1. The problem statement, all variables and given/known data
Sulfur dioxide reacts with the oxygen in humid air to produce sulfur trioxide.
After the reaction, how many moles are left of: SO_{2}, O_{2} and how many moles of SO_{3} were created?
2. Relevant equations
2 SO_{2} + O_{2} > 2 SO_{3}
3. The attempt at a solution
The limiting reactant is SO_{2}, so we know that it will fully react and we'll end up with 0 moles of SO_{2}.
From previous steps, I know that I have 0.1021 moles of SO_{2}, and 0.0857 moles of O_{2}. I also know that after the reaction, I will have 0.03474 moles of O_{2} left.
I can't, for the life of me, figure out how many moles of SO_{3} I'll have at the end.
Shouldn't there be some conservation of mass? I keep finding that I'll have 0.1021 moles of SO_{3} at the end, which is the same amount as the SO_{2}.
Is this correct? I seem to think that the reaction with O_{2} will have changed the number of moles.
