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10 October, 10:37

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O DH = - 890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

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  1. 10 October, 10:58
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    94.56KJ

    Explanation:

    1.7 grams of CH4 contains 1.7/16 moles of CH4.

    If 1 mole of CH4 give 890KJ

    1.7/16 moles of CH4 gives 1.7/16*890 = 94.56KJ
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