Starting with sodium chloride,how would you proceed to prepare:
$(i)$ sodium metal
$(ii)$ sodium hydroxide
$(iii)$ sodium peroxide
$(iv)$ sodium carbonate?

(N/A) $(i)$ Sodium metal: Sodium is extracted from fused $NaCl$ by the Downs process. The electrolyte is a mixture of $NaCl$ $(40 \%)$ and $CaCl_2$ $(60 \%)$ at $1123 \ K$. Steel is the cathode and graphite is the anode. $Na^{+} + e^- \rightarrow Na$ (at cathode); $2Cl^- \rightarrow Cl_2 + 2e^-$ (at anode).
$(ii)$ Sodium hydroxide: It is prepared by the electrolysis of an aqueous solution of $NaCl$ (brine) in a Castner-Kellner cell. $2NaCl + 2H_2O \rightarrow 2NaOH + Cl_2 + H_2$.
$(iii)$ Sodium peroxide: Sodium metal obtained from the Downs process is heated on aluminium trays in an atmosphere of $CO_2$-free air to form sodium peroxide. $2Na + O_2 \rightarrow Na_2O_2$.
$(iv)$ Sodium carbonate: It is prepared by the Solvay process. $2NH_3 + H_2O + CO_2 \rightarrow (NH_4)_2CO_3$; $(NH_4)_2CO_3 + H_2O + CO_2 \rightarrow 2NH_4HCO_3$; $NH_4HCO_3 + NaCl \rightarrow NH_4Cl + NaHCO_3$; $2NaHCO_3 \rightarrow Na_2CO_3 + H_2O + CO_2$.