Boyle's Law And Ideal Gases

Question 1

Definition of ideal gas

Answer 1

A gas in which all collisions between particles are perfectly elastic and in which no IMF exists

Question 2

Definition of a real gas

Answer 2

A gas that deviates from ideal gas behaviour under certain conditions

Question 3

What does it mean for a collision to be elastic?

Answer 3

No energy gets lost in the collision

Question 4

What does the average kinetic energy depend on?

Answer 4

Temperature

Question 5

Describe the particles in solids

Answer 5

Particles are close together and exhibit vibratory motion

Question 6

Describe the particles in liquids

Answer 6

Particles are further apart and freer to move. They can vibrate, spin, and move from place to place. Diffusion can take place.

Question 7

Describe the particles in gases

Answer 7

Spaces between particles are large and can be compressed. Molecules bump into each other, and the walls of the container, creating a pressure that acts in all directions

Question 8

Definition of diffusion

Answer 8

Particles of one gas spreading through another gas (occurs in liquids too)

Question 9

Conditions that real gases behave most like an ideal gas

Answer 9

• high temperatures
• low pressures

Question 10

Assumptions about ideal gases

Answer 10

• gases are made up of particles that are smaller than the spaces between them (essentially points in space)
• all collisions are elastic (no energy is lost)
• all particles have different amounts of energy, but the average kinetic energy depends on the temperature
• IMF are basically nonexistent
• an increase in temperature will result in an increase in kinetic energy of particles

Question 11

Define boyle’s law

Answer 11

For a fixed amount of gas at constant temperature, pressure is inversely proportional to volume