Kinetic molecular theory of gases inquiry PDF

Preview

Summary

Download Kinetic molecular theory of gases inquiry PDF

Description

Lucid - Assessment Content

Lucid ©2000-2006 Kinetic Molecular Theory of Gases Inquiry Exercises Problems Summary Page Course Home Logout

11/3/20, 12 :34 AM

MODEL: POSTULATES OF THE KINETIC MOLECULAR THEORY 1. The volume of individual molecules in a gas is negligible because their size is very much smaller than the distance between them. 2. Gas molecules move constantly and randomly through the volume of the container they occupy at various speeds and in every direction. 3. The forces of attraction and repulsion between molecules in a gas are negligible except when they collide with each other.

Key Questions 1. According to the kinetic molecular theory, what assumptions are made regarding the size of the molecules in a gas? The size is smaller than the distance between them.

4. Gas molecules continually collide with each other and with the walls of the container. The collisions are elastic, which means that the total translational kinetic energy of the colliding molecules does not change. 5. The average kinetic energy of the gas molecules, , is proportional to the absolute temperature of the gas. Specifically, using M = molar mass, = mean 2. According to the kinetic molecular theory, what square molecular speed, R = gas constant, and T = Kelvin temperature: assumptions are made regarding the interactions = 1/2 M = 3/2 RT between molecules in a gas? They continuously collide with each other and the walls of the container.

3. According to the kinetic molecular theory, are collisions between molecules visualized more like collisions between sponge balls or collisions between bowling balls? Explain. Sponge balls because the collisions are elastic.

4. According to kinetic molecular theory, what information would you need to calculate the mean square molecular speed of a pure substance in the gas phase? T - temperature, molar mass in kg/mol

5. How can the postulates of the kinetic molecular theory be used to explain the ideal gas law, i.e., that the pressure of a gas is inversely proportional to the volume of the container (V) and is directly proportional to the number of molecules (n) and the product of temperature and gas constant (RT)? PV = nRT 1x1=1x1x1 V x 2 = 1 x 1 x 1 (0.5) PV = nRT 1x1=1x1x1 Vx1=2x2x2 V = 6. Pressure is determined by the

https://lucid.chem.sunysb.edu/Lucid/assessment/assessment.jsp?&&seq=1&

Page 1 of 2

Lucid - Assessment Content

https://lucid.chem.sunysb.edu/Lucid/assessment/assessment.jsp?&&seq=1&

11/3/20, 12 :34 AM

Page 2 of 2...