The mercury cell is still sometimes used in industry to prepare chlorine, Cl2, and caustic soda, NaOH.
(a)In the first stage of the process a solution of sodium chloride is electrolysed using a voltage of 4.00V. Chlorine gas is obtained at one of the electrodes. The other electrode is made of mercury. Sodium metal forms at this electrode in a liquid alloy, called sodium amalgram. In your answers below it is not necessary to include the mercury in any equations.
(i)Half equation for the reaction that takes place at the positive electrode?
(ii)Half eqn at the negative electrode?
(iii)Explain why a voltage of 4.00V is needed, using relevant values of electrode potentials
(iv)What volume of chlorine is it possible to obtain from this electrolysis when a steady current of 10kA is passed for an hour?
Given;1 Faraday=9.65x10^4
Molar gas volume under these conditions=24.0dm3
I can do (i),(ii) and (iii) and part of (iv). I found the moles of chlorine gas but can't figure out the next step. I thought I might have to use PV=nRT.
Thanks for any help!