Final answer:
Using a balanced chemical equation and a mole-mass calculation sequence, 862 grams of SO3 can react with 3.59 moles of Fe2O3. The molar ratio and molar mass of SO3 are used to make the conversion.
Step-by-step explanation:
To determine how many grams of SO3 can react with 3.3 moles of Fe(NO3)3, we will use the balanced chemical equation Fe2O3 +3SO3 → Fe2(SO4)3 and a two-step mole-mass calculation sequence. First, we will set up a molar ratio to calculate the number of moles of SO3 required for the reaction, using the given quantity of Fe2O3.
Given 3.59 moles of Fe2O3, according to the balanced equation, we need 3 moles of SO3 for every mole of Fe2O3. Therefore, we multiply:
3.59 mol Fe2O3 × (3 mol SO3 / 1 mol Fe2O3) = 10.77 mol SO3
Next, using the molar mass of SO3, which is 80.065 g/mol, we convert the moles of SO3 to grams:
10.77 mol SO3 × 80.065 g/mol = 862.34055 g SO3
Hence, 862 g of SO3, expressed to three significant figures, will react with 3.59 mol of Fe2O3. This exemplifies how such problems can generally be resolved using a mole-mass calculation sequence.