Make sure you check that all your September homework is done.
The answers to the three statements given in class:
1. Balloon expanding on a hot day.
Charle's Law as the changing variables are temperature and volume. The latex material of a balloon allows it to expand. As the heat increases, the particles increase their kinetic motion & collide more often on the sides of the moveable container causing it to expand and the volume of the balloon increases.
2. Can of hairspray exploding in a hot car.
Gay- Lussacs Law as the changing variables are pressure and temperature. The can is a non-moveable container. As the temperature increases inside the can, the kinetic energy of the molecules increases the amount of collisions on the side of the container and therefore increases the pressure inside of the can, eventually causing it to explode.
3. A can of hairspray exploding in an airplane.
Boyle's law as the changing variables are pressure and volume. ( Temperature would change however it would be cooler at higher altitudes and would not cause a can to explode). The can is a non-moveable container. As the air pressure outside the can decreases at high altitude, this causes the pressure inside the can to be greater than outside, thus allowing the gas molecules to push against the container and the can expands ( increasing the volume). Since the can is a non-moveable container, the ultimate result of the expansion of the can is for it to explode.
Gases
Avogadro`s Law: See Worksheet below
General/Combined gas law, Ideal gas law, and Boyle`s, Charles, GL`s and
Avogadro`s Law calculations
*only do significant figures and scientific notation for the questions
on pg 97-98*
Pg 104 # 1, 2, 4, 9, 10, 12
Pg 107 # 5, 8, 11
Pg 97 # 7, 10, 16, 20, 22, 29, 33, 35, 36, 38, 45, 47
Gas Stoichiometry
Pg 110 #2, 4, 6, 7, 8
Dalton's Law *Answer using significant figures*
Pg 113 #1, 3, 5, 8
Extra Practice for Dalton's Law attached below.
Review Sheet for Term 1 attached below.
Answers to homework pg 104
1. a) Under the same conditions each
container will have the same number of moles and therefore the same number of
molecules.
b) Helium 0.339 g
Oxygen 2.72 g
Carbon Dioxide 3.73 g
2. 971 kPa
4. 225 deg celsius or 498 K
9. 242 g/mol
10. 98.5 g
12. 44.2 g/mol
Answers to homework pg 107
5. 1.022 L
8. 0.127 L
11. 310 K
Answers to homework pg 97
7. 2.9 x 102 L
10. 8.23 L
16. 933 K
20. 0.386 L
22. 97 °C
29. 271 kPa
33. 91 L
35. 0.0098 mol
36. 6.34 x 10-3 g
38. a) 0.21 mol
b) 9.24 x 10-4 mol
c) 3.7 x 10 -3 mol
45. a) 8.93 x 10-2 mol
b) 3.01 x 10 23 molecules
47. The temperature at SATP is 25 °C, while at STP it is 0 °C. According to the kinetic theory of gases,
the higher the temperature, the higher the kinetic energy of the particles, the greater volume a gas will occupy due to expansion of the gas.
Answers to homework pg 110
#2. 114 g of nitrogen
#4. a) 64.99 L b) 1.63 x 10 ^24 molecules
#6. a) 78 L of water vapour b) 97.015 L
#7. b) 2.0 L
#8. a) 7.5 L b) 5.0 L
Answers to homework pg 113
#1, 3, 5, 8
#1. 301 kPa
#3. 13.92 kPa
#5. Methane = 750 kPa
Oxygen = 480 kPa
Nitrogen = 1100 kPa
Propane = 240 kPa
#8. Chlorine occupies 64.0% of the container
The answers to the three statements given in class:
1. Balloon expanding on a hot day.
Charle's Law as the changing variables are temperature and volume. The latex material of a balloon allows it to expand. As the heat increases, the particles increase their kinetic motion & collide more often on the sides of the moveable container causing it to expand and the volume of the balloon increases.
2. Can of hairspray exploding in a hot car.
Gay- Lussacs Law as the changing variables are pressure and temperature. The can is a non-moveable container. As the temperature increases inside the can, the kinetic energy of the molecules increases the amount of collisions on the side of the container and therefore increases the pressure inside of the can, eventually causing it to explode.
3. A can of hairspray exploding in an airplane.
Boyle's law as the changing variables are pressure and volume. ( Temperature would change however it would be cooler at higher altitudes and would not cause a can to explode). The can is a non-moveable container. As the air pressure outside the can decreases at high altitude, this causes the pressure inside the can to be greater than outside, thus allowing the gas molecules to push against the container and the can expands ( increasing the volume). Since the can is a non-moveable container, the ultimate result of the expansion of the can is for it to explode.
Gases
Avogadro`s Law: See Worksheet below
General/Combined gas law, Ideal gas law, and Boyle`s, Charles, GL`s and
Avogadro`s Law calculations
*only do significant figures and scientific notation for the questions
on pg 97-98*
Pg 104 # 1, 2, 4, 9, 10, 12
Pg 107 # 5, 8, 11
Pg 97 # 7, 10, 16, 20, 22, 29, 33, 35, 36, 38, 45, 47
Gas Stoichiometry
Pg 110 #2, 4, 6, 7, 8
Dalton's Law *Answer using significant figures*
Pg 113 #1, 3, 5, 8
Extra Practice for Dalton's Law attached below.
Review Sheet for Term 1 attached below.
Answers to homework pg 104
1. a) Under the same conditions each
container will have the same number of moles and therefore the same number of
molecules.
b) Helium 0.339 g
Oxygen 2.72 g
Carbon Dioxide 3.73 g
2. 971 kPa
4. 225 deg celsius or 498 K
9. 242 g/mol
10. 98.5 g
12. 44.2 g/mol
Answers to homework pg 107
5. 1.022 L
8. 0.127 L
11. 310 K
Answers to homework pg 97
7. 2.9 x 102 L
10. 8.23 L
16. 933 K
20. 0.386 L
22. 97 °C
29. 271 kPa
33. 91 L
35. 0.0098 mol
36. 6.34 x 10-3 g
38. a) 0.21 mol
b) 9.24 x 10-4 mol
c) 3.7 x 10 -3 mol
45. a) 8.93 x 10-2 mol
b) 3.01 x 10 23 molecules
47. The temperature at SATP is 25 °C, while at STP it is 0 °C. According to the kinetic theory of gases,
the higher the temperature, the higher the kinetic energy of the particles, the greater volume a gas will occupy due to expansion of the gas.
Answers to homework pg 110
#2. 114 g of nitrogen
#4. a) 64.99 L b) 1.63 x 10 ^24 molecules
#6. a) 78 L of water vapour b) 97.015 L
#7. b) 2.0 L
#8. a) 7.5 L b) 5.0 L
Answers to homework pg 113
#1, 3, 5, 8
#1. 301 kPa
#3. 13.92 kPa
#5. Methane = 750 kPa
Oxygen = 480 kPa
Nitrogen = 1100 kPa
Propane = 240 kPa
#8. Chlorine occupies 64.0% of the container
avogadroslawworksheet.doc | |
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answers_to_avogadro.pdf | |
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ideal_and_combined_gas_laws_ans.pdf | |
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partialpressures.pdf | |
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daltons_laws_of_partial_pressure_ans.pdf | |
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term1review.doc | |
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answers.docx | |
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