Problem: From the data below, calculate the total heat (in J) needed to convert 22.00 g of ice at −6.00°C to liquid water at 0.500°C: mp at 1 atm:     0.0°C                      Δ  H°fus:      6.02 kJ/molcliquid:               4.21 J/g•°C              csolid:        2.09 J/g•°C

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From the data below, calculate the total heat (in J) needed to convert 22.00 g of ice at −6.00°C to liquid water at 0.500°C: 

mp at 1 atm:     0.0°C                      Δ  H°fus:      6.02 kJ/mol
cliquid:               4.21 J/g•°C              csolid:        2.09 J/g•°C

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Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves. Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.