Unit 5: Gases & Atmospheric Chemistry

Question 1

Intermolecular

Answer 1

Between Molecules.

Question 2

Intramolecular

Answer 2

Within Molecules.

Question 3

What are the 4 properties of gases?

Answer 3

1) Molecules are far apart
2) Weak intermolecular attraction
3) Molecules have free movement
4) Easily compressible

Question 4

What are the 4 properties of liquids?

Answer 4

1) Molecules not very close held
2) Less intermolecular attraction
3) Molecules have some movement
4) Not compressible

Question 5

What are the 4 properties of solids?

Answer 5

1) Molecules are close held
2) Strong intermolecular attraction
3) Restricted movement
4) Not compressible

Question 6

What are the 4 chemical behaviours of gases?

Answer 6

1) Chemically Inert
2) Very Reactive
3) Acidic
4) Basic

Question 7

What are the 5 assumptions of the Kinetic Theory of Matter? What is a gas that follows all of these assumptions called?

Answer 7

1) Gases consist of a large number of tiny particles that are far apart
2) Collisions between molecules are elestic which mean there is no net loss of kinetic energy it is completely transfered during collisions
3) Gas particles are in constant, rapid, random motion
4) No forces of attraction act on gas particles
5) The average kinetic energy of gas particles depeneds on the temperature of the gas

If a gas follows all of these assumptions it is called an ideal gas.

Question 8

What is the equation to find the pressure of a gas?

Answer 8

P= Force Exerted / Per Unit of Area

Question 9

Gas Pressure

Answer 9

The force resulting from molecular collisions on a surface. When you increase the number of particles/volume then you increase the number of collision and increase pressure.

Question 10

Standard Atmospheric Pressure (SAP)

Answer 10

Atmospheric pressure in dry air at a temperature of 0ºC at sea level.

Question 11

What are the 7 units of pressure?

Answer 11

1) atm
2) mmHg
3) torr
4) Pa
5) kPa
6) bar
7) psi

Question 12

How do you convert a temperture in celcius to kelvin?

Answer 12

Take your given temperature and add 273.

Question 13

What is a summarization of Boyles, Charles and Lussacs Law?

Answer 13

Boyles: A fixed amount of gas at a constant temperature is inversely proportional to the applied pressure on the gas

Charles: When temperature increases so does the speed of the gas molecules. They collide with the wall more frequently therefore the volume will increase

Lussacs: The pressure of a fixed amount of gas at a constant volume is directly proportional to it’s kelvin temperature

Question 14

What is the equation for the Ideal Gas Law?

Answer 14

PV = NRT

Question 15

In