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Home  >>  JEEMAIN and AIPMT  >>  Chemistry  >>  Redox Reactions
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In hydrogen gas electrode on increasing $[H^+]$ concentration,then (at $P_{H_2}=1atm)$

$\begin{array}{1 1}(a)\;E_{H^+/H_2}\;decreases&(b)\;E_{H^+/H_2}\;increases\\(c)\;E_{H^+/H_2}\;constant&(d)\;None\end{array}$

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By Nernst equation
$E_{H^+/H_2}=E^o_{H^+/H_2}-\large\frac{0.0591}{1}$$\log\large\frac{ \sqrt{P_{H_2}}}{[H^+]}$
Since cell reaction is
$H^+e^-\rightarrow \large\frac{1}{2}$$H_2(g)$
Standard hydrogen electrode as reference electrode
$E_{H^+/H_2}=-0.059\log \large\frac{1}{[H^+]}$
$E_{H^+/H_2}=-0.059\times P_H$
If we increase $[H^+]$ then $P_H$ increases to $E_{H^+/H_2}$ increases
Hence (b) is the correct answer.
answered Dec 11, 2013 by sreemathi.v

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