What is the balanced equation of the oxidation-reduction between methyl alcohol and copper oxide?

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Answer 1 · 2018-03-05T05:52:12

We use the tedious method of half-equations......

#H_3COH(l) + CuO(s) rarr H_2C=O(aq)+H_2O(l)+Cu(s)#

...how did we get this....?

Copper oxide is reduced...#Cu^(2+)rarrCu^0#

#CuO(s) +2H^+ +2e^(-) rarr Cu + H_2O(l)# #(i)#

Methyl alcohol is oxidized...#C(-II)rarrC(0)#

#CH_3OH rarr H_2C=O(aq) +2H^+ +2e^(-)# #(ii)#

And we simply take #(i)+(ii)# to eliminate the electrons..

#H_3COH(l) + CuO(s) rarr H_2C=O(aq)+Cu(s)+H_2O(l)#

Is this balanced with respect to mass and charge? If it is not, then it cannot be accepted as a model of chemical reactivity.