Using whole number coefficients, how do we (a.) represent the oxidation of potassium metal by water; and (b.) represent the oxidation ammonia to give #NO_2#?

1 Answer
anor277
Apr 24, 2017

Well, I would balance #a.# to give........

#K(s) + H_2O(l) rarr KOH(aq) + 1/2H_2(g)uarr#

Explanation:

But you wanted whole number coefficients, so we double the creature to give..........

#2K(s) + 2H_2O(l) rarr 2KOH(aq) + H_2(g)uarr#

And for the oxidation of ammonia #(b)#:

#NH_3(g) + O_2(g) rarr NO_2(g) + 3/2H_2(g)#, and double again to gives................:

#2NH_3(g) + 2O_2(g) rarr 2NO_2(g) + 3H_2(g)#.

Both equation are balanced with respect to mass and charge. Sometimes I find the half-integral coefficients useful in that it is easier to assess stoichiometry this way.

Are these redox reactions? Why or why not?

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