How much heat is transferred when 7.19 grams of H2 reacts with excess nitrogen, according to the following equation: N2(g) + 3 H2 (g) –>

Question

How much heat is transferred when 7.19 grams of H2 reacts with excess nitrogen, according to the following equation: N2(g) + 3 H2 (g) –> 2 NH3 (g) \DeltaΔH = +46.2 kJ

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Tryphena 4 years 2021-09-03T12:04:53+00:00 1 Answers 11 views 0

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  1. Gerda
    0
    2021-09-03T12:06:29+00:00
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    Answer:

    Q=54.8kJ

    Explanation:

    Hello there!

    In this case, according to the given chemical reaction, it is possible for us to realize that the 46.2 kJ of energy are given per mole of reaction, which are related to 3 moles of hydrogen; Thus, we can calculate the energy per mole of hydrogen as shown below:

    \Delta H=\frac{46.2kJ}{mol} *\frac{1mol}{3molH_2}\\\\ \Delta H=15.4\frac{kJ}{molH_2}

    Now, to calculate the total energy, we convert the grams to moles of hydrogen as shown below:

    Q=7.19gH_2*\frac{1molH_2}{2.02gmolH_2}*15.4\frac{kJ}{molH_2} \\\\Q=54.8kJ

    Best regards!

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