Question

Suppose 650 mL of hydrogen gas are produced through a displacement reaction involving solid iron and sulfuric acid, H2SO4, at STP. How many grams of iron (II) sulfate are produced? Density H2(g) is on your periodic table.

Answer 1

4.415 g of FeSO₄

Step-by-step explanation:

The balance chemical equation for given single replacement reaction is as follow;

Fe + H₂SO₄ → FeSO₄ + H₂

Data Given;

Volume = 650 mL = 0.65 L

Density at STP = 0.08988 g/L

Mass = Density × Volume = 0.08988 g/L × 0.65 L = 0.0584 g

Step 1: Calculate Moles of H₂ as;

Moles = Mass / M.Mass

Moles = 0.0584 g / 2.01 g/mol

Moles = 0.0290 mol of H₂

Step 2: Find out moles of FeSO₄ as;

According to balance chemical equation,

1 mole of H₂ is produced along with = 1 mole of FeSO₄

So,

0.0290 moles of H₂ will be produced along with = X moles of FeSO₄

Solving for X,

X = 0.0290 × 1 mol / 1 mol

X = 0.0290 moles of FeSO₄

Step 3: Calculate mass of FeSO₄ as;

Mass = Moles × M.Mass

Mass = 0.0290 mol × 151.90 g/mol

Mass = 4.415 g of FeSO₄