# chemistry

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 1.00X 10 to the 4th kg of oil burns at the same temperature and pressure?

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1. Multiply 1.00*10^4 kg by 0.012 to get the mass of sulfur burned. Convert ot to grams by multiplying by 1000.
M(S) = 1.20*10^5 g

The mass of SO2 formed is twice the mass of the S burned, because one S atom and two O atoms both weigh the same.

Divide the mass of SO2 formed by 2.60 g/L to get the number of liters of SO2 formed.

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2. Step 1. Write the balanced equation. You have that.

Step 2. Convert 1.00 x 10^4 kg oil to grams S (it's 1.2% S by mass).

Step 3. Convert g S to mols S.

Step 4. Using the coefficient in the balanced equation, convert mols S to mols SO2.

Step 5. Convert mols SO2 to grams SO2 from mols SO2 x molar mass SO2 = g SO2.

Step 6. Using the density, convert g SO2 to liters SO2. (There is no pressure or temperature listed in the problem; therefore, I assume the problem intends for you to calculate liters SO2 at the temperature and pressure for which the density is given.).

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3. .092L

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4. 46,153.84615

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