FREE! Click here to Join FunTrivia. Thousands of games, quizzes, and lots more!
Quiz about Kinetic Theory of Gases and Related Laws
Quiz about Kinetic Theory of Gases and Related Laws

Kinetic Theory of Gases and Related Laws Quiz


This quiz will test your understanding of the gas laws you may have studied in either chemistry or physics. A couple or more numerical problems are included, so a pen and and paper may be handy.

A multiple-choice quiz by pokho. Estimated time: 5 mins.
  1. Home
  2. »
  3. Quizzes
  4. »
  5. Science Trivia
  6. »
  7. Physics
  8. »
  9. Laws and Theories of Physics

Author
pokho
Time
5 mins
Type
Multiple Choice
Quiz #
398,213
Updated
Dec 03 21
# Qns
10
Difficulty
Tough
Avg Score
6 / 10
Plays
179
-
Question 1 of 10
1. Gases are generally more compressible than solids and liquids.


Question 2 of 10
2. Perhaps the best known equation pertaining to the gas laws is the ideal gas equation. Which of the following laws may NOT be required to derive the ideal gas equation? Hint


Question 3 of 10
3. Which of the following is NOT one of the postulates of the kinetic theory of gases? Hint


Question 4 of 10
4. You have a gas 'A' at pressure k in a container. You have another gas 'B' at pressure 2k in another container, which has only half the volume of the one containing gas A. If both the containers are mixed together, what is the pressure given that the two gases don't react? Hint


Question 5 of 10
5. At the same conditions of temperature and pressure, which of the following gases will diffuse the fastest? Hint


Question 6 of 10
6. Certain assumptions in the kinetic theory of gases have been found to be fallacious through experimentation. This results in differences between the behavior of real gases and the ideal gas, barring certain conditions. Which is NOT a fallacious assumption? Hint


Question 7 of 10
7. While learning thermal physics and thermochemistry, you are sure to encounter the Maxwell-Boltzmann distribution graph. What does the peak of the curve represent? Hint


Question 8 of 10
8. Real gases behave differently from ideal gases. Which scientist is credited with making adjustments accordingly and formulating the 'real gas' equation named for him? Hint


Question 9 of 10
9. At conditions of standard temperature and pressure (STP ), which of these has the highest mass? (Remember that each of these consist of diatomic molecules) Hint


Question 10 of 10
10. With the number of molecules staying the same, an ideal gas is heated until it is twice the original temperature and the pressure is doubled as well. What happens to the volume of the gas? Hint



(Optional) Create a Free FunTrivia ID to save the points you are about to earn:

arrow Select a User ID:
arrow Choose a Password:
arrow Your Email:




Most Recent Scores
Mar 17 2024 : Guest 75: 2/10
Feb 01 2024 : Guest 172: 2/10

Quiz Answer Key and Fun Facts
1. Gases are generally more compressible than solids and liquids.

Answer: True

Solids possess the least compressibility and thermal expansion, liquids have more, and gases the most.

Many of the beginner fluid and classical mechanics' equations overlook compressibility in solids and liquids as being negligible.
2. Perhaps the best known equation pertaining to the gas laws is the ideal gas equation. Which of the following laws may NOT be required to derive the ideal gas equation?

Answer: Graham's Law of Effusion

The gas law not mentioned here but also useful for the cause, is Gay-Lussac's Law. This establishes that the pressure of a given mass of gas is directly proportional to its temperature in the KELVIN scale, or P/T = k.

Boyle's Law establishes that the pressure of a gas at a given temperature is inversely proportional to the volume of the gas, or PV = k.

Charles' Law establishes that the volume of a gas is directly proportional to the temperature of the concerned gas in Kelvins, or V/T = k.

We can easily derive the ideal gas equation hence, PV = nRT, where R is the universal gas constant. These gas laws form the basis of kinetic gas theory as well.
3. Which of the following is NOT one of the postulates of the kinetic theory of gases?

Answer: All gaseous molecules move towards the walls of the container

On the contrary, the postulates of the kinetic theory of gases state that each gas molecule moves randomly, causing it to be also called the 'Dynamic Particle Theory'. It also states that the pressure of a gas is derived from the gaseous molecules colliding with the walls of a container.

From these postulates, the kinetic gas equation is derived:

Pv = (mnc^2)/3

where P is the pressure of the gas, V the volume, m mass of each gaseous molecule, n the total number of molecules and c the Root Mean Square speed of the gas.
4. You have a gas 'A' at pressure k in a container. You have another gas 'B' at pressure 2k in another container, which has only half the volume of the one containing gas A. If both the containers are mixed together, what is the pressure given that the two gases don't react?

Answer: 4k/3

To solve this question, you can apply Dalton's Law of Partial Pressures, which states that if you mix two such gases that do not react with each other, the total pressure exerted is equal to the sum of the partial pressures of the respective gases mixed together.

