Module 6a: Gas Laws

Question 1

What does Kinetic Theory of Matter tell you?

Answer 1

A prediction of how matter should behave

Question 2

T/F: All matter is made up of moving particles

Answer 2

T

Question 3

Solids have tightly bound particles that ______

Answer 3

vibrate

Question 4

Describe the particles in liquids

Answer 4

Free to move
still attracted to each other

Question 5

Describe the particles in gases

Answer 5

Far apart
move freely

Question 6

Phase changes occur with increases in ________ in matter

Answer 6

Kinetic energy

Question 7

What form does kinetic energy normally come in?

Answer 7

Heat

Question 8

What happens when you heat up a solid?

Answer 8

Particles can vibrate which increases entropy.
particles break apart and matter liquifies.
Continues to heat up. Can evaporate (turn into gas)

Question 9

T/F: Physical properties of gases are all similar

Answer 9

T

Question 10

Describe the boiling point of most gases?

Answer 10

Low

Question 11

Gases are composed mainly of __________ elements with ________ formulas, ___________ compounds, and ________ molar masses

Answer 11

Nonmetallic
Simple
Small
Low

Question 12

What are 3 additional characteristics of gasses

Answer 12

Expand to fill their container
highly compressible
extremely low densities

Question 13

What happens when you compress and cool a gas?

Answer 13

Turns into a liquid

Question 14

What type of mixture are 2 gases?

Answer 14

Homogeneous mixture

Question 15

Describe the molecules in gases

Answer 15

Move independently
no forces keeping them together or pushing them apart

Question 16

T/F: Kinetic Theory of Gases: Gases consist of large numbers of molecules that are in continuous, random motion

Answer 16

T

Question 17

T/F: Kinetic Theory of Gases: Attractive and repulsive forces between gas molecules are strong

Answer 17

F

weak

Question 18

When you increase the temperature, the kinetic energy goes ______

Answer 18

Up

Question 19

T/F: Kinetic Theory of Gases: Energy can be transferred between molecules during collisons, but the average kinetic energy of the molecules does not change with time, as long as the temperate of the gas remains constant

Answer 19

T

Question 20

T/F: Kinetic Theory of Gases: Average kinetic energy of gas molecules is dependent on a few factors

Answer 20

F

is ONLY dependent on the temperature

Question 21

_________ is related to the average kinetic energy

Answer 21

temperature

Question 22

u(rms) =

Answer 22

The root mean-squared speed

associated with average kinetic speed

Question 23

T/F: At any given temperature, the average kinetic energy of molecules is the same

Answer 23

T

Question 24

R =

Answer 24

0.08206

Question 25

Temperature is measured in _______

Answer 25

Kelvin

Question 26

Describe the relationship between molar mass and particle speed

Answer 26

Lower molar mass = higher speed Higher molar mass = lower speed

Question 27

Kelvin =

Answer 27

C + 273.15

Question 28

What does STP mean?

Answer 28

Standard Temperature and Pressure Temp = 273.15 Kelvin Pressure = 1atm/760mmHg/760torr

Question 29

Pressure Values:

Answer 29

1 atm = 760 mmHg = 760 torr

Question 30

Pressure =

Answer 30

Force / Area

Question 31

What is Atomospheric Pressure?

Answer 31

The weight of air per unit of area

Question 32

What is the atomospheric pressure at sea level?

Answer 32

760 mmHg

Question 33

Describe Gas Law: Boyle's Law

Answer 33

P₁V₁ = P₂V₂ Pressure inversely related to Volume Temp is constant Decrease volume = increase pressure

Question 34

Describe Gas Law: Charles' Law

Answer 34

V₁/T₁ = V₂/T₂ Temp directly related to volume Pressure and amount are constant increase temp = increase volume

Question 35

Describe Gas Law: Gay-Lussac's Law

Answer 35

P₁/T₁ = P₂/T₂ Pressure is directly related to temp Volume and amount are constant increase temp = increase pressure

Question 36

What gas law explains why water boils over at a lower temp at higher elevations?

Answer 36

Gay-Lussac's Law

Question 37

Describe Gas Law: Combined Gas Law

Answer 37

(P₁V₁)/T₁ = (P₂V₂)/T₂ Combination of Boyle's, Charles', and Gay-Lussac's Law n is constant

Question 38

Describe Gas Law: Avogadro's Law

Answer 38

V₁/n₁ = V₂/n₂ Volume directly related to moles Temp and pressure are constant increases moles = increased volume

Question 39

At STP, how much volume does 1 mol of gas occupy?

Answer 39

22.4 L

Question 40

n =

Answer 40

number of moles

Question 41

Describe Gas Law: Ideal Gas Law

Answer 41

PV= nRT R = 0.08206

Question 42

Describe Gas Law: Dalton's Law

Answer 42

If 2 gases that DO NOT REACT are combined in a container, ACT AS IF THEY ARE ALONE P_t = P₁ + P₂ + P₃..... P₁ = (n₁/n_t) x P_t

Question 43

Describe Gas Law: Graham's Law

Answer 43

r₁/r₂ = sq(M₂/M₁) Relates molar mass of 2 gases to their rate of speed decrease molar mass = increase rate of speed

Question 44

What is effusion?

Answer 44

Escape of gas molecules through a tiny hole into an evacuated space until equilibrium is reached.

Question 45

What is diffusion?

Answer 45

Spread of a substances through a space from a higher pressure to a lower pressure

Question 46

Describe Gas Law: Henry's Law

Answer 46

Solubility of a gas in a volume of liquid is porportional to partial pressure of that gas in equilibrium with that of the liquid

Question 47

In the real world, the behavior of gases conforms to the ideal gas law only at ______ temperatures and ______ pressures

Answer 47

high low

Question 48

T/F: A gas will show different behaviors at high pressures and low temperatures

Answer 48

T Gases need high temps and low pressures to be predictable

Question 49

T/F: The assumptions of the Kinetic Theory of Gases are tue even when gases are exposed to low temperatures and high pressures

Answer 49

F In the real world, this doesn't work. This makes gas unstable.

Question 50

Describe Gas Law: Van der Waals Equation

Answer 50

Takes into account ideal gas deviations Adjustments include: Pressure and Volume (P + N^2 a/V^2) (V-nb) = nRT *HE SAIDDDDDD HE WONT PUT THIS ON THE TEST*

Question 51

If we are to ASSUME a volume, what is it?

Answer 51

100ml

Question 52

What is w/v?

Answer 52

(weight in grams) / 100ml !!!!!!!!!!!!!!!!!

Question 53

What is w/w?

Answer 53

(weight in grams) / 100g !!!!!!!!!!!!!!!!!!!!!!!!!!!