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8 March, 14:10

4. A calorimeter contains 500 g of water at 25°C. You place a hand warmer containing 200 g of liquid sodium acetate inside the calorimeter. When the sodium acetate finishes crystallizing, the temperature of the water inside the calorimeter is 39.4°C. The specific heat of water is 4.18 J/g-°C. What is the enthalpy of fusion (Hf) of the sodium acetate? (Show your work.) Where necessary, use q = mHf.

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  1. 8 March, 15:41
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    First, we must calculate the energy released by the sodium acetate by assuming all the heat released is absorbed by the water. The heat absorbed by the water is given by:

    Q = mcΔT

    Q = 500 * 4.18 * (39.4 - 25)

    Q = 30,096 J = 30.096 kJ

    The enthalpy of fusion is expressed in kJ/mol, so we must first calculate the moles of sodium acetate using:

    moles = mass / Mr

    moles = 200 / 82.03

    moles = 2.44 mol

    ΔHf = - 30.096 / 2.44

    ΔHf = - 12.33 kJ/mol
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