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13 Dec 2019

The enthalpy of vaporization of water at 100 degrees celsius and 1 atm is 40.631 kj/mol, and the enthalpy of fusion of ice at 0 degrees celsius and 1 atm is 333.6 J/g. What is the deltaH for 225g steam at 100 degrees celsius condensing to a liquid at 100 degrees celsius? If all of this heat could be transferred to ice at 0 degrees celsius, what mass of ice would melt?

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Patrina Schowalter
Patrina SchowalterLv2
17 Dec 2019

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Related questions

Using the values for the heat of fusion, specific heat of water, and or heat vaporization, calculate the amount of heat energy in each of the following: a) joules to condense 125 g of steam at 100 degrees celsius and to cool the liquid to 15.0 degrees celsius; b) joules needed to melt a 525-g ice sculpture at 0 degrees celsius and to warm the liquid to 15.0 degrees celsius; c) kilojoules released when 85.0 g of steam condenses at 100 degrees C, cool the liquid, and freeze it at 0 degrees C; d) joules to warm 55.0 mL of water (density=1.00 g/mL) from 10.0 degrees C and vaporize it at 100 degrees C.

Using the values for the heat of fusion, specific heat of water, and or heat vaporization, calculate the amount of heat energy in each of the following: a) joules to condense 125 g of steam at 100 degrees celsius and to cool the liquid to 15.0 degrees celsius; b) joules needed to melt a 525-g ice sculpture at 0 degrees celsius and to warm the liquid to 15.0 degrees celsius; c) kilojoules released when 85.0 g of steam condenses at 100 degrees C, cool the liquid, and freeze it at 0 degrees C; d) joules to warm 55.0 mL of water (density=1.00 g/mL) from 10.0 degrees C and vaporize it at 100 degrees C.

How much heat is absorbed when 1.0 g of ice at -5.0 degrees Celsius is heated to water at 10 degrees Celsius?

The molar heat capacity of ice is 36.57 J/mol K, the molar heat capacity of water is 75.4 J/mol K, and the molar heat capacity of steam is 33.67 J/mol K. The enthalpy of fusion is 6.01 kJ/mol, and the enthalpy of vaporization is 40.67 kJ/mol.

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