Unlock hundreds more features
Save your Quiz to the Dashboard
View and Export Results
Use AI to Create Quizzes and Analyse Results

OR
Sign inSign in with Facebook
Sign inSign in with Google
Quizzes > Quizzes for Business > Education

Chemistry Gas Laws Assessment Quiz

Test Your Knowledge of Gas Law Concepts

Difficulty: Moderate
Questions: 20
Learning OutcomesStudy Material
Colorful paper art depicting elements of a Chemistry Gas Laws Assessment Quiz

Ready to challenge yourself with a comprehensive chemistry gas law quiz? Joanna Weib invites students to explore core gas laws through engaging multiple-choice questions that cover real-world scenarios. This assessment is perfect for AP Chemistry students or anyone brushing up on Boyle's, Charles's, and Dalton's laws. After finishing, users can freely modify the test in our editor to tailor it for classroom or self-study use. Looking for more practice? Check out our Chemistry Knowledge Assessment Quiz , Chemistry Fundamentals Quiz , or browse all quizzes for additional topics.

A gas occupies 4.0 L at 1.0 atm and constant temperature. According to Boyle's law, what volume will it occupy at 2.0 atm?
4.0 L
2.0 L
1.0 L
8.0 L
Boyle's law states that pressure and volume are inversely proportional at constant temperature. Doubling the pressure halves the volume from 4.0 L to 2.0 L. Therefore, at 2.0 atm the volume is 4.0 L × (1.0 atm / 2.0 atm) = 2.0 L.
A gas has a volume of 2.0 L at 300 K and constant pressure. According to Charles's law, what will its volume be at 600 K?
4.0 L
2.0 L
6.0 L
1.0 L
Charles's law says that volume is directly proportional to temperature at constant pressure. Doubling the temperature from 300 K to 600 K doubles the volume from 2.0 L to 4.0 L.
Which gas law describes the direct proportionality between pressure and temperature for a fixed volume of gas?
Gay-Lussac's law
Charles's law
Boyle's law
Avogadro's law
Gay-Lussac's law states that pressure is directly proportional to absolute temperature at constant volume. This contrasts with Charles's law, which relates volume and temperature. Thus, for constant volume, pressure increases as temperature increases, as described by Gay-Lussac's law.
A gas sample has a pressure of 1.0 atm at 200 K. If it is heated to 400 K at constant volume, what is its new pressure?
0.5 atm
2.0 atm
1.0 atm
4.0 atm
By Gay-Lussac's law, pressure is proportional to temperature at constant volume. Doubling the temperature from 200 K to 400 K doubles the pressure from 1.0 atm to 2.0 atm. Therefore, the new pressure is 2.0 atm.
Which law relates the volume of a gas to the number of moles at constant temperature and pressure?
Avogadro's law
Charles's law
Boyle's law
Dalton's law
Avogadro's law states that equal volumes of gases at the same temperature and pressure contain equal numbers of moles. This law directly connects volume and amount (moles) of gas. Therefore, volume is proportional to number of moles.
A 5.0 L gas sample at 1.0 atm and 300 K is heated to 400 K while the pressure is increased to 2.0 atm. Using the combined gas law, what is the new volume?
6.67 L
2.50 L
3.33 L
5.00 L
The combined gas law relates pressure, volume, and temperature. Plugging in the values yields V2 = 5.0 L × (1.0 atm / 2.0 atm) × (400 K / 300 K) ≈ 3.33 L. Therefore the new volume is approximately 3.33 L.
Using the ideal gas law, how many moles of an ideal gas occupy 2.0 L at 1.0 atm and 273 K? (R = 0.0821 L·atm·K−1·mol−1)
1.00 mol
0.089 mol
0.167 mol
0.100 mol
The ideal gas law PV = nRT gives n = PV/RT = (1.0 atm × 2.0 L) / (0.0821 × 273 K) ≈ 0.089 mol. This calculation uses R = 0.0821 L·atm·K−1·mol−1. Therefore the molar amount is about 0.089 mol.
Which real-life scenario best illustrates Charles's law?
Nitrogen and oxygen pressures adding in air
A hot air balloon rises when the air inside is heated
The rate of diffusion of gases
A sealed syringe changes pressure when compressed
Charles's law describes how gas volume increases with temperature at constant pressure. Heating the air inside a balloon causes it to expand and become buoyant. Therefore, the hot air balloon example fits Charles's law.
In a container, gas A has a partial pressure of 200 mmHg and gas B has a partial pressure of 300 mmHg. What is the total pressure according to Dalton's law?
600 mmHg
100 mmHg
500 mmHg
200 mmHg
Dalton's law of partial pressures states that total pressure is the sum of partial pressures of each gas. Adding 200 mmHg and 300 mmHg gives a total of 500 mmHg. Therefore, the total pressure is 500 mmHg.
A mixture contains nitrogen at 600 mmHg and oxygen at 200 mmHg in a closed container. What is the total pressure of the gas mixture?
800 mmHg
400 mmHg
600 mmHg
200 mmHg
