frac{1}{2}{{H}_{2}}(g)\xrightarrow{{}}{{H}^{+}}(aq)+{{e}^{-}}\] \[{{E}_{cell}}=E_{cell}^{o}-0.0591\log [{{H}^{+}}]\] (b) \[{{E}_{cell}}=E_{cell}^{o}-0.0591\log {{[{{H}^{+}}]}^{2}}\] (c)\[Ag(s)\xrightarrow{{}}A{{g}^{+}}(aq)\] \[{{E}_{cell}}=E_{cell}^{o}-0.0591\log [A{{g}^{+}}]\] (d)\[Ag(s)+C{{l}^{-}}(aq)\xrightarrow{{}}AgCl(s)+{{e}^{-}}\] \[{{E}_{cell}}=E_{cell}^{o}-0.0591\,\,\log \frac{1}{[C{{l}^{-}}]}\] Thus, in case (d), the\[{{E}_{cell}}\]increases with increase in the concentration of cell.You need to login to perform this action.
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