3.7.0.0: Heating Curves and Phase Changes (Problems)

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PROBLEM $$\PageIndex{1}$$

From the phase diagram for water, determine the state of water at:

1. 35 °C and 85 kPa
2. −15 °C and 40 kPa
3. −15 °C and 0.1 kPa
4. 75 °C and 3 kPa
5. 40 °C and 0.1 kPa
6. 60 °C and 50 kPa

Liquid

solid

solid

gas

gas

liquid

PROBLEM $$\PageIndex{2}$$

Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water that you drink may eventually be converted into sweat and evaporate. If you drink a 20-ounce bottle of water that had been in the refrigerator at 3.8 °C, how much heat is needed to convert all of that water into sweat and then to vapor?? (Note: Your body temperature is 36.6 °C. For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water.)

81.17 kJ

PROBLEM $$\PageIndex{3}$$

How much heat is required to convert 422 g of liquid H2O at 23.5 °C into steam at 150 °C?

1130 kJ

PROBLEM $$\PageIndex{4}$$

Titanium tetrachloride, TiCl4, has a melting point of −23.2 °C and has a ΔH fusion = 9.37 kJ/mol.

1. How much energy is required to melt 263.1 g TiCl4?
2. For TiCl4, which will likely have the larger magnitude: ΔH fusion or ΔH vaporization? Explain your reasoning.

13.0 kJ

It is likely that the heat of vaporization will have a larger magnitude since in the case of vaporization the intermolecular interactions have to be completely overcome, while melting weakens or destroys only some of them.

PROBLEM $$\PageIndex{5}$$

What phase changes will take place when water is subjected to varying pressure at a constant temperature of 0.005 °C? At 40 °C? At −40 °C?

0.005 °C: gas to solid to liquid

40 °C: gas to liquid

−40 °C: gas to solid to liquid (maybe)

PROBLEM $$\PageIndex{6}$$

From the phase diagram for carbon dioxide, determine the state of CO2 at:

1. 20 °C and 1000 kPa
2. 10 °C and 2000 kPa
3. 10 °C and 100 kPa
4. −40 °C and 500 kPa
5. −80 °C and 1500 kPa
6. −80 °C and 10 kPa

liquid

solid

gas

gas

gas

gas

PROBLEM $$\PageIndex{7}$$

Determine the phase changes that carbon dioxide undergoes as the pressure changes if the temperature is held at −50 °C? If the temperature is held at −40 °C? At 20 °C?

−50 °C: gas to liquid to solid

−40 °C: gas to liquid to solid

20 °C: gas to liquid to solid

PROBLEM $$\PageIndex{8}$$

Dry ice, CO2(s), does not melt at atmospheric pressure. It sublimes at a temperature of −78 °C. What is the lowest pressure at which CO2(s) will melt to give CO2(l)? At approximately what temperature will this occur?

Dry ice, CO2(s), will melt to give CO2(l) at 5.11 atm at −56.6 °C, the triple point of carbon dioxide.

PROBLEM $$\PageIndex{9}$$

Elemental carbon has one gas phase, one liquid phase, and three different solid phases, as shown in the phase diagram:

1. On the phase diagram, label the gas and liquid regions.
2. Graphite is the most stable phase of carbon at normal conditions. On the phase diagram, label the graphite phase.
3. If graphite at normal conditions is heated to 2500 K while the pressure is increased to 1010 Pa, it is converted into diamond. Label the diamond phase.
4. Circle each triple point on the phase diagram.
5. In what phase does carbon exist at 5000 K and 108 Pa?
6. If the temperature of a sample of carbon increases from 3000 K to 5000 K at a constant pressure of 106 Pa, which phase transition occurs, if any?

liquid

sublimation