Question

The reaction taking place in the cell $Pt|\underset{1atm}{H_2\left(g\right)}|HCl\left(1.0M\right)|AgCl|Ag$ is:

• A. $AgCl+\left(1/2\right)H_2\to Ag+H^{+}+C{l}^{-}$
• B. $Ag+H^{+}+C{l}^{-}\to AgCl+\left(1/2\right)H_2$
• C. $2A{g}^{+}+H_2\to 2Ag+2H^{+}$
• D. $2Ag+2H^{+}\to 2A{g}^{+}+H_2$

Answer 1

The correct option is A $AgCl+\left(1/2\right)H_2\to Ag+H^{+}+C{l}^{-}$

In the given cell, $H_2$ is getting oxidised to $H^{+}$ and $A{g}^{+}$ is reduced to $Ag$.

So, reaction taking place is $AgCl+\frac{1}{2}{H}_2\to Ag+H^{+}+C{l}^{-}$