Week 4: Thermodynamic Properties II

Question 1

Define Boyle’s Law

Answer 1

When temperature is constant, pressure increases while volume decreases. Pressure and volume are inversely proportional.

Question 2

Define Charles’s Law

Answer 2

When pressure is constant, temperature and volume increase. Temperature and volume are directly proportional.

Question 3

Define Gay-Lussac’s Law

Answer 3

When volume is constant, pressure and temperature increase. Pressure and temperature are directly proportional.

Question 4

Ideal Gas Equation

Answer 4

Pv = RT

Question 5

When does the ideal gas equation fail?

Answer 5

1. High pressures.
2. Low temperatures.

Question 6

Kinetic Theory of Gases

Answer 6

A statistical analysis of gases of how individual molecules move as a whole which has come up with a very similar result as the experimentally demonstrated ideal gas equation.

Question 7

Six assumptions of the kinetic theory of gases:

Answer 7

1. The average distance separating the gas particles (i.e. their mean free path length between collisions) is large compared to their size.
2. The particles have the same mass.
3. The number of particles is so large that statistical treatment can be applied.
4. The particles are in constant, random, and rapid motion.
5. Except during collisions, the interactions among particles are negligible.
6. The average kinetic energy of the gas particles depends only on the absolute temperature of the system.

Question 8

What is the purpose of the compressibility factor?

Answer 8

To correct the ideal gas equation and expand its use into areas such as high pressure and low temperature regions where it originally breaks down.

Question 9

Compressibility Factor Equation

Answer 9

Z = Pv/RT

Question 10

Corrected Ideal Gas Equation

Answer 10

Pv = ZRT