1. Write the balanced chemical equation:

2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

2. Calculate the molar mass of butane (C₄H₁₀):

Molar mass of C = 12.01 g/mol

Molar mass of H = 1.01 g/mol

Molar mass of C₄H₁₀ = (4 * 12.01) + (10 * 1.01) = 58.12 g/mol

3. Convert grams of butane to moles:

Moles of C₄H₁₀ = (58 g) / (58.12 g/mol) = 1 mol

4. Use the mole ratio from the balanced equation:

The balanced equation shows that 2 moles of C₄H₁₀ produce 8 moles of CO₂. Therefore, the mole ratio is 2:8 or 1:4.

5. Calculate moles of CO₂ produced:

Moles of CO₂ = (1 mol C₄H₁₀) * (4 mol CO₂ / 1 mol C₄H₁₀) = 4 moles CO₂

Answer: 4 moles of CO₂ form when 58 grams of butane burn in oxygen.