Problem: An ice cube tray contains enough water at 22.0 ˚C to make 18 ice cubes that each has a mass of 30.0 g. The tray is placed in a freezer that uses CF2Cl2 as a refrigerant. The heat of vaporization of CF2Cl2 is 158 J/g. What mass of CF 2Cl2 must be vaporized in the refrigeration cycle to convert all the water at 22.0 ˚C to ice at -5.0 ˚C? The heat capacities for H2O (s) and H2O (l) are 2.03 J/g • ˚C and 4.18 J/g • ˚C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol.

FREE Expert Solution

+q absorbed by refrigerant  = -q released to freeze water 


qreleased=(mclT)1+(mcsT)2+(nΔHfreezing)mass water=18 ice cube×30.0 gice cube=540 g

qreleased=540 g×[4.18Jg°C(0°C-22.0°C)+2.03Jg°C(-5°C-0°C)]                         +(540 g H2O×1 mol H2O18.0 g H2O×-6.02 kJmol)

**ΔHfreezing = -ΔHfusion 

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Problem Details

An ice cube tray contains enough water at 22.0 ˚C to make 18 ice cubes that each has a mass of 30.0 g. The tray is placed in a freezer that uses CF2Cl2 as a refrigerant. The heat of vaporization of CF2Cl2 is 158 J/g. What mass of CF 2Cl2 must be vaporized in the refrigeration cycle to convert all the water at 22.0 ˚C to ice at -5.0 ˚C? The heat capacities for H2O (s) and H2O (l) are 2.03 J/g • ˚C and 4.18 J/g • ˚C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol.