How much thermal energy is added to 10.0 g of ice at - 20.0°C to convert it to water vapor at 120.0°C?

7479 cal.

31262.2 joules

Explanation:

This is a calorimetry problem where water in its three states changes from ice to vapor.

We must use, the calorimetry formula and the formula for latent heat.

Q = m. C. ΔT

Q = Clat. m

First of all, let's determine the heat for ice, before it melts.

10 g. 0.5 cal/g°C (0° - (-20°C) = 100 cal

Now, the ice has melted.

Q = Clat heat of fusion. 10 g

Q = 79.7 cal/g. 10 g → 797 cal

We have water at 0°, so this water has to receive heat until it becomes vapor. Let's determine that heat.

Q = m. C. ΔT

Q = 10 g. 1 cal/g°C (100°C - 0°C) → 1000 cal

Water is ready now, to become vapor so let's determine the heat.

Q = Clat heat of vaporization. m

Q = 539.4 cal/g. 10 g → 5394 cal

Finally we have vapor water, so let's determine the heat gained when this vapor changes the T° from 100°C to 120°

Q = m. C. ΔT

Q = 10 g. 0.470 cal/g°C. (120°C - 100°C) → 94 cal

Now, we have to sum all the heat that was added in all the process.

100 cal + 797 cal + 1000 cal + 5394 cal + 94 cal = 7479 cal.

We can convert this unit to joules, which is more acceptable for energy terms.

1 cal is 4.18 Joules.

Then, 7479 cal are (7479. 4.18) = 31262.2 joules