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23 February, 01:52

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?

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  1. 23 February, 05:18
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    9842kJ of energy are released

    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
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