Questions on Gas Pressure
Multiple-Choice Questions – Gas Pressure
1. What is the primary cause of gas pressure in a container?
A) Attraction between gas molecules
B) Expansion of gas volume
C) Collisions of gas particles with the container walls
D) The gravitational pull of the Earth
E) Movement of electrons
2. Which instrument is used to measure atmospheric pressure?
A) Thermometer
B) Barometer
C) Calorimeter
D) Voltmeter
E) Hygrometer
3. Standard atmospheric pressure at sea level is:
A) 101.3 °C
B) 273 mmHg
C) 1 atm
D) 760 cmHg
E) 100 kPa
4. Which of the following units is not used to measure gas pressure?
A) atm
B) mmHg
C) kPa
D) °C
E) torr
5. The pressure exerted by a gas is directly proportional to:
A) The gravitational force
B) The volume of the container
C) The number of collisions with container walls
D) The surface area of the container
E) The shape of gas molecules
6. As the volume of a gas decreases, the pressure:
A) Increases
B) Decreases
C) Stays the same
D) Becomes zero
E) Doubles regardless of temperature
7. What happens to gas pressure if temperature increases (with volume constant)?
A) Decreases
B) Increases
C) Remains unchanged
D) Becomes zero
E) Depends on molar mass
8. Atmospheric pressure is caused by:
A) Magnetic fields
B) Heat from the sun
C) Weight of the air
D) Gravity of the moon
E) Rotation of the Earth
9. Which gas law relates pressure and volume?
A) Charles’s Law
B) Avogadro’s Law
C) Boyle’s Law
D) Gay-Lussac’s Law
E) Dalton’s Law
10. When the pressure on a gas increases and temperature is constant, the volume:
A) Increases
B) Remains constant
C) Decreases
D) Doubles
E) Becomes zero
11. Which statement is true about pressure in a gas?
A) It only exists in solids
B) It’s only affected by temperature
C) It is uniform throughout a closed container
D) It depends on the color of the gas
E) It is stronger at the top of the container
12. What is 760 mmHg equivalent to?
A) 1.00 atm
B) 100 atm
C) 0.10 atm
D) 7.6 atm
E) 1013 atm
13. If the number of moles of gas increases in a sealed container, the pressure will:
A) Stay the same
B) Decrease
C) Increase
D) Become zero
E) Double regardless of temperature
14. A gas pressure of 2 atm is equal to:
A) 1520 mmHg
B) 760 mmHg
C) 101.3 kPa
D) 1.5 atm
E) 500 mmHg
15. Which factor does not affect gas pressure?
A) Number of particles
B) Temperature
C) Volume
D) Color of the gas
E) Frequency of collisions
16. Gas pressure inside a tire increases on a hot day because:
A) Tire rubber expands
B) Air leaks out
C) Gas molecules move faster
D) Gravity pulls harder
E) Molecules become larger
17. Partial pressure refers to:
A) The pressure of the heaviest gas only
B) The pressure of one gas in a mixture
C) The total pressure of a gas
D) The difference between internal and external pressure
E) The volume of the gas
18. Dalton’s Law of Partial Pressures states:
A) Total pressure is the sum of partial pressures
B) Gas volume is constant
C) Gases move at the same speed
D) Pressure decreases at high temperature
E) All gases behave identically
19. If pressure is measured as 405 mmHg, what is it in atm?
A) 0.75 atm
B) 0.53 atm
C) 0.85 atm
D) 0.33 atm
E) 0.25 atm
20. In a rigid container, doubling the temperature (in Kelvin) of a gas will:
A) Double the pressure
B) Halve the pressure
C) Not affect pressure
D) Stop particle motion
E) Remove all collisions
Answers and Explanations
1. C – Gas pressure is due to collisions of particles with the container walls.
2. B – A barometer is used to measure atmospheric pressure.
3. C – Standard pressure = 1 atm, also equal to 760 mmHg or 101.3 kPa.
4. D – Celsius (°C) is a temperature unit, not for pressure.
5. C – More frequent collisions = higher pressure.
6. A – As volume decreases, particles collide more often = pressure increases.
7. B – Temperature rise = faster particles = higher pressure.
8. C – Atmospheric pressure results from the weight of air above us.
9. C – Boyle’s Law: Pressure ∝ 1/Volume (at constant T).
10. C – Increase in pressure compresses gas, reducing volume.
11. C – In a closed container, gas pressure is evenly distributed.
12. A – 760 mmHg = 1 atm = 101.3 kPa.
13. C – More gas particles = more collisions = higher pressure.
14. A – 1 atm = 760 mmHg → 2 atm = 1520 mmHg.
15. D – Color has no effect on pressure.
16. C – Higher temperature increases particle speed, which increases pressure.
17. B – Partial pressure is the pressure from one gas in a mixture.
18. A – Dalton’s Law: Total pressure = sum of individual gas pressures.
19. B – 405 mmHg ÷ 760 mmHg = 0.53 atm.
20. A – For constant volume, pressure ∝ temperature (Kelvin) → pressure doubles.
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