According to Dalton's law, the total pressure is the sum of the partial pressures. Summing 600 mmHg and 200 mmHg yields 800 mmHg. Therefore, the total pressure is 800 mmHg.
How many liters does 10.0 g of helium occupy at 1.0 atm and 25°C? (Molar mass of He = 4.00 g·mol−1, R = 0.0821 L·atm·K−1·mol−1)
5.42 L
61.2 L
33.6 L
12.3 L
First calculate moles: n = 10.0 g / 4.00 g·mol−1 = 2.50 mol. Then use PV = nRT: V = nRT / P = (2.50 × 0.0821 × 298 K) / 1.0 atm ≈ 61.2 L. Therefore, the volume is approximately 61.2 L.
A gas sample is at 1.0 atm, 8.0 L, and 300 K. Its pressure is increased to 3.0 atm and volume to 5.0 L. Using the combined gas law, what is the new temperature?
150 K
562.5 K
450 K
300 K
Using P1V1/T1 = P2V2/T2, rearrange to T2 = T1 × (P2V2) / (P1V1) = 300 K × (3.0 atm × 5.0 L) / (1.0 atm × 8.0 L) ≈ 562.5 K. Therefore, the new temperature is about 562.5 K.
Under which conditions does a real gas deviate most from ideal behavior?
High pressure and high temperature
Low pressure and high temperature
Low pressure and low temperature
High pressure and low temperature
Real gases deviate from ideal behavior when intermolecular forces and molecular volumes become significant. These effects are strongest at high pressures and low temperatures. Therefore, under those conditions a gas behaves least ideally.
A car tire is inflated to 35.0 psi at 25°C. If the temperature rises to 45°C with constant tire volume, what is the new pressure? (Assume ideal behavior)
37.3 psi
33.0 psi
35.0 psi
40.0 psi
Using Gay-Lussac's law (P1/T1 = P2/T2), convert temperatures to Kelvin: 298 K and 318 K. Then P2 = 35.0 psi × (318/298) ≈ 37.3 psi. Therefore, the pressure increases to about 37.3 psi.
In a gas mixture at 10.0 atm, the mole fraction of gas A is 0.20. What is the partial pressure of gas A?
0.20 atm
8.0 atm
5.0 atm
2.0 atm
Dalton's law relates partial pressure to mole fraction: P_A = X_A × P_total = 0.20 × 10.0 atm = 2.0 atm. Therefore, the partial pressure of gas A is 2.0 atm.
In the van der Waals equation (P + a(n/V)^2)(V − nb) = nRT, what does the constant a represent?
The magnitude of intermolecular attractive forces
The effective volume occupied by gas particles
The absolute temperature at which gas condenses
The ideal gas constant
In the van der Waals equation, the a term corrects for intermolecular attractions that lower the pressure. A larger a indicates stronger attractive forces. Therefore, a quantifies the magnitude of those forces.
Using the van der Waals constants for CO2 (a = 3.59 L^2·atm·mol−2, b = 0.0427 L·mol−1), what is the approximate volume of 1.00 mol of CO2 at 1.00 atm and 273 K?
25.00 L
22.29 L
22.41 L
20.00 L
Applying the van der Waals equation and solving iteratively gives a volume slightly below the ideal value of 22.41 L. The correction yields ≈22.29 L. Therefore, the real gas occupies about 22.29 L under these conditions.
Hydrogen gas collected over water has a total pressure of 1.00 atm, and the water vapor pressure at that temperature is 0.03 atm. What is the pressure of the dry hydrogen gas?
0.97 atm
0.03 atm
1.00 atm
1.03 atm
When collecting gas over water, Dalton's law dictates that the total pressure is the sum of the gas and water vapor pressures. Subtracting the water vapor pressure yields 1.00 atm − 0.03 atm = 0.97 atm. Therefore, the dry hydrogen pressure is 0.97 atm.
At the same temperature, which of the following gases has the highest root mean square speed?
N2
CO2
H2
O2
The root mean square speed is inversely proportional to the square root of molar mass. H2 has the lowest molar mass among the options, so its molecules move fastest. Therefore, H2 has the highest rms speed.
The compressibility factor Z = PV/(nRT) for a gas is observed to be less than 1. What does this indicate about the gas behavior?
The gas behaves ideally
Intermolecular attractions dominate, making the gas more compressible than ideal
Intermolecular repulsions dominate, making the gas less compressible
The temperature is above the critical temperature
A Z value below 1 indicates that attractive forces between molecules cause the gas to occupy less volume than predicted by the ideal gas law. This makes the gas more compressible. Therefore, dominant attractions cause the deviation.
0
{"name":"A gas occupies 4.0 L at 1.0 atm and constant temperature. According to Boyle's law, what volume will it occupy at 2.0 atm?", "url":"https://www.quiz-maker.com/QPREVIEW","txt":"A gas occupies 4.0 L at 1.0 atm and constant temperature. According to Boyle's law, what volume will it occupy at 2.0 atm?, A gas has a volume of 2.0 L at 300 K and constant pressure. According to Charles's law, what will its volume be at 600 K?, Which gas law describes the direct proportionality between pressure and temperature for a fixed volume of gas?","img":"https://www.quiz-maker.com/3012/images/ogquiz.png"}

