How do you balance #Cl_2(g) + H_2O(l) rarr HClO(g) + HCl(aq)#?

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Answer 1 · 2016-11-04T17:33:45

Is this not already balanced?:

#Cl_2(g) + H_2O(l) rarr HClO(aq) + HCl(aq)#

This is a disproportionation reaction, in which chlorine gas is oxidized and reduced:

#1/2Cl_2(g) +H_2O(l) rarr ClO^(-) +2H^+ +e^- # #i.#

#1/2Cl_2(g) +e^(-) rarr Cl^(-)# #ii.#

Overall #i.+ii.=#:

#Cl_2(g) +H_2O(l) rarr ClO^(-)+Cl^(-) +2H^+#

OR

#Cl_2(g) +H_2O(l) rarr ClOH(aq)+HCl(aq)#