how many grams SO2 are produced when 20(g) FeS2 reacts with 16(g) O2?
4FeS2(g)+15O2(g)=2Fe2O2(s)+8SO2(g)
I doubt the Fe2O2. More likely to be Fe2O3 or FeO. I would go with Fe2O3.
4FeS2 + 11O2 ==> 2Fe2O3 + 8SO2
Convert 20 g FeS2 to moles. moles = grams/molar mass
Using the coefficients in the balanced equation, convert moles FeS2 to moles SO2.
Convert moles SO2 to grams. g = moles x molar mass.
To determine the number of grams of SO2 produced when 20 grams of FeS2 reacts with 16 grams of O2, we need to use the stoichiometry of the balanced chemical equation provided.
First, let's calculate the moles of FeS2 and O2 using their respective molar masses. The molar mass of FeS2 (Iron Pyrite) is approximately 119.98 g/mol, and the molar mass of O2 is approximately 32 g/mol.
Moles of FeS2 = Mass of FeS2 / Molar mass of FeS2
Moles of FeS2 = 20 g / 119.98 g/mol ≈ 0.1667 mol
Moles of O2 = Mass of O2 / Molar mass of O2
Moles of O2 = 16 g / 32 g/mol = 0.5 mol
Next, we use the stoichiometry of the balanced chemical equation to determine the moles of SO2 produced. According to the equation, 4 moles of FeS2 react with 15 moles of O2 to produce 8 moles of SO2.
Using the mole ratio from the balanced chemical equation:
Moles of SO2 = (moles of O2 × 8 moles of SO2) / 15 moles of O2
Moles of SO2 = (0.5 mol × 8) / 15 ≈ 0.2667 mol
Finally, we can calculate the mass of SO2 produced using its molar mass, which is approximately 64.06 g/mol.
Mass of SO2 = Moles of SO2 × Molar mass of SO2
Mass of SO2 = 0.2667 mol × 64.06 g/mol ≈ 17.07 g
Therefore, approximately 17.07 grams of SO2 are produced when 20 grams of FeS2 reacts with 16 grams of O2.