Question

Use the reaction: 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) + 5720 kJ. In the reaction, 200.0g of hydrocarbon react with excess oxygen gas. How much energy is released?

Answer 1

9842kJ of energy are released

Step-by-step explanation:

Based on the reaction:

2 C₄H₁₀ (g) + 13 O₂ (g) → 8 CO₂(g) + 10 H₂O (g) + 5720 kJ

When 2 moles of C₄H₁₀ react with 13 moles of O₂ there are released 5720 kJ of energy

As molar mass of C₄H₁₀ is 58.12g/mol, moles in 200.0g of the hydrocarbon are:

200.0g C₄H₁₀ ₓ (1mol / 58.12g) = 3.441 moles of C₄H₁₀

As 2 moles of C₄H₁₀ release 5720kJ of energy, 3.441 moles of C₄H₁₀ release:

3.441 moles C₄H₁₀ ₓ (5720kJ / 2 moles C₄H₁₀) = 9842kJ of energy are released