# Question #483cf

##### 1 Answer

91804 J

#### Explanation:

This problem requires you to calculate two heats in order to solve it completely: the heat required to raise the temperature of the ice to its melting point of

First, we'll work on raising the temperature to

Where:

The heat capacity of water is

Next, we need to find the heat needed to actually melt the ice. To do this, we'll need to multiply the grams of ice we have by the **enthalpy of fusion of ice** , or the amount of energy you need to melt ice. You may have slightly different values for this based on units and rounding used by your specific book, but the one I will use is the one I got from Wikipedia, which is

Now, we just multiply the two

Now all we need to do is add the two heats procured:

Note that this is a positive value. This tells you that you are putting thermal energy into the system, which means that the process of melting ice is endothermic, as we would have expected.

Hope that helped :)