Gas Laws Quiz Questions And Answers
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Do you know about the gas laws in chemistry? Take this gas laws quiz to see how well you know about the laws of gas. The gas laws consist of three primary laws, i.e., Charles' Law, Boyle's Law, and Avogadro's Law, all of which will later combine into the General Gas Equation and Ideal Gas Law. How attentive were you when we were taught about gas laws and their formulas in class? Take up the quiz below and get to test your understanding. All the best! Share the quiz with friends for practice.
Questions and Answers
- 1.
A bottle is filled with oxygen and sealed at room temperature. The bottle is then left in a hot car. According to Charles' law, the pressure in the bottle will increase from heating.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
True. According to Charles' Law, which describes the relationship between the temperature and volume of a gas at constant pressure, when the temperature of a gas increases, its volume also increases (assuming the pressure remains constant). In the scenario you described, as the bottle of oxygen is left in a hot car, the temperature inside the bottle increases, and according to Charles' Law, this would lead to an increase in volume. Since the bottle is sealed, the increased volume results in increased pressure inside the bottle. Therefore, the statement is true: the pressure in the bottle will increase from heating.Rate this question:
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- 2.
Nitrogen gas has occupied a volume of 500ml at a pressure of 0.971atm. What volume will the gas fill at a pressure of 1.50 atm, assuming the temperature remains constant?
- A.
342mL
- B.
424mL
- C.
324mL
- D.
442mL
- E.
242mL
Correct Answer
C. 324mLExplanation
According to Boyle's Law, at constant temperature, the product of pressure and volume is constant. Therefore, we can use the following equation to solve for the new volume: (Pressure1 * Volume1) = (Pressure2 * Volume2). Plugging in the given values, we have (0.971 atm * 500 mL) = (1.50 atm * Volume2). Solving for Volume2, we get Volume2 = (0.971 atm * 500 mL) / (1.50 atm) = 324 mL. Therefore, the gas will fill a volume of 324 mL at a pressure of 1.50 atm, assuming the temperature remains constant.Rate this question:
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- 3.
Not all Gas Law problems have Kelvin (K) as the unit of temperature. They can be expressed in Celsius (°C) and Fahrenheit(°F). So, convert 123°C to K.
- A.
396K
- B.
486K
- C.
369K
- D.
458K
- E.
693K
Correct Answer
A. 396KExplanation
Gas Law problems can be solved using different units of temperature, including Celsius and Fahrenheit. In this question, the task is to convert 123°C to Kelvin. To convert Celsius to Kelvin, we add 273.15 to the Celsius value. Therefore, 123°C + 273.15 = 396.15K. Rounding to the nearest whole number, the correct answer is 396K.Rate this question:
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- 4.
Gas pressure is caused by:
- A.
Gas molecules heating up.
- B.
Gas molecules react with other gas molecules.
- C.
Gas molecules hitting the walls of a container.
- D.
Gas molecules hitting other gas molecules.
Correct Answer
C. Gas molecules hitting the walls of a container.Explanation
Gas pressure is caused by gas molecules hitting the walls of a container. When gas molecules move around randomly, they collide with the walls of the container, exerting a force on them. This force per unit area is what we refer to as gas pressure. The more frequently and forcefully the molecules collide with the walls, the higher the gas pressure will be. Heating up the gas molecules or their reactions with other gas molecules may affect their speed and energy, but it is the collisions with the container walls that directly contribute to the gas pressure.Rate this question:
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- 5.
At a pressure of 5.0 atmospheres, a sample of gas occupies 40 liters. What volume will the same sample occupy at 1.0 atmosphere?
- A.
0.0050 L
- B.
0.13 L
- C.
200 L
- D.
8.0 L
Correct Answer
C. 200 LExplanation
According to Boyle's Law, the volume of a gas is inversely proportional to its pressure, when the temperature and amount of gas are constant. Therefore, if the pressure decreases by a factor of 5 (from 5.0 atm to 1.0 atm), the volume will increase by the same factor. Since the initial volume is 40 liters, the final volume will be 40 liters multiplied by 5, which equals 200 liters.Rate this question:
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- 6.
As the volume of confined gas decreases at the constant temperature, the pressure exerted by the gas ______.
- A.
Decreases
- B.
Increases
- C.
Stay the same
- D.
