Kinetic Molecular Theory and sample TEST questions

Kinetic Molecular Theory ... 6 things

Kinetic Molecular Theory (long version) The experimental observations about the behavior of gases can be explained with a simple theoretical model known as the kinetic molecular theory. This theory is based on the following postulates, or assumptions. 1. Gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion. 2. These particles are much smaller than the distance between particles. Most of the volume of a gas is therefore empty space. 3. These particles move in a straight line until they collide with another particle or the walls of the container. 4. There is no force of attraction between gas particles or between the particles and the walls of the container. 5. Collisions between gas particles or collisions with the walls of the container are perfectly elastic. None of the energy of a gas particle is lost when it collides with another particle or with the walls of the container. ELASTIC = NO energy lost 6. The average kinetic energy of a collection of gas particles depends on the temperature of the gas and nothing else. The kinetic molecular theory can be used to explain each of the experimentally determined gas laws. (see the formula bar on the bottom of your Table of Elements ... lower left hand side)

Kinetic Molecular Theory Sample Test Question 3 According to the Kinetic Molecular Theory, collisions between molecules in a gas a. are inelastic b. are perfectly elastic c. cause a loss of total kinetic energy d. never occur

b. are perfectly elastic

Kinetic Molecular Theory Sample Test Question 1 The Kinetic Molecular Theory of gases assumes that the particles of an ideal gas are separated by great distances. This implies that the gas particles are considered to have no definite: a. mass b. volume c. density d. energy

b. volume

Kinetic Molecular Theory Sample Test Question 4 What happens to the average kinetic energy of the particles in a sample of gas as the temperature of the sample is increased? a. the average kinetic energy does not change b. The change in average kinetic energy cannot be determined c. The average kinetic energy decreases d. The average kinetic energy increases

d. The average kinetic energy increases

Kinetic Molecular Theory Sample Test Question 6 Which of the following is NOT an assumption of kinetic molecular theory a. average kinetic energy of the gas particles is proportional to the temperature b. gas particles do not attract or repel each other c. actual volume of gas particles is effectively zero d. collisions between gas particles (and container walls) are inelastic

d. collisions between gas particles (and container walls) are inelastic

Kinetic Molecular Theory Sample Test Question 2 According to the Kinetic Molecular Theory, particles of an ideal gas a. attract each other but do not collide b. repel each other and collide c. collide but do not attract each other d. do not collide and do not attract or repel each other.

d. do not collide and do not attract or repel each other.

Kinetic Molecular Theory Sample Test Question 5 What causes gas pressure in a container such as a helium balloon? a. atmospheric pressure acting on the outside walls of the container b. the walls of the container c. the vacuum maintained in the container d. the simultaneous collisions of fast moving particles in the container

d. the simultaneous collisions of fast moving particles in the container

Kinetic Molecular Theory (easy summary) 6 things

Kinetic Molecular Theory (easy summary) 1. Gas particles are in constant rapid motion. 2. Gas particles are separated by relatively large distances...gases particles themselves have basically no volume. 3. Gas particles move in straight line 4. Gas particles have no attractive or repulsive forces between them. 5. When gas particles collide, they do not transfer kinetic energy to what they collide with ... therefore NO energy is lost = Perfectly ELASTIC collisions 6. The average kinetic energy (average velocity) of a gas is dependent on the temperature of the gas. Directly Proportional ... increase in temp = increase in avg kinetic energy