1. JEOPARDY REVIEW
The Gas Laws

2. Jeopardy Categories
Boyle’s
Law
Charles’ Law
Combined Gas Law
PV=nRT
Graham’s Law
Dalton’s Law
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3. Boyle’s Law- $100 INVERSELY
According to Boyle’s Law, the volume of a gas varies ____________ (directly or inversely)
with its pressure, assuming that temperature is constant.
INVERSELY
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4. Boyle’s Law- $200 DECREASES
According to Boyle’s Law, the volume of a gas ______________ (increases, decreases, or stays the same) when the pressure increases and temperature is held constant.
DECREASES
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5. Boyle’s Law- $300
A sample of oxygen gas at constant temperature occupies a volume of mL at 740. torr pressure. What volume in mL will it occupy at 800. torr pressure?
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6. Boyle’s Law- $500
Ammonia gas occupies a volume of 450. mL at a pressure of 720. mm Hg. What volume in mL will it occupy at standard pressure?
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7. Boyle’s Law- $1000
Fluorine gas has a volume of 317 mL. When the volume is decreased to 250. mL, its pressure is 1.50 atm. What was the original pressure in torr?
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8. CHARLES $100
According to Charles’ Law, the volume of a gas varies ____________ (directly or inversely)
with the Kelvin temperature, assuming that pressure is constant.
DIRECTLY
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9. CHARLES - $200
According to Charles’ Law, the volume of a gas ______________ (increases, decreases, or stays the same) when the temperature increases and pressure is held constant.
INCREASES
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10. CHARLES - $300
A sample of nitrogen occupies a volume of L at 298 K. What volume in liters will it occupy at 368 K?
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11. CHARLES - $500
Hydrogen gas was cooled from 423K to 323K. Its new volume is liters. What was its original volume?
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12. CHARLES - $1000
A sample of argon gas is cooled and its volume decreased from mL to mL. If its final temperature was 218 K, what was its original temperature in degrees Celsius?
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13. VOLUME PRESSURE TEMPERATURE
Combined - $100
What are the three variables in the Combined Gas Law?
VOLUME PRESSURE TEMPERATURE
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14. Combined - $200 V1 = 3.0 L V2 = ? T1 = 293 K T2 = 303 K
P1 = 1.5 atm P2 = 2.5 atm
V1 = 3.0 L V2 = ?
T1 = 293 K T2 = 303 K
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15. Combined - $300 V1 = 0.256 L V2 = 0.250 L T1 = 298 K T2 = 323 K
P1 = 720. torr P2 = ?
V1 = L V2 = L
T1 = 298 K T2 = 323 K
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16. Combined - $500 V1 = 4.00 L V2 = 6.00 L T1 = ? T2 = 471 K
P1 = 95.0 kPa P2 = 101kPa
V1 = 4.00 L V2 = 6.00 L
T1 = ? T2 = 471 K
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17. Combined - $1000
A gas has an initial volume of 125 mL and pressure of 125 kPa. When its volume is decreased to 100. mL and its pressure is decreased to 100. kPa, its temperature is changed to 348 K. What is the initial temperature of this gas in K?
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18. PV=nRT - $100
Why must pressure be in atmospheres, volume be in liters, and temperature be in Kelvin when using the constant with a numerical value of ?
Because the Universal Gas Constant, R, that has a value of has a unit of (L•atm)/(mol•K). The units must be consistent or they will not cancel out.
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19. PV=nRT - $200
How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 298 K?
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20. PV=nRT - $300
What volume will 2.0 moles of nitrogen occupy at atm and 293 K?
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21. PV=nRT - $500
At what temperature will 0.70 mol of chlorine gas exert a pressure of 900. torr of pressure at a and a volume of 500. mL?
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22. PV=nRT - $1000
An elemental gas has a mass of 10.3 g. If the volume is 58,400 mL and the pressure is 758 mm Hg at a temperature of 2.5°C, how many moles are present? What is the gas?
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23. GRAHAM - $100 Rates of EFFUSION
Graham’s Law allows a scientist to make predictions about what property of gases if the molecular masses are known?
Rates of EFFUSION
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24. GRAHAM - $200
According to Graham’s Law, a gas will effuse at a rate that is _____________ proportional to the square root of its molecular mass.
INVERSELY
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25. GRAHAM - $300
Based on molecular masses, which will effuse faster: Hydrogen or Oxygen
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26. GRAHAM - $500
Arrange the following gases in order of increasing rates of effusion (slowest to fastest): NH3, CO2, He, Cl2
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27. GRAHAM - $1000
Under the same conditions of temperature and pressure, what is the relative rate of effusion of oxygen gas effuse compared to hydrogen gas?
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28. TOTAL PRESSURE DALTON - $100
Dalton’s Law says that the sum of the individual pressures of all the gases that make up a mixture is equal to the ___________ ___________.
TOTAL PRESSURE
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29. DALTON - $200
The partial pressures of a gas are 22.1 torr, 168 torr, and 33.0 torr. What is the total pressure of this gas?
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30. DALTON - $300
A 250. mL sample of oxygen is collected over water at 25.0°C and torr pressure. What is the pressure of the dry gas alone? (Vapor pressure of water at 25.0 °C = 23.8 torr)
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31. DALTON - $500
A mixture of 2.00 moles of hydrogen, 3.00 moles of ammonia, 4.00 moles of carbon dioxide, and 5.00 moles of nitrogen exerts a total pressure of 800. torr. What is the partial pressure in torr of carbon dioxide?
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32. What element is used when discussing units of pressure in mm?
DALTON - $1000
What element is used when discussing units of pressure in mm?
(pressure= mm ____ )
Mercury ; Hg
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