Fluctuates
Correct Answer
B. IncreasesExplanation
When the volume of a confined gas decreases at a constant temperature, the gas particles are forced into a smaller space, leading to more frequent collisions with the walls of the container. These collisions result in an increase in the pressure exerted by the gas. Therefore, as the volume decreases, the pressure exerted by the gas increases.Rate this question:
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- 7.
A sample of Argon has a volume of 0.43 mL at 299K. At what temperature in degrees Celsius will it have a volume of 1 mL if the pressure remains constant?
- A.
695°C
- B.
422°C
- C.
428°C
- D.
694°C
Correct Answer
B. 422°CExplanation
To solve this problem, you can use the combined gas law, which relates the initial and final conditions of a gas sample. The combined gas law is expressed as:
(P₁ * V₁) / T₁ = (P₂ * V₂) / T₂
Where:
P₁ and P₂ are the initial and final pressures (which can be assumed to be constant unless mentioned).
V₁ and V₂ are the initial and final volumes.
T₁ and T₂ are the initial and final temperatures in Kelvin.
In this case, you're given V₁ = 0.43 mL and T₁ = 299 K.
The pressure remains constant. You want to find T₂ when V₂ = 1 mL.
Let's plug these values into the equation:
P₁ (0.43 mL) / 299 K = P2 (1 mL)/ T₂
T₂ = 299 / 0.43
T₂ ≈ 695.35 K
To convert this temperature to degrees Celsius, subtract 273.15:
T₂ ≈ 695.35 K - 273.15 ≈ 422.2°C
So, the correct answer is approximately 422°C.Rate this question:
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- 8.
Each of these flasks contains the same number of molecules. In which container is the pressure highest?
- A.
Flask 1
- B.
Flask 2
- C.
Flask 3
- D.
Flask 4
- E.
Flask 5
Correct Answer
A. Flask 1Explanation
As the volume decrease the pressure increases because there are more collisions per unit of surface area within the container.Rate this question:
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- 9.
A Good example of Charles' law is when a piece of metal expands in the heat.
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
Gas laws are not applicable to SOLIDSRate this question:
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- 10.
Assume that the temperature remains constant. How can you increase the pressure of a gas without changing the number of gas particles?
- A.
Increase the container volume.
- B.
Add more molecules of the gas.
- C.
Decrease the container volume.
- D.
None of the above.
Correct Answer
C. Decrease the container volume.Explanation
Boyle's law, a fundamental gas law, states that at a constant temperature, the pressure of a gas is inversely proportional to its volume. In other words, as the volume decreases, the pressure increases, and vice versa.Rate this question:
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- 11.
In a closed container at 1.0 atmosphere, the temperature of a sample of gas is raised from 300 K to 400 K. What will be the final pressure of the gas?
- A.
0.010 atm
- B.
0 atm
- C.
100 atm
- D.
1.3 atm
Correct Answer
D. 1.3 atmExplanation
When the temperature of a gas is increased while keeping the volume constant, the pressure of the gas also increases. This relationship is described by the ideal gas law, which states that pressure is directly proportional to temperature. Therefore, when the temperature is raised from 300 K to 400 K, the pressure of the gas will also increase. The correct answer of 1.3 atm indicates that the final pressure of the gas will be higher than the initial pressure of 1.0 atm.Rate this question:
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- 12.
At constant pressure and 25°C, a sample of gas occupies 4.5 liters. At what temperature will the gas occupy 9.0 liters?
- A.
596K
- B.
50K
- C.
50°C
- D.
596°C
Correct Answer
A. 596KExplanation
According to Charles's Law, the volume of a gas is directly proportional to its temperature, assuming constant pressure. Therefore, if the initial volume is 4.5 liters and the final volume is 9.0 liters, the temperature must double to achieve this doubling in volume. Since the initial temperature is 25°C, which is equivalent to 298K, the final temperature can be calculated by doubling this value, resulting in 596K. Always convert temperatures to Kelvin before using the combined gas law.Rate this question:
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- 13.
You drove continuously from Laguna to Manila, and you observed that the pressure in your tires increased. This is because of the increased temperature outside the tire caused by friction.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
As you drive, the friction between the tires and the road generates heat, causing the temperature of the air inside the tires to rise. Since the tires are closed systems, the increased temperature leads to an increase in the pressure of the air inside. This phenomenon is described by the ideal gas law, which states that as the temperature of a gas increases, its pressure also increases, assuming the volume and amount of gas remain constant.Rate this question:
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- 14.
