Question

When an aqueous solution of $AgN{O}_3$ is electrolysed between platinum electrodes, the substances liberated at anode and cathode are

• A. silver is deposited at cathode and $O_2$ is liberated at anode
• B. silver is deposited at cathode and $H_2$ is liberated | at anode
• C. hydrogen is liberated at cathode and $O_2$ is liberated at anode
• D. silver is deposited at cathode and $Pt$ is dissolved in electrolyte

Answer 1

Answer: (A)

At cathode : $A{g}_{\left(aq\right)}^{+}+e^{-}\to A{g}_{\left(s\right)}$
At anode : $2O{H}_{\left(aq\right)}^{-}\to \frac{1}{2}{O}_{2\left(g\right)}+H_2{O}_{\left(l\right)}+2e^{-}$