Chemistry

The amount of energy released by the combustiom of 100 g of C2H2 (g) is ______ MJ.

2CH2 + 5O2 ----> 4CO2(g) + 2H2O(g) ΔH= -2511.0 kJ

Do I use ΔH = Hproducts - Hreactants? And if so how would that help me solve for the energy released?

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  1. I'm assuming the CH2 should be C2H2 (Acetylene) ...

    From the balanced equation, two moles of acetylene => -2511Kj = 2.511Mj

    Convert 100g C2H2 to moles 100g/26g/mol = 3.85 moles

    Set ratio ...
    (2/3.85 = 2.511/x => x = [(2)(2.511)]/(3.85)Mj = 1.30Mj

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  2. No and yes.
    You don't need to use dHrxn = (n*dHf products) - (n*dHf reactants) because the problems has already done that for you. For the reaction given dH is -2511.0 kJ and that is for 2 mols of C2H2 or 2*26 = 52 g.
    So the revised question is if 52 g releases 2511.0 kJ how much will 100 g release? Can you take it from there?

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