Unit 8 (chapter 13)

Question 1

Absolute temperature

Question 2

amount of gas

Question 3

Avogadro’s number

Question 4

Boyle’s law

Question 5

Charles’ law

Answer 5

When the amount and pressure of a gas are held constant, the volume and Kelvin temperature are directly proportional

Question 6

Combined Gas Law

Question 7

Dalton’s Law

Answer 7

For a mixture of gases in a container, the total pressure exerted is the sum of the partial pressures of the gases present

Question 8

Gay-Lussac’s Law

Answer 8

When the amount and volume of a gas are held constant, the pressure and Kelvin temperature are directly proportional

Question 9

ideal gas

Answer 9

a gas that follows the kinetic molecular theory completely

Question 10

Ideal Gas Law

Question 11

kinetic molecular theory

Answer 11

A set of rules on how we expect gases to behave
- Gases consist of very small particles that are far apart relative to their size (mostly empty space)
- Gas particles are in constant, random motion. The moving particles constantly collide with each other and the walls of the container
- Collisions between gas particles and container walls are elastic collisions
- There are no forces of attraction or repulsion between gas particles (will not clump or repel because they’re moving too fast)
- The average kinetic energy of gas particles depends on the gas temperature (hotter = faster)

Question 12

partial pressure

Answer 12

the pressure that the gas would exert if it were alone

Question 13

pressure

Question 14

standard pressure

Answer 14

air pressure of dry air at sea level

Question 15

standard temperature

Answer 15

273K

Question 16

temperature

Question 17

volume

Question 18

kinetic energy

Answer 18

energy anything has if it’s moving. moving faster means more energy
Average kinetic energy is directly proportional to Kelvin temperature

Question 19

solids kinetic energy

Answer 19

very little

Question 20

liquids kinetic energy

Answer 20

more than solids

Question 21

gases kinetic energy

Answer 21

lots, in constant motion. 1000mph at STP

Question 22

Inelastic collisions

Answer 22

kinetic energy disappears (ex: slime balls hitting each other)

Question 23

Elastic collisions

Answer 23

Bounces right back, no kinetic energy waster (ex: rubber balls hitting each other)

Question 24

Expandability

Answer 24

If an open container had gas, the fas would leave the container and fill any given area (unique to gases)

Question 25

Diffusion

Answer 25

The process of gases moving around (ex: movie theater popcorn smell filling a mall) (unique to gases)

Question 26

Compressibility

Answer 26

Because there’s so much empty space in gases, you can squeeze them into very small spaces (unique to gases)

Question 27

SI unit for pressure

Answer 27

Pa

Question 28

Atmospheric pressure & gravity

Answer 28

atmospheric pressure changes with elevation (gravity)

Question 29

conversion factors (mm Hg)

Answer 29

1 standard atmosphere = 1.000 atm = 760.0 mm Hg = 760.0 torr

Question 30

conversion factors (Pa)

Answer 30

1 standard atmosphere = 101,325 Pa

Question 31

conversion factors (psi)

Answer 31

1.000 atm = 14.69 psi

Question 32

To fully describe a gas…

Answer 32

you need to know
- temperature (T)- K or °C (standard T=273K)
- volume (V)- L or mL
- pressure (P)
- amount (n)- mol

Question 33

Avogadro’s Law

Answer 33

for a gas at a constant temperature and pressure, the volume is directly proportional to the number of moles