chemistry

(You may have seen this before) A crude oil burned in electrical generating plants contains about 1.2% sulfur by mass. When the oil burns, the sulfur forms sulfur dioxide gas:

S(s) + O2(g) -------> SO2(g)

How many liters of SO2 (d = 2.60 g/L) are produced when 1.00 x 104 kg of oil burns at the same temperature and pressure?

Is my work correct?
1.00 x 10^4 kg of oil * 1.2% = 1.2 x 10^2 kg of sulfur
1.2 x 10^5 g of sulfur * (1 mol/32 g) = 3.75 * 10^3 mol S
3.75 * 10^3 mol S * (1 mol SO2/ 1 mol S) = 3.75 * 10^3 mol SO2
3.75 * 10^3 mol SO2 * (64 g / 1 mol SO2) = 2.4 * 10^5 SO2
2.4 * 10^5 g SO2 / (2.60 g/L) =
9.23 * 10^4 L SO2

seems awefully large, but i don't think i did anything wrong

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  1. It looks ok to me and I agree it sounds large but I don't see anything wrong.

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