How much energy does it take to melt a 16.87 g ice cube? ΔHfus = 6.02 kJ/mol How much energy does it take to melt a 16.87 g ice cube? = 6.02

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How much energy does it take to melt a 16.87 g ice cube? ΔHfus = 6.02 kJ/mol How much energy does it take to melt a 16.87 g ice cube? = 6.02 kJ/mol 108 kJ 102 kJ 5.64 kJ 936 J none of the above

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Thiên Di 4 years 2021-09-02T19:30:41+00:00 1 Answers 192 views 0

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  1. thuhuong
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    2021-09-02T19:32:22+00:00
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    Answer:

    How much energy does it take to melt a 16.87 g ice cube? ΔHfus = 6.02 kJ/mol How much energy does it take to melt a 16.87 g ice cube? = 6.02 kJ/mol

    A. 108 kJ

    B. 102 kJ

    C. 5.64 kJ

    D. 936 kJ

    E. none of the above

    5.64 kJ

    Explanation:

    The Heat of fusion is the heat energy required to dissolve a given mass of ice at melting point.

    Step by Step Calculation

    The heat energy required to dissolve ice can be calculated using the expression below;

    Q = ΔH_{f} x m ………………………………………..1

    where Q is the heat energy required;

               ΔH_{f}  is the heat of fusion for ice;

               m is the mole

    All the parameters above are provided in the question except m, so to get m we use the molar mass of water (also for ice) which is 18.01528 g/mol
    .

    This means that 18.01528 g of ice is contained in one mole, therefore the mole for 16.87 g of ice is given as;

    m = \frac{16.87g}{18.015g/mol}

    m = 0.9364 mole of ices

    Now the parameters are complete, we are given;

    ΔH_{f}  = 6.02 kJ/mol

    m = 0.9364 mol

    Q =?

    Substituting into equation 1, we have

    Q =  6.02 kJ/mol x 0.9364 mol

    Q = 5.64 kJ

    Therefore, the energy required to melt 16.87 g of ice is 5.64 kJ

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