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:

answer: the metamorphic rocks are formed when they are exposed to high pressure and high temperatures. this happens when one of the earth's plates comes in contact with the other plate by traveling in opposite directions, straight into each other or slipping under one another. the friction that is caused by this activity results in   melting of rocks and when it cools they are known as metamorphic rocks. this process needs a controlled amount of pressure and temperature otherwise it may turn into magma.