13.1 and 14

Question 0

2 extra points about kinetic theory of gases

Answer 0

random walk

no repulsive or attractive forces

Question 1

3 assumptions in kinetic theory of gases

Answer 1

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 2

3 units of pressure

Answer 2

pascal
atm - standard atmosphere
millimeters of Hg - mm Hg

Question 3

which unit of pressure is SI

Answer 3

kPa

Question 4

what causes pressure

Answer 4

simultaneous collisions of billions of rapidly moving particles in a gas with an object

Question 5

What is STP

Answer 5

standard temperature and pressure
0 degrees C
101.3 kPa
1 atm

Question 6

What is the volume of 1 mole of gas at STP

Answer 6

22.4 L

Question 7

what is the relationship between temperature and average kinetic energy

Answer 7

directly proportional

Question 8

what does it mean when two variables are directly proportional

Answer 8

increase or decrease together

Question 9

what does it mean when two variables are inversely proportional

Answer 9

1 increases while the other decreases

Question 10

why does pressure increase when you increase the number of moles

Answer 10

adding moles increases the number of collisions which results in pressure

Question 11

why does pressure increase when you increase the temperature

Answer 11

the kinetic energy increases and faster-moving particles strike the walls of their container with more energy

Question 12

why does air rush out of an object at high pressure and into an object at low pressure

Answer 12

differential pressure

the air is trying to reach atmospheric pressure

Question 13

what is the combined gas law

Answer 13

P1V1 P2V2
—– = ——
T1 T2

Question 14

what variable can be calculated from the ideal gas law that cannot be calculated by the combined gas law

Answer 14

number of moles

Question 15

What is the ideal gas law

Answer 15

N=PV
—
RT

PV=nRT

Question 16

what is r

Answer 16

ideal gas constant

8.31

Question 17

how to determine R at stp

Answer 17

R*moles

Question 18

what is partial pressure

Answer 18

the contribution each gas in a mixture makes to the total pressure

Question 19

what is compressibility

Answer 19

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

Question 20

what is effusion

Answer 20

a gas escapes through a tiny hole in its container

Question 21

what is diffusion

Answer 21

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

Question 22

what is the total pressure

Answer 22

the sum of the partial pressures

Question 23

diffusion and effusion rates

Answer 23

gases of lower molar mass do it faster than those with high molar masses

Question 24

the rate of effusion of a gas is _____ compared to a gas's molar mass

Answer 24

inversely proportional to the square root of a gas's molar mass

Question 25

when are real gases most similar to ideal gases

Answer 25

high temperatures and low pressures

Question 26

as pressure increases volume...

Answer 26

decreases

Question 27

as temperature increases volume...

Answer 27

increases

Question 28

as temperature increases, pressure...

Answer 28

increases

Question 29

why are gases compressible

Answer 29

volume of particles is smaller than volume of gas | distance between particles is large

Question 30

what is kinetic energy

Answer 30

the energy an object has because it is moving

Question 31

what is a vacuum

Answer 31

empty space with no particles and no pressure