16 grams of ice at –32°c is to be changed to steam at 182°c. the entire process requires cal. round your answer to the nearest whole number. the specific heat of both ice and steam is 0.5 cal/g°c. the specific heat of water is 1.00 cal/gk. the heat of fusion is 80 cal/g and the heat of vaporization is 540 cal/g.

12432 cal.

Explanation:

The process to change ice at -32 ºC to steam at 182 ºC can be divided into 5 steps:

1. Heat the ice to 0 ºC, which is the fusion temperature.

2. Melt the ice (obtaining liquid water), which is a process at constant pressure and temperature, so the liquid obtained is also at 0ºC.

3. Heat the liquid water from 0 ºC to 100 ºC, which is the vaporization normal temperature of the water.

4. Vaporization of all the water; this is also a process that occurs at constant pressure and temperature, so the produced steam will be at 100ºC.

5. Heat the steam from 100 ºC to 182 ºC.

Each process has a required energy, and the sum of the energy required for each and all of the steps is the total amount of energy required for the whole process:

is a heating process for the ice, so we know that the energy required is proportional to the temperature difference through the specific heat:

is a phase change process, so we do not use the specific heat (sensible heat), but the fusion heat (latent heat), so:

Analogously,

Finally, the total energy required is:

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