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24 January, 12:50

According to the following thermochemical equation, what mass of H2O (in g) must form in order to produce 488 kJ of energy?

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  1. 24 January, 14:00
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    m = 95.47 g

    Explanation:

    The reaction is missing. I found it, and here's the missing part:

    SiO2 (s) + 4HF (s) - > SiF4 (s) + 2H2O (l) ΔH°rxn = - 184 kJ

    According to the reaction, 2 moles of water are produced in this reaction, and this also produces 488 kJ of energy.

    To calculate the mass of any compound we use the expression:

    m = n*MM

    The molar mass of water is 18 g/mol. so, we need the moles of water to get the mass. The relation between the heat and energy is the following:

    ΔH = Q/n - --> solving for n:

    n = Q/ΔH.

    So, let's calculate moles of water used here:

    n = 488 * 2/184

    n = 5.304 moles

    Now we can calculate the mass:

    m = 5.304 * 18

    m = 95.47 g
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