A aqueous solution of is prepared and exactly of this solution is fully electrolysed using inert ele — Electrochemistry Chemistry Question

💡 Solution & Explanation

Molarity = $4.0\text{ M}$. Volume = $0.5\text{ L}$. Moles of $NaCl = 4.0 \times 0.5 = 2.0$ moles. Therefore, there are $2.0$ moles of $Cl^-$ ions available in the solution. The anodic reaction is $2Cl^- \rightarrow Cl_2 + 2e^-$. Thus, 2 moles of $Cl^-$ ions will produce exactly 1.0 mole of $Cl_2$ gas.