Chemistry help please? :)

I'm like super stuck on this question, help will be appreciated. 10 points to first correct answer :)

Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid.
• Write a balanced equation for the reaction.
• Calculate the theoretical yield of sulfuric acid.
• Calculate the percent yield of the reaction.
(One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

Thank youuu!!

The actual mechanism for the reaction is rather complicated; it's actually three processes:

2 SO2 + O2 → 2 SO3
SO3 + H2O → H2SO4(g)
H2SO4(g) → H2SO4(l)

so the overall reaction is

2SO2 + O2 + 2H2O → 2H2SO4

To get the theoretical yield, figure out the moles of SO2 that you have started with, and then convert moles of the product (sulfuric acid) to grams or kilograms. It's moles to moles since there's a "2" in front of both SO2 and H2SO4, right?

The percent yield is then just 250 gm over the theoretical yield.

okay i can only do the balanced equation, which i think is:

SO2 + 1/2 O2 + H2O = H2SO4

never ever done percentage yield

1. 2SO2+O2+2H2O=2H2SO4
2. Dunno
3.dunno