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How do I balance this reaction using half-redox equations? $$\ce{2SO2 + O2->2SO3}$$
My work is:
Oxidation: $\ce{SO2 + H2O -> SO3 + 2e- + 2H+}$
Reduction: $\ce{H2O + 2e- + O2 -> SO3 + 2H+}$
Total: $\ce{SO2 + 2H2O + O2 -> 2SO3 + 4H+}$
BUT it's false. What did I do wrong?
WELL I think you put something erroneous in your reduction formula.
You will never get SO3 out of just O2 and water. Instead of SO3
The reduction formla will be 4e- + O2 + 4H+ --> 2 H2O
Multiply oxidation formula by 2 and add it to new reduction formula and you got your answer
