Question

Electrolysis of an aqueous solution of _______ process hydrogen at cathode, chlorine at anode and sodium hydroxide in the solution

Answer 1

Answer:

The reaction at the cathode is:

The reaction at the cathode is:[latex]{H}_{2}O (l) + 2 {e}^{- } \rightarrow {H}_{2}(g) + 2{ OH}^{- }[/latex]

The reaction at the cathode is:[latex]{H}_{2}O (l) + 2 {e}^{- } \rightarrow {H}_{2}(g) + 2{ OH}^{- }[/latex]The reaction at the anode is:

The reaction at the cathode is:[latex]{H}_{2}O (l) + 2 {e}^{- } \rightarrow {H}_{2}(g) + 2{ OH}^{- }[/latex]The reaction at the anode is:[latex]{Cl}^{- } \rightarrow \frac{1}{2} {Cl}_{2}(g) +1e^-[/latex]

The reaction at the cathode is:[latex]{H}_{2}O (l) + 2 {e}^{- } \rightarrow {H}_{2}(g) + 2{ OH}^{- }[/latex]The reaction at the anode is:[latex]{Cl}^{- } \rightarrow \frac{1}{2} {Cl}_{2}(g) +1e^-[/latex]The overall reaction is as follows:

The reaction at the cathode is:[latex]{H}_{2}O (l) + 2 {e}^{- } \rightarrow {H}_{2}(g) + 2{ OH}^{- }[/latex]The reaction at the anode is:[latex]{Cl}^{- } \rightarrow \frac{1}{2} {Cl}_{2}(g) +1e^-[/latex]The overall reaction is as follows:[latex]NaCl(aq) + {H}_{2}O(l) \rightarrow {Na}^{+}(aq) + {OH}^{-}(aq) + {H}_{2}(g) + \frac{1}{2}{Cl}_{2}(g)[/latex]

The reaction at the cathode is:[latex]{H}_{2}O (l) + 2 {e}^{- } \rightarrow {H}_{2}(g) + 2{ OH}^{- }[/latex]The reaction at the anode is:[latex]{Cl}^{- } \rightarrow \frac{1}{2} {Cl}_{2}(g) +1e^-[/latex]The overall reaction is as follows:[latex]NaCl(aq) + {H}_{2}O(l) \rightarrow {Na}^{+}(aq) + {OH}^{-}(aq) + {H}_{2}(g) + \frac{1}{2}{Cl}_{2}(g)[/latex]Reduction of Na+ (E° = –2.7 v) is energetically more difficult than the reduction of water (–1.23 v), so in aqueous solution, the latter will prevail.