Each of these flasks contains the same number of gas molecules. In which would the pressure be lowest?
- A.
Flask 1
- B.
Flask 2
- C.
Flask 3
- D.
Flask 4
Correct Answer
A. Flask 1Explanation
As the temperature decreases, molecules move more slowly and collide with the walls of the containerless often.Rate this question:
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- 15.
Neon gas has a volume of 2,000 ml with a pressure of 1.8atm. However, the pressure decreased to 1.3 atm; what is now the volume of the neon gas?
- A.
2, 795mL
- B.
2,769mL
- C.
3,795mL
- D.
3,759mL
Correct Answer
B. 2,769mLExplanation
The volume of a gas is inversely proportional to its pressure, according to Boyle's Law.
According to this law, P1V1= P2V2
Using this formula we can calculate the new volume
1.8*2000= 1.3*V2
V2= 2769 ml approximatelyRate this question:
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- 16.
Each of these flasks is the same size and at the same temperature. Which one contains the most molecules?
- A.
Flask 1
- B.
Flask 2
- C.
Flask 3
- D.
Flask 4
Correct Answer
D. Flask 4Explanation
The highest pressure indicates the greatest number of collisions with the wall of the container, and therefore the most molecules.Rate this question:
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- 17.
When a supply of hydrogen gas is held in a 4-liter container at 320 K, it exerts a pressure of 800 torrs. The supply is moved to a 2-liter container and cooled to 160 K. What is the new pressure of the confined gas?
- A.
800 torr
- B.
1600 torr
- C.
200 torr
- D.
400 torr
Correct Answer
A. 800 torrExplanation
The pressure of a gas is directly proportional to its temperature and inversely proportional to its volume, according to the ideal gas law. When the supply of hydrogen gas is moved to a 2-liter container, the volume is halved. Since the volume is reduced by half, the pressure will double. However, when the gas is cooled to 160 K, the temperature is also halved. Since the temperature is reduced by half, the pressure will also be halved. Therefore, the new pressure of the confined gas will remain the same as the original pressure, which is 800 torr.Rate this question:
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- 18.
Which Gas Law is involved when a balloon pops after being sat on?
- A.
Charles Law
- B.
Boyle's Law
- C.
Law of Pressure Gradient
- D.
None of the Above
Correct Answer
B. Boyle's LawExplanation
According to Boyle's Law “at a constant temperature, increases in pressure is directly proportional to the increase in volume.Rate this question:
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- 19.
A small sample of helium gas occupies 6 mL at a temperature of 250 K. At what temperature does the volume expand to 9 mL?
- A.
125K
- B.
375K
- C.
500K
- D.
2250K
Correct Answer
B. 375KExplanation
As the volume of the gas increases from 6 mL to 9 mL, it means that the gas is expanding. According to Charles's Law, the volume of a gas is directly proportional to its temperature, assuming constant pressure. Therefore, if the volume increases, the temperature must also increase. Since the initial temperature is 250 K and the final volume is 9 mL, we can set up a proportion: (6 mL / 250 K) = (9 mL / x). Solving for x, we find that the final temperature is 375 K.Rate this question:
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- 20.
Organize the following gasses in order of their rates of diffusion, from slowest to fastest.
- oxygen, O2
- ammonia, NH3
- hydrogen, H2
- carbon dioxide, CO2
- A.
Hydrogen, oxygen, carbon dioxide, ammonia
- B.
Oxygen, hydrogen, carbon dioxide, ammonia
- C.
Hydrogen, ammonia, oxygen, carbon dioxide
- D.
Hydrogen, oxygen, ammonia, carbon dioxide
- E.
Carbon dioxide, oxygen, ammonia, hydrogen
Correct Answer
E. Carbon dioxide, oxygen, ammonia, hydrogenExplanation
The correct order of the gases from slowest to fastest rates of diffusion is carbon dioxide, oxygen, ammonia, and hydrogen. This is because carbon dioxide molecules are larger and heavier, making them diffuse more slowly. Oxygen molecules are smaller and lighter, allowing them to diffuse faster than carbon dioxide. Ammonia molecules are smaller and lighter than oxygen molecules, so they diffuse even faster. Hydrogen molecules are the smallest and lightest, resulting in the fastest rate of diffusion.Rate this question:
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Feb 02, 2024Quiz Edited by
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Jan 23, 2009Quiz Created by
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