Problem: Assume 12,500 J of energy is added to 2.0 moles of solid H2O (ice) at 0.0°C. The molar heat of fusion is 6.02 kJ/mole. The specific heat of water is 4.184 J/mol K. The molar heat of vaporization is 40.6 kJ/mole. The resulting sample contains which of the following?(a) Only ice(b) Ice and water(c) Only water(d) Water and water vapor(e) Only water vapor

FREE Expert Solution

Account the energy needed to convert the 2 moles of solid H2O to liquid and eventually gas if enough energy is supplied given that 12,500 J of energy is added.

Recall that heat of fusion is the required heat to totally convert solid H2to liquid H2

In this case, we have the molar heat of fusion of water as 6.02 kJ/mole.

Calculating the energy needed to convert 2 moles of ice to liquid:

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Problem Details

Assume 12,500 J of energy is added to 2.0 moles of solid H2O (ice) at 0.0°C. The molar heat of fusion is 6.02 kJ/mole. The specific heat of water is 4.184 J/mol K. The molar heat of vaporization is 40.6 kJ/mole. The resulting sample contains which of the following?

(a) Only ice

(b) Ice and water

(c) Only water

(d) Water and water vapor

(e) Only water vapor