Name: ______Date: ______Mods: ______
Chapter 10 Review Sheet
Part 1: Vocabulary
Define the following terms, using your class notes, reading guide or text book:
surface tensionamorphous solidadhesiondeposition
capillary actioncrystalline solidcohesionmelting
effusionunit cellcondensationfreezing
diffusionvapor pressureevaporationviscosity
fluidvolatilesublimationtriple point
Part 2: Phase Diagrams
Refer to the phase diagram below when answering the questions:
NOTE: “Normal” refers 1 atm = 101.3 kpa = 760 mmHg
1) What is the normalfreezing point of this substance? ______
2) What is the normal boiling point of this substance? ______
3) What is the normalmelting point of this substance? ______
4) What is the phase (s, l, g) of a substance at 2.0 atm and 100 °C? ______
5) What is the phase (s, l, g) of a substance at 0.75 atm and 100 °C? ______
6) What is the phase (s, l, g) of a substance at 0.5 atm and 100 °C? ______
7) What is the phase (s, l, g) of a substance at 1.5 atm and 50 °C? ______
8) What is the phase (s, l, g) of a substance at 1.5 atm and 200°C? ______
9) What is the phase (s, l, g) of a substance at 1.5 atm and 800°C? ______
10) What is the condition of the triple pointof this substance? T= ______, P= ______
11) If a quantity of this substance was at an initial pressure of 1.25 atm and a temperature of 3000 Cwaslowered to a pressure of 0.25 atm, what phase transition(s) would occur? ______
12) If a quantity of this substance was at an initial pressure of 1.25 atm and a temperature of 00 C was lowered to a pressure of 0.25 atm, what phase transition(s) would occur? ______
13) If a quantity of this substance was at an initial pressure of 1.0 atm and a temperature of 2000 C was lowered to a temperature of -2000 C, what phase transition(s) would occur? ______
14) If a quantity of this substance was at an initial pressure of 0.5 atm and a temperature of 2000 C was lowered to a temperature of -2000 C, what phase transition(s) would occur? ______
15) If this substance was at a pressure of 2.0 atm, at what temperature would it melt? ______
16) If this substance was at a pressure of 2.0 atm, at what temperature would it boil? ______
17) If this substance was at a pressure of 0.75 atm, at what temperature would it melt? ______
18) If this substance was at a pressure of 0.75 atm, at what temperature would it boil? ______
19) At what temperature do the gas and liquid phases become indistinguishable from each other? ______
20) At what pressure would it be possible to find this substance in the gas, liquid, and solid phase?_____
Part 3: Vapor Pressure Diagrams
Use the following diagram to answer question 1-8 below.
1. What is the vapor pressure of A at 35°C? ______
2. What is the vapor pressure of B at 35°C? ______
3. At what temperature is the vapor pressure of A 106.6 kPa? ______
4. What is the vapor pressure of B at this temperature? ______
5. At what temperature is the vapor pressure of B 106.6 kPa? ______
6. What is the “normal” boiling point of A? ______
7. What is the “normal” boiling point of B? ______
8. At what temperature would A boil in Denver where atmospheric pressure is
93.3 kPa?______
The following table shows the vapor pressure of a certain liquid at various temperatures.
Graph the data in the table provided.
Temp (ºC) / Pressure (kPa) / Temp (ºC) / Pressure (kPa) / Temp (ºC) / Pressure (kPa)0 / 1 / 60 / 22 / 120 / 80
10 / 2 / 70 / 29 / 130 / 93
20 / 3 / 80 / 37 / 140 / 107
30 / 7 / 90 / 46 / 150 / 122
40 / 11 / 100 / 56
50 / 16 / 110 / 68
1. What effect does rising temperature have on vapor pressure?
3. If atmospheric pressure was hypothetically 96 kPa for this problem, what would be the normal
boiling point of the substance you graphed? ______
4. What would happen to the boiling point of the substance if the external pressure were to increase?
5. How would the cooking time of an egg that is to be hard boiled be affected by high altitude (like in Denver). Explain.