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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22-05-2017
Chemistry

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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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scme1702 scme1702 · Answer 1 · 2017-05-29T13:39:29+02:00

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