When 1 mol of methane is burned at constant pressure, −890 kJ/mol of energy is released as heat. If a 1.67 g sample of methane is burned at

Question

When 1 mol of methane is burned at constant pressure, −890 kJ/mol of energy is released as heat. If a 1.67 g sample of methane is burned at constant pressure, what will be the value of ∆H

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Ngọc Hoa 5 years 2021-07-30T20:34:29+00:00 1 Answers 168 views 1

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  1. kimchi2
    0
    2021-07-30T20:35:46+00:00
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    Answer:

    \Delta H=-92.7kJ

    Explanation:

    Hello there!

    In this case, according to the given information, we can infer that 890 kJ of energy are released when 1 mole of methane is burned; however, to find the total heat when 1.67 grams are burned, we first need to calculate the moles in this mass of methane:

    1.67gCH_4*\frac{1molCH_4}{16.04gCH_4}=0.104molCH_4

    And thus, for calculating the resulting ∆H, we proceed as follows:

    \Delta H=-890kJ/mol*0.104mol\\\\\Delta H=-92.7kJ

    Regards!

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