[Name of Test]



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Worksheet #1

1. Calculate the amount of heat in kilojoules needed to vaporize 1.50 moles of water at 100.0° C (ΔHvap = 40.7 kJ/mole)

2. How many moles of H2O at 100°C can be vaporized using 75.5 kJ? (ΔHvap = 40.79 kJ/mole)

3. If 1.48 kJ will melt 15.0 grams of C6H4Br2 at its melting point, what is the molar heat of fusion of C6H4Br2?

4. How many kJ are released when 25.0 grams of liquid water freezes to form ice at 0° C? (ΔHfus = 6.008 kJ/mole)

5. Calculate the amount of heat given off in kilojoules when 10.0 g of benzene condenses at it’s normal boiling point. (Benzene = C6H6, ΔHvap = 30.8 kJ/mole)

6. How much heat in kilojoules is absorbed when 4.00 moles of Carbon Tetrachloride is melted at it’s normal melting point? (ΔHfus = 3.28 kJ/mole)

7. How many joules are needed to heat 25.0 grams of aluminum (Cp = 0.899 J/g °C) from 10.5 °C to 40.7°C?

8. If a 55.75 gram block of metal at 25.2 °C absorbs 500 calories it will heat up to 95.7 °C. Calculate the specific heat of the metal.

9. If a 75.0 gram sample of iron (Cp = 0.444 J/g °C) at 15.2 °C absorbs 225 joules, what does the temperature become?

10. How many grams of silver (Cp = 0.444 J/g °C) can be cooled from 75.2 °C to 27.5 °C by releasing 525 joules of heat? (1 calorie = 4.184 joules)

Worksheet #2

7. How much heat in calories, will be needed to change the temperature of 10.0 g of liquid water from 20.0°C to 100.0°C? (Cp of H2O = 1.0 cal/g °C)

8. How many kJ are needed to convert 25.0 g of C2H5OH from a liquid at 50.0° C to a gas to 100.0° C.

For C2H5OH Boiling point = 78.0°C

Specific heat of liquid = 113 J/mole °C

Specific heat of gas = 86.5 J/mole °C

ΔHvap = 39.3 kJ/mole)

9. Calculate the number of calories needed when 80.0 g of ice at 0.00° C is changed to steam at 100.0° C. (Cp of H2O = 1.0 cal/g °C) (ΔHfus = 80 cal/g and ΔHvap = 540 cal/g)

10. Calculate the quantity of heat energy (to the nearest calorie) required to convert 15.0 g of ice at -8.00° C to steam at 105.0° C. (Specific heats: ice = 0.500 cal/ g°C; water = 1.00 cal/g° C; steam = 0.480ca1/g°C.) (ΔHfus = 80 cal/g and ΔHvap = 540 cal/g)

Review

1. Explain the relationship between equilibrium vapor pressure and intermolecular forces. Use water as an example of the relationship.

2. How much heat (in calories and joules) would it take to heat up: a) 36.0 grams of water from 10.0 to 20.0°C?

b) 2.00 moles of water from 20.0 to 30.0°C?

c) 1.204 x 1024 molecules of water from 273 K to 10.0 °C?

3. How much heat would be required to:

a) melt 54.0 g of ice at 0.00 °C?

b) boil the same amount of water at 100.0 °C?

4. Graph the following situation comparing heat and temperature:

90.0 grams of ice at - 10.0 °C is heated until it reaches a temperature of 85.0°C

5. Find out how much heat was required in the previous problems. Answer in cal, J, and KJ.

6. If 36.0 g of water at 35.0°C has 8.00 kJ of heat applied to it, what will the final temperature of the water be?

7. If 5.0 moles of a substance needs 35 J of heat to boil it, what is the substances molar heat of vaporization?

8. If 10.0 J can melt 60.0 g of a substance with a molar heat of fusion of 5.0 J/mole, what is the molar mass of the substance?

9. If 72.0 grams of steam at 105.0°C were cooled to 50.0°C, how much heat would the system have to lose? (Draw a picture)

10. What is the molar heat of vaporization of a substance where it takes 80.0 J to vaporize 40.0 moles?

Chapter 10 Last Chance Review

Answer these questions on a separate sheet of paper

1. Why are there so few liquids?

2. What are the 8 properties of liquids? (7) of solids?

3. Explain the properties of a liquid and of a solid in terms of the Kinetic Theory (motion, arrangement, and attractive forces.)

4. What is the difference between evaporation and boiling?

5. Explain (in detail) how a liquid can be boiled (two types). Your answer should contain information about atmospheric pressure, vapor pressure, temperature, liquid molecules, and vapor molecules.

6. What is the difference between a crystalline solid and an amorphous solid? How does their organization differ? How does this effect their melting points? What are some examples of each? In your answer, you should describe both solids in terms of their motion, arrangement, and attractive forces. Show me how these factors relate to melting point.

7. What are unit cells? What are the four types? What do they look like?

8. What are the 4 types of crystalline particles? Describe their binding forces. Relate their binding forces to their melting points and to their predominant state (solid, liquid, and/or gas).

9. Draw and label a phase diagram.

10. Understand Le Chatelier’ s Principle. What happens when stress is applied to a system?

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