turbongirl10
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PLEASE ANSWER FAST
If iron pyrite, FeS2, is not removed from coal, oxygen from the air will combine with both the iron and the sulfur as coal burns. If a furnace burns an amount of coal containing 198.20 g of FeS2, how much SO2 (an air pollutant) is produced?

4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2
Select one:
a. 211.7
b. 52.92
c. 590.8
d. 582.1

Respuesta :

cristisp93

First we need to calculate the number of moles of FeS[tex]_{2}[/tex]:

number of moles = mass (grams) / molecular mass (g/mol)

number of moles of FeS[tex]_{2}[/tex] = 198.2/120 = 1.65 moles

From the chemical reaction we deduce that:

if            4 moles of FeS[tex]_{2}[/tex] produces 8 moles of SO[tex]_{2}[/tex]

then  1.65 moles of FeS[tex]_{2}[/tex] produces X moles of SO[tex]_{2}[/tex]

X = (1.65×8)/4 = 3.3 moles of SO[tex]_{2}[/tex]

Now we can calculate the mass of SO[tex]_{2}[/tex]:

mass (grams) = number of moles × molecular mass (grams/mole)

mass of SO[tex]_{2}[/tex] = 3.3×64 = 211.2 g

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