Account the energy needed to convert the **2 moles of solid H _{2}O**

Recall that *heat of fusion* is the required heat to totally convert solid H_{2}O to liquid H_{2}O

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**:

Assume 12,500 J of energy is added to 2.0 moles of solid H_{2}O (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

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