Gas Laws

Question 1

What did Boyle discover

Answer 1

Pressure-volume relationship

For a given mass of a gas at a constant temperature, the volume of a gas varies inversely with pressure

Question 2

What did Charles discover

Answer 2

Temperature and volume of a gas at constant pressure
For a given mass of a gas at a constant pressure, the volume of the gas is directly proportional to its temperature in Kelvin

Question 3

What did Gay-Lussac discover

Answer 3

Temperature and pressure
For a given volume of gas, as the temperature of an enclosed gas increases, the pressure of a gas is directly proportional

Question 4

Combined gas law

Answer 4

Relationship between temperature, pressure, and volume of a gas

Question 5

True or false: Boyle’s law states that pressure is inversely proportional to volume

Answer 5

True

Question 6

True or false: Charle’s law states that volume and temperature are directly proportional

Answer 6

True

Question 7

True or false: Gay-Lussac’s law states that pressure and temperature are directly proportional

Answer 7

True

Question 8

True or false: If the pressure is increased by a factor of 3 times then the volume will increase by a factor of 2 times

Answer 8

False

Question 9

True or false: If the temperature is increased by a factor of 2 times then the pressure will increase by a factor of 2 times

Answer 9

True

Question 10

True or false: Decreasing the volume of a container by 1/2 will double the pressure

Answer 10

True

Question 11

True or false: A graph of volume vs. temperature will produce a curve

Answer 11

False

Question 12

True or false: A graph of an inversely proportional relationship will produce a straight line

Answer 12

False

Question 13

True or false: When steam condenses in a closed container a partial vacuum is created

Answer 13

True

Question 14

True or false: A balloon placed in cold water will increase in volume

Answer 14

False

Question 15

Kinetic Theory of Matter

Answer 15

All particles of matter are in constant motion

Question 16

How does the Kinetic Theory of Matter work for solids

Answer 16

Particles are moving so so so slowly it is practically impossible to see

Question 17

Gases are made up of

Answer 17

Tiny particles of negligible volume (very very small)

Question 18

Random walk definition

Answer 18

Gas particles move in a straight line until they hit something and then change direction

Question 19

All collisions between gas particles are

Answer 19

Elastic

Question 20

Elastic definition

Answer 20

The gas particles do not stick together when they collide

Question 21

Can KE be transferred?

Answer 21

Yes but it cannot be lost

Question 22

As the number of collisions increase

Answer 22

Pressure increases

Question 23

How will the collisions increase

Answer 23

More particles

Increase in temperature causes more frequent collisions of gas particles with other gas particles and walls

Question 24

Name of a space with no gas pressure

Answer 24

Vacuum

Question 25

Definition of ideal gases

Answer 25

Gases that follow all rules of the kinetic molecular theory

Question 26

What did Dalton discover

Answer 26

Gas pressure depends on the amount of gas and the average kinetic energy of its particles Total pressure of a mixture of gases is = to the sum of its individual partial pressures

Question 27

What did Graham discover

Answer 27

Diffusion and effusion | The rate of effusion of a gas is inversely proportional to the square root of the the gas' molar mass

Question 28

Diffusion definition

Answer 28

The tendency of gas particles to spontaneously spread out until uniformly distributed

Question 29

Effusion definition

Answer 29

The escape of a gas through a tiny pinhole in a container of gas

Question 30

An ideal gas has

Answer 30

No molecular volume, no attractive forces

Question 31

In reality are ideal gases real

Answer 31

There are no perfectly ideal gases but under most conditions, real gases will mostly act like ideal gases

Question 32

When do gases not act like ideal gases

Answer 32

High pressure, low temperature, high molar mass, and polar molecules