2528.82 grams of iron is needed to react completely with 5.65 moles of sulfur.
To find the mass of iron needed to react with 5.65 moles of sulfur (S8) in the given chemical equation:
8 Fe + S8 → 8 FeS
You can use the stoichiometry of the reaction to determine the mass of iron required.
Step 1: Write down the balanced chemical equation.
The balanced chemical equation shows the mole-to-mole ratio of reactants and products. In this case, 8 moles of iron react with 1 mole of sulfur (S8) to produce 8 moles of iron sulfide (FeS).
Step 2: Find the molar mass of sulfur (S8).
The molar mass of sulfur (S8) can be calculated by adding the molar masses of 8 sulfur atoms (S), as S8 is a molecule containing 8 sulfur atoms.
Molar mass of S8 = 8 × molar mass of S
The molar mass of sulfur (S) is approximately 32.06 g/mol (you can find this value on the periodic table).
Molar mass of S8 = 8 × 32.06 g/mol = 256.48 g/mol
Step 3: Calculate the moles of sulfur (S8) you have.
Given that you have 5.65 moles of sulfur (S8), you can use this value directly.
Step 4: Use the mole ratio to find moles of iron (Fe).
From the balanced equation, you know that 8 moles of iron react with 1 mole of sulfur (S8). So, you can set up a proportion to find the moles of iron:
(8 moles Fe / 1 mole S8) = (X moles Fe / 5.65 moles S8)
Solving for X:
X = (8 moles Fe / 1 mole S8) × (5.65 moles S8) = 45.2 moles Fe
Step 5: Calculate the mass of iron (Fe) required.
Now that you know you need 45.2 moles of iron to react with 5.65 moles of sulfur, you can find the mass of iron using its molar mass.
The molar mass of iron (Fe) is approximately 55.85 g/mol.
Mass of Fe = moles of Fe × molar mass of Fe
Mass of Fe = 45.2 moles × 55.85 g/mol ≈ 2528.82 g
So, you would need approximately 2528.82 grams of iron to react completely with 5.65 moles of sulfur (S8) in the given reaction.