A partial pressure is the amount of pressure the gas would exert when occupying the new volume. This may be found by using Boyle's law.
5. At the same conditions of temperature and pressure, which of the following gases will diffuse the fastest?

Answer: Hydrogen

According to Graham's law of effusion/diffusion, the rate of diffusion/effusion of gases is inversely proportional to the square root of the respective densities of the gases.

Hydrogen is the lightest gas among the four listed, and in fact among all the gases, and hence has the quickest rate of diffusion.
6. Certain assumptions in the kinetic theory of gases have been found to be fallacious through experimentation. This results in differences between the behavior of real gases and the ideal gas, barring certain conditions. Which is NOT a fallacious assumption?

Answer: Gaseous molecules move randomly in all directions

It must be noted that ideal gases are 'ideal and hypothetical' - and may not be very accurate when gases are actually modelled experimentally. It was observed through experimental results that pressure-volume graphs weren't a straight line, but instead a curve.

Deviations caused by the factors in the answer options are higher in gases that can be liquefied or are soluble in water. In such gases, the molecules tend to be closer together, increasing deviations caused by attraction or repulsion between them.

These faulty assumptions have the least effect when the pressure is low and the temperature is high. However, under high pressure and at low temperature, the molecules come closer - due to which the intermolecular forces of attraction and repulsion between molecules may not be negligible anymore, and neither will be the volume of the gas compared to the volume occupied by its molecules.

The extent of deviations from ideal gas behaviour is measured by the quantity Z, or compressibility factor, represented by z = (PV)/(NRT).

For an ideal gas , the value of Z is 1. If the value of Z is less than 1, negative deviation has been shown and the gas is more compressible than expected behavior. If the value of Z is more than 1, positive deviation has been shown and the gas is less compressible than expected behavior.
Noted as 'certain conditions' in the question, real gases do act like ideal gases at a certain temperature and Z =1. This temperature is known as the Boyle's Point of the concerned gas.
7. While learning thermal physics and thermochemistry, you are sure to encounter the Maxwell-Boltzmann distribution graph. What does the peak of the curve represent?

Answer: Most probable speed

The y-axis represents the number of molecules and the x-axis represents the molecular speed. Consequently , the x-coordinate at the peak would show the speed at which you will find the maximum amount of molecules.

The most probable speed can be found by using the following formula:

c* = square root of ( 2*R*T/M) where R is the universal gas constant, T is the temperature and M is the molar mass of the gas species concerned.
8. Real gases behave differently from ideal gases. Which scientist is credited with making adjustments accordingly and formulating the 'real gas' equation named for him?

Answer: Van Der Waals

The Dutch physicist J.D. Van Der Waals won his Nobel Prize in 1910 for these advancements.

This is the modified Van Der Waals' equation:

(P + an^2/V^2)(V-nb) = nRT

The constant 'a' corrects for differing intermolecular forces of attraction while 'b' corrects for the effective size of the molecules. (Its value is four times the actual volume of the molecules).

The values of these constants vary according to the nature of the gas.
9. At conditions of standard temperature and pressure (STP ), which of these has the highest mass? (Remember that each of these consist of diatomic molecules)

Answer: 22.4 L of chlorine

At conditions of STP ( 273 Kelvin temperature and 1 atmosphere pressure) , one mole of any gas has a volume of 22.4 L. (You can always find it using the ideal gas equation if you don't remember.)

The mass of 22.4 L of chlorine = mass of 1 mol of chlorine = 35.5 g
Mass of 89.6 L of hydrogen gas = mass of 4 mol of hydrogen gas = 16 g
Mass of oxygen is directly given -> 30 g
Mass of 1.5 mol of fluorine gas = 1.5 * 19 = 28.5 g
10. With the number of molecules staying the same, an ideal gas is heated until it is twice the original temperature and the pressure is doubled as well. What happens to the volume of the gas?

Answer: It stays the same

This question requires the application of the combined gas law. Since 'n' remains equal and R is a constant, we can bring it down to this equation:

Initial Pressure * Initial Volume/ Initial temperature = Final Pressure * Final Volume/ Final temperature

Given that final temperature = 2 * initial temperature and final pressure = 2 * initial pressure, the required ratio may be found using appropriate substitution in the given equation.
Source: Author pokho

This quiz was reviewed by FunTrivia editor rossian before going online.
Any errors found in FunTrivia content are routinely corrected through our feedback system.
Related Quizzes
1. Laws in Physics Average
2. Wave Laws in Physics Average
3. Ohm's Lore Average
4. Gas Laws Average
5. Who Needs Airbags? Average
6. Gases Are All Around Us! Tough
7. Replace Those Units! Tough
8. Relativity From a Relative Layman Tough
9. Theories of Matter Difficult
10. Physics - Unit By Unit! Easier
11. The Physics of Football Average
12. Tabula Rosy's Learning Lab Average

3/28/2024, Copyright 2024 FunTrivia, Inc. - Report an Error / Contact Us