# CHem Part 2

Part of the SO2 that is introduced into the atmosphere by combustion of sulfur containing compounds ends up beingh converted to sulfuric acid.

2SO2 (g) + O2 (g) ---> 2H2SO4 (aq)

How much sulfuric acid can be formed from 5 moles of SO2, 2 moles of O2 and an unlimited quantity of water?

First, look at my first post in which I thought your equation was not right; however, your equation will give the correct answer, anyway. Did you make this up or was it in the original problem? Using your equation,
Since 2 mols SO2 yield 2 mols H2SO4; then 5 mols SO2 will yield 5 mols H2SO4.

1 mol O2 yields 2 mols H2SO4; therefore, 2 mols O2 yield 4 mols H2SO4.
Thus, O2 is the limiting reagent and the number of mols H2SO4 formed will be that produced by 2 mols O2 (which is 4 mols H2SO4). You may convert that to grams if you wish by 4 mols H2SO4 x molar mass H2SO4 = ?? g H2SO4.

Ok...got that part

what about the unlimited quantity of water part?

That just means you have all you need; therefore, it can't be a limiting reagent. And the problem doesn't ask for how much water is used.

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