**Specific Heat, J/g.°C**

**2.06 - ice**

**4.18 - water**

**2.03 - steam**

**Molar heat of fusion for water, kJ/mol - 6.02**

**Molar hear of vaporization for water, kJ/mol - 40.6**

**Use the information given above, calculate the energy involved in the conversion of 235 g of steam at 373 K to ice at 243 K. Be sure to use the correct sign and answer in kJ.**

**Concepts and reason**

Specific heat is the energy required to raise the temperature of 1 g of a substance by.

To calculate the energy released to change the temperature, use the formula,

**Answer:**

**Explanation:**

Mass of the steam is given as 235 g. The specific heat for steam is . These values are substituted and heat released is calculated.

Take the temperature in **C** units. To convert the temperature from K to **C** , subtract 273 from it.

First, calculate the moles of steam as follows;

During the phase change, the change in temperature is zero. In this case, use the following formula to calculate the heat required:

**Explanation:**

Here, the phase changes from steam to liquid. Hence, here molar heat of vaporization should be used.

**Explanation:**

Here, the temperature of water changes. Hence, the specific heat of water should be substituted for c.

**Explanation:**

Here, the phase changes from water to ice. Hence, the heat of fusion should be used here.

Here, heat is released during the process. Hence, the heat energy released is .

**Explanation:**

The energy is released during the process of conversion of steam at 373 K to ice at 243 K. Hence, the sign of the energy involved in the process is negative.