Final answer:
To balance the equation, 3 molecules of hydrogen gas are produced. To find out how many grams of SO3 can react with 3.59 mol of Fe2O3, we use a two-step mole-mass calculation sequence, resulting in 862 g of SO3.
Step-by-step explanation:
The missing number to balance the given equation 2 Fe + 3H₂SO₄ → 1 Fe₂³(SO₄)3 + _ H₂ is 3. By balancing the hydrogen atoms, we can find that three molecules of hydrogen gas (H₂) are produced. Now, let’s address the main question which involves calculating how many grams of SO3 can react with 3.59 mol of Fe2O3 by using a mole-mass calculation sequence.
Following the balanced chemical equation Fe2O3 + 3SO3 → Fe2(SO4)3, we determine the appropriate molar ratio which is 3 mol SO3 to 1 mol Fe2O3. This sets up our conversion factor:
- 3.59 mol Fe2O3 × (3 mol SO3 / 1 mol Fe2O3) = 10.77 mol SO3
Next, using the molar mass of SO3, which is 80.07 g/mol, we calculate the mass:
- 10.77 mol SO3 × 80.07 g/mol = 862 g of SO3
The final answer, expressed with three significant figures, is 862 g of SO3 that will react with 3.59 mol of Fe2O3.