Chapter 13.1 And 14 Vocab and Key Concepts

Question 0

Kinetic theory

Answer 0

All matter consists of tiny particles that are in constant motion

Question 1

Kinetic energy

Answer 1

The energy an object has because of it’s motion

Question 2

Gas pressure

Answer 2

Results from the force exerted by a gas per unit surface area of an object

Question 3

Vacuum

Answer 3

An empty space with no particles and no pressure

Question 4

Atmospheric pressure

Answer 4

Results from the collisions of atoms and molecules in air with objects

Question 5

Barometer

Answer 5

A device that is used to measure atmospheric pressure

Question 6

Pascal (Pa)

Answer 6

The SI unit of pressure

Question 7

Standard atmosphere (atm)

Answer 7

The pressure required to support 760mm of mercury in a mercury barometer at 25degreesC

Question 8

What is the numerical relationship converting atm?

Answer 8

1 atm = 760 mm Hg = 101.3 kPa

Question 9

Briefly describe the assumptions of kinetic theory as applied to gases.

Answer 9

• The particles in a gas are considered to be small, hard spheres with an insignificant volume
• The motion of the particles in a gas is rapid, constant, and random
• All collisions between particles in a gas are perfectly elastic

Question 10

Use kinetic theory to explain what causes gas pressure.

Answer 10

Gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a gas with an object

Question 11

How is Kelvin temperature of a substance related to the average kinetic energy of its particles?

Answer 11

The Kelvin temperature of a substance is directly proportional to the average kinetic energy of the particles of the substance

Question 12

Compressibility

Answer 12

A measure of how much the volume of matter decreases under pressure

Question 13

Ideal gas constant

Answer 13

(R) has the value 8.31 (L•kPa)/(K•mol)

Question 14

Ideal gas law

Answer 14

The gas law that includes all 4 variables - P, V, T, and n

Equation: PV=nRT

Question 15

Partial pressure

Answer 15

The contribution each gas in a mixture makes to the total pressure is called this exerted by that gas

Question 16

Dalton’s law of partial pressures

Answer 16

States that, at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

Question 17

Diffusion

Answer 17

The tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout

Question 18

Effusion

Answer 18

A gas escapes through a tiny hole in its container

Question 19

Why is a gas easy to compress?

Answer 19

The space between the particles in a gas

Question 20

List three factors that can affect gas pressure.

Answer 20

The amount of gas, volume, and temperature

Question 21

How are the pressure and volume of a gas related at a constant temperature?

Answer 21

If the temperature is constant, as the pressure of a gas increases, the volume decreases

Question 22

If pressure is constant, how does a change in temperature affect the volume of a gas?

Answer 22

If pressure is constant, as the temperature of an enclosed gas increases, the volume increases

Question 23

What is the relationship between the temperature and pressure of a contained gas at constant volume?

Answer 23

As the temperature of an enclosed gas increases, the pressure increases, if the volume is constant

Question 24

In what situations is the combined gas law useful?

Answer 24

It allows you to do calculations for situations in which only the amount of gas is constant

Question 25

What do you need to calculate the amount of gas in a sample at given conditions of temperature, pressure, and volume?

Answer 25

To calculate the number of moles of a contained gas requires an expression that contains the variable n

Question 26

Under what conditions do real gases deviate most from ideal behavior?

Answer 26

At low temperatures and high pressures

Question 27

In a mixture of gases, how is the total pressure determined?

Answer 27

It is the sum of the partial pressures of the gases

Question 28

What is the effect of molar mass on rates of diffusion and effusion?

Answer 28

Gases of a lower mass diffuse an effuse faster than gases of higher molar mass

Question 29

Equation for ideal gas law

Answer 29

PV=nRT

Question 30

Equation converting Celsius to kelvin

Answer 30

K= degrees C + 273

Question 31

Equation for circumference

Answer 31

C=2pi r

Question 32

Equation for volume

Answer 32

V= 4/3 pi r^3

Question 33

Conversion between mili- and normal

Answer 33

1000mm=1m

Question 34

Conversion from normal to kilo-

Answer 34

1000m=1km

Question 35

Equation for Dalton's law of partial pressures

Answer 35

P total = P1 + P2 + P3 + .....