Respuesta :
a) The balanced chemical equation provided is \(4 \text{FeS}_2 + 11 \text{O}_2 = 2 \text{Fe}_2\text{O}_3 + 8 \text{SO}_2\).
The molar ratio between \(\text{FeS}_2\) and \(\text{SO}_2\) is \(4:8\) or \(1:2\). This means that for every 4 moles of \(\text{FeS}_2\) burned, 8 moles of \(\text{SO}_2\) are produced.
Given that 1.4 kg of pyrite ore is used, and it contains 12% impurities, the amount of pure \(\text{FeS}_2\) is \(0.88 \times 1.4 \, \text{kg}\).
Now, calculate the moles of \(\text{FeS}_2\) using its molar mass. The molar mass of \(\text{FeS}_2\) is the sum of the atomic masses of iron (Fe) and sulfur (S) multiplied by 2 (since there are two sulfur atoms in \(\text{FeS}_2\)).
Next, using the molar ratio from the balanced equation, determine the moles of \(\text{SO}_2\) produced.
Finally, convert the moles of \(\text{SO}_2\) to volume using the ideal gas law (\(PV = nRT\)), where \(P\) is the pressure, \(V\) is the volume, \(n\) is the number of moles, \(R\) is the gas constant, and \(T\) is the temperature.
b) First, determine the moles of \(\text{SO}_2\) needed using the stoichiometric coefficients from the balanced equation.
Next, use the molar ratio between \(\text{FeS}_2\) and \(\text{SO}_2\) (from the balanced equation) to find the moles of \(\text{FeS}_2\) needed.
Given that the raw material is 85% pyrite, calculate the mass of raw material needed by dividing the moles of pure \(\text{FeS}_2\) by the percentage purity of the raw material.
The molar ratio between \(\text{FeS}_2\) and \(\text{SO}_2\) is \(4:8\) or \(1:2\). This means that for every 4 moles of \(\text{FeS}_2\) burned, 8 moles of \(\text{SO}_2\) are produced.
Given that 1.4 kg of pyrite ore is used, and it contains 12% impurities, the amount of pure \(\text{FeS}_2\) is \(0.88 \times 1.4 \, \text{kg}\).
Now, calculate the moles of \(\text{FeS}_2\) using its molar mass. The molar mass of \(\text{FeS}_2\) is the sum of the atomic masses of iron (Fe) and sulfur (S) multiplied by 2 (since there are two sulfur atoms in \(\text{FeS}_2\)).
Next, using the molar ratio from the balanced equation, determine the moles of \(\text{SO}_2\) produced.
Finally, convert the moles of \(\text{SO}_2\) to volume using the ideal gas law (\(PV = nRT\)), where \(P\) is the pressure, \(V\) is the volume, \(n\) is the number of moles, \(R\) is the gas constant, and \(T\) is the temperature.
b) First, determine the moles of \(\text{SO}_2\) needed using the stoichiometric coefficients from the balanced equation.
Next, use the molar ratio between \(\text{FeS}_2\) and \(\text{SO}_2\) (from the balanced equation) to find the moles of \(\text{FeS}_2\) needed.
Given that the raw material is 85% pyrite, calculate the mass of raw material needed by dividing the moles of pure \(\text{FeS}_2\) by the percentage purity of the raw material.
