1.0 L of 0.1 M aqueous solution of KCl  is electrolysed. A current of 96.50 mA is passed through the solution for 10 hours. Which is / are correct ? (Assume volume of solution remains constant during electrolysis)

i = 96.50 mA, $t=10\times 60\times 60s$

 Solution is 1.0 L and 0.1 M

Moles present $=1\times 0.1=0.1$ moles

Reactions :

         $2H^{+}+2e\to H_2:2C{l}^{-}\to C{l}_2+2e^{-}$

         $\frac{w}{M}=\frac{it}{nF}=\frac{w}{M}=\frac{96.50\times 10\times 60\times 60\times {10}^{-3}}{2\times 96500}=0.018$

         For $C{l}^{-}=0.036$; Molarity = 0.1 -0.036 = 0.064

         $V_{C{l}_2}=\frac{0.018\times 22.4}{2}=0.202Lor202ml$

            K⁺ will not discharge