Learning Outcomes

  1. Analyse relationships between pressure, volume, and temperature using gas laws
  2. Calculate changes in gas behavior with combined law equations
  3. Identify real-life applications of Boyle's, Charles's, and Avogadro's laws
  4. Apply the ideal gas law to determine unknown variables
  5. Demonstrate understanding of partial pressures with Dalton's law
  6. Evaluate deviations from ideal behavior in real gases

Cheat Sheet

  1. Boyle's Law: Pressure-Volume Relationship - Boyle's Law states that at a constant temperature, pressure and volume of a gas are inversely related: squeeze it and the volume shrinks. This principle explains why syringes draw in and push out fluids so smoothly and why deep-sea divers must adjust their gauges. It's a cornerstone in understanding how engines and lungs work. GeeksforGeeks Gas Laws
  2. Charles's Law: Temperature-Volume Relationship - Charles's Law tells us that at constant pressure, a gas expands when heated and contracts when cooled, directly proportional to its absolute temperature. This is the magic behind hot air balloons rising as the air inside warms up. Remember to use Kelvin so you don't end up with negative volumes! GeeksforGeeks Gas Laws
  3. Gay-Lussac's Law: Temperature-Pressure Relationship - Gay-Lussac's Law reveals that at constant volume, pressure increases linearly with temperature. Ever wondered why an aerosol can might burst in a hot car? This law explains it! It also guides safety limits in pressure cookers and industrial reactors. GeeksforGeeks Gas Laws
  4. Avogadro's Law: Volume and Moles Relationship - Avogadro's Law asserts that at constant temperature and pressure, equal volumes of gases contain the same number of molecules. Doubling the moles doubles the volume, which is why 1 mole of any gas occupies about 22.4 L at STP. It helps chemists predict yields in reactions. Avogadro's Law Wiki
  5. Combined Gas Law: Integrating Boyle's, Charles's, and Gay-Lussac's Laws - The Combined Gas Law merges Boyle's, Charles's, and Gay-Lussac's laws into one handy equation: (P₝V₝)/T₝ = (P₂V₂)/T₂. Use it whenever pressure, volume, and temperature all shift, like in scuba diving gear or tire inflation on a hot day. Always convert to Kelvin! Pearson Combined Gas Law
  6. Ideal Gas Law: Relating Pressure, Volume, Temperature, and Moles - The Ideal Gas Law, PV = nRT, ties together pressure, volume, number of moles, and temperature with the gas constant R. It lets you calculate any one variable if you know the other three, making it a chemist's best friend. Real gases follow it closely under many conditions. GeeksforGeeks Gas Laws
  7. Dalton's Law of Partial Pressures - Dalton's Law states that in a mixture of non-reacting gases, total pressure equals the sum of each gas's partial pressure. This is crucial for calculating breathing gas mixes in diving and understanding air composition. It also explains why carbonated drinks fizz when opened. Dalton's Law Wiki
  8. Real-Life Applications of Gas Laws - Gas laws govern everything from how your lungs inflate (Boyle's Law) to the lift behind hot air balloons (Charles's Law) and the behavior of car engines (Ideal Gas Law). Engineers, doctors, and meteorologists all rely on these principles daily. Seeing them in action makes study feel like a real-world scavenger hunt! GeeksforGeeks Gas Laws
  9. Deviations from Ideal Gas Behavior - Real gases deviate from the Ideal Gas Law at high pressures and low temperatures because molecules occupy space and attract each other. The Van der Waals equation adds correction factors to R and V, giving a more accurate picture of real-world behavior. This matters in high-pressure industrial processes. GeeksforGeeks Gas Laws
  10. Importance of Temperature in Kelvin - Always convert temperatures to the Kelvin scale when using gas laws, since it starts at absolute zero where molecular motion ceases. Simply add 273.15 to a Celsius reading to avoid negative values and maintain true proportionality. This small step keeps your calculations spot-on. Kelvin Scale Wiki
Make a Quiz (FREE) Copy & Edit This Quiz Create a Quiz with AI

Education Quizzes

Powered by: Quiz Maker