Final answer:
To calculate the volume of SO2 produced at STP from the reaction of 50.0 g of FeS, use stoichiometry. Convert the mass of FeS to moles, use the mole ratio to determine the moles of SO2 produced, and convert the moles of SO2 to volume in liters using the ideal gas law.
Step-by-step explanation:
To calculate the volume of SO2 produced at STP from the reaction of 50.0 g of FeS using the balanced equation, we need to use stoichiometry. First, we convert the mass of FeS to moles by dividing it by the molar mass of FeS. Then, we use the mole ratio from the balanced equation to determine the moles of SO2 produced. Finally, we convert the moles of SO2 to volume in liters using the ideal gas law.
Given:
- Mass of FeS = 50.0 g
- Balanced equation: 4 FeS + 7 O2 -> 2 Fe2O3 + 4 SO2
Step 1: Convert mass of FeS to moles
Moles of FeS = mass of FeS / molar mass of FeS
Step 2: Use mole ratio to determine moles of SO2 produced
Moles of SO2 = Moles of FeS * (4 moles of SO2 / 4 moles of FeS)
Step 3: Convert moles of SO2 to volume in liters
Volume of SO2 = Moles of SO2 * 22.4 L/mol (at STP)