# Calculate the amount of heat (in kJ) that must be absorbed to convert 108 g of ice at #0^@"C"# to water at #70^@"C"#?

##### 1 Answer

You'd need **67.6 kJ** of heat to convert that much ice at

So, you need to go from ice at *solid*, to water at *liquid*. This implies that you will go through a phase change, i.e. from ice at

As a result, you're going to have to consider two heats, one needed for the phase change and the other needed to raise the temperature of water from

The heat needed for the phase change will be

Plug in your values to get

The heat needed to raise the temperature of the water will be

Plug in your values to get

The *total heat* needed will be

I'll leave the answer rounded to three sig figs and expressed in kJ, so you'll get