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You need 3 calculations.

1 - Heat removed to change a gas to liquid

2 - Heat removed to cool H2O from 100C to 0C

3 - Heat needed to change a liquid to a solid

1 - Heat of vaporization (or condensation) for water = 2260J/1g H2O

75.0g H2O x 2260J/1g H2O = 169,500J

2 - Change in temp = 100C

75.0g H2O x 100C x 4.184J/gC = 31,380J

3 - Heat of fusion for water = 334J/1g ice

75.0g H2O x 334J/1g ice = 25,050J

Add Joules together = 225,930J

Convert to kJ = 225,930J x 1kJ/1000J = 225.93kJ

Since 75.0 has 3 sig figs, the answer would be 226kJ

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12y ago
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Q: How many kilojoules are released when 75.0g of steam at 100 degrees C condenses cools to 0 degrees C and freezes at 0 degrees C?
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