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15 June, 11:11

How much heat is absorbed/released when 20.00 g of NH3 (g) (17.0307g/mol) react in the presence of excess O2 (g) to produce NO (g) and H2O (l) according to the following chemical equation? 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (l) ΔH° = 1168 kJ

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  1. 15 June, 12:05
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    342.8 kJ are absorbed

    Explanation:

    In the reaction:

    4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (l) ΔH° = 1168 kJ

    As ΔH > 0, the heat is absorbed. Also, when 4 moles of NH3 are involved in the reaction, there are absorbed 1168 kJ.

    Having this in mind, moles of NH3 in 20.00g are:

    20.00g * (1mol / 17.0307g) = 1.174 moles

    Thus, 1.174 moles of NH3 absorbed:

    1.174 moles * (1168 kJ / 4 moles) = 342.8 kJ are absorbed.
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