Ask Question
11 May, 10:56

When 0.455 g of anthracene, c14h10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63°c. assuming that the specific heat of water is 4.18 j / (g ∙ °c), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene?

+2
Answers (1)
  1. 11 May, 11:10
    0
    Answer is: enthalpy of combustion per mole of anthracene is - 7073.21 kJ/mol.

    Balanced chemical rreaction of anthracene combustion:

    C₁₄H₁₀ + 33/2O₂ → 14CO₂ + 5H₂O.

    m (C₁₄H₁₀) = 0.455 g; mass of anthracene.

    ΔT (H₂O) = 8.63°C.

    m (H₂O) = 500.0 g; mass of water.

    cp = 4.18 J/g·°C; specific heat of water.

    n (C₁₄H₁₀) = m (C₁₄H₁₀) : M (C₁₄H₁₀).

    n (C₁₄H₁₀) = 0.455 g : 178.23 g/mol.

    n (C₁₄H₁₀) = 0.00255 mol; amount of anthracene.

    Q = ΔT (H₂O) · m (H₂O) · cp.

    Q = 8.63°C · 500 g · 4.18 J/g·°C.

    Q = 18036.7 J : 1000 J/kJ.

    Q = 18.037 kJ; heat absorb by water.

    ΔH = Q : n (C₁₄H₁₀).

    ΔH = 18.037 kJ : 0.00255 mol.

    ΔH = 7073.21 kJ/mol.
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “When 0.455 g of anthracene, c14h10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers