Title: Chapter 9: Gases
Course: Test

Q: On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____.
- Boyles law
- Ideal gas law
- Charles law
A: Charles law

Q: What is the relationship between pressure and volume of a gas at constant temperature?
- as volume decreases, pressure increases
- as volume decreases, pressure decreases
- as volume increases, pressure increases
A: as volume decreases, pressure increases

Q: How many mm Hg are in 0.890 atm of pressure?
- 854 mm Hg
- 676 mm Hg
- 1.17 × 10^-3 mm Hg
A: 676 mm Hg

Q: How many atmospheres are in 710 mm Hg?
- 0.934 atm
- 1.07 atm
- 5.40 × 10^5 atm
A: 0.934 atm

Q: The average tire pressure for an automobile is 38.5 psi which is how many atmospheres of pressure?
- 1.77 × 10^-3 atm
- 566 atm
- 2.62 atm
A: 2.62 atm

Q: What is the volume for 1.00 mole of gas at STP?
- 24.5 L
- 22.4 L
- 2.05 L
A: 22.4 L

Q: What is the standard pressure for 1.00 mole of gas at STP?
- 760 mm Hg
- 1.03 atm
- 103 kPa
A: 760 mm Hg

Q: 286 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP?
- 572 L
- 143 L
- 286 L
A: 572 L

Q: 159 L of hydrogen gas at STP reacts with excess chorine gas. What is the maximum amount of gas product that can be formed at STP?
- 159 L
- 79.5 L
- 318 L
A: 318 L

Q: A _____ is an instrument used to measure atmospheric pressure specifically in the area of meteorology.
- barometer
- manometer
- altimeter
A: barometer

Q: A _____ is a general instrument that utilizes a liquid column, typically mercury, to measure pressure.
- barometer
- manometer
- altimeter
A: manometer

Q: How many psi are in 760. mm Hg?
- 1.47 × 10^1 psi
- 3.93 × 10^4 psi
- 2.54 × 10^-5 psi
A: 1.47 × 10^1 psi

Q: A sample of nitrogen gas occupies 9.20 L at 21 °C and 0.959 atm. If the pressure is increased to 1.15 atm at constant temperature, what is the newly occupied volume?
- 11.0 L
- 7.67 L
- 9.20 L
A: 7.67 L

Q: The pressure of a gas in a container is 1.85 atm and occupies a volume of 12.5 L. If the original volume is reduced by half at constant temperature, what would happen to the pressure?
- the pressure would double
- the pressure would reduce by half
- the pressure would remain the same
A: the pressure would double

Q: The pressure of a gas in a container is 1.23 atm and occupies a volume of 1.5 L. If the original volume is doubled at constant temperature, what would happen to the pressure?
- the pressure would remain the same
- the pressure would double
- the pressure would reduce by half
A: the pressure would reduce by half

Q: Suppose your car is equipped with tire pressure monitoring system (TPMS) and the tire pressure is 34.0 psi on a 98 °F day in California. You decided to take a road trip to Alaska where the temperature drops to 20 °F. As you arrived in Alaska, you noticed that the tire pressure monitoring system alert light is illuminated. Why did this happen?
- as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated
- as temperature decreases, gas molecules gain kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated
- as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated
A: as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated

Q: On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. Why did this happen?
- as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips
- as temperature increases, gas molecules lose kinetic energy and the volume of gas increases inside the bag of chips
- as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips
A: as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips

Q: What mass of nitrogen is needed to fill an 855 L tank at STP?
- 0.978 kg
- 1.07 kg
- 0.533 kg
A: 1.07 kg

Q: What mass of oxygen is needed to fill a 585 L tank at STP?
- 0.835 kg
- 0.765 kg
- 0.417 kg
A: 0.835 kg

Q: What is the pressure in a 5.80 L container that has 0.545 moles of oxygen gas at 22.0 °C?
- 0.170 atm
- 2.28 atm
- 231 atm
A: 2.28 atm

Q: What is the pressure in a 3.41 L container that has 0.741 moles of oxygen gas at 26.0 °C?
- 5.34 atm
- 0.464 atm
- 62.0 atm
A: 5.34 atm

Q: How many moles of CO_2 gas are present in a 9.1 L container at 25 °C and 1.35 atm?
- 4.96 × 10^-3 moles
- 5.99 moles
- 0.502 moles
A: 0.502 moles

Q: Oxygen gas (P_O_2 = 1.10 atm), nitrogen gas (P_N_2 = 0.840 atm), and carbon dioxide gas (P_CO_2 = 0.125 atm) occupy the same container. What is the total pressure in the container?
- 2.07 atm
- 1.94 atm
- 0.135 atm
A: 2.07 atm

Q: A container filled with neon and argon gas is 25.00% by volume neon. What is the partial pressure of argon if the total pressure inside the container is 5.500 atm?
- 412.5 atm
- 1.375 atm
- 4.125 atm
A: 4.125 atm

Q: A container filled with helium and argon gas is 8.00% by volume argon. What is the partial pressure of argon if the total pressure inside the container is 4.100 atm?
- 0.328 atm
- 3.77 atm
- 32.8 atm
A: 0.328 atm

Q: What is the temperature for STP conditions?
- 273.15 K
- 298.15 K
- 0 K
A: 273.15 K

Q: What is the pressure for STP conditions?
- 740 mm Hg
- 780 mm Hg
- 760 mm Hg
A: 760 mm Hg

Q: 28.5 L of an unknown gas has a mass of 55.92 g at STP. What is the identity of the unknown gas?
- CO_2
- O_2
- N_2
A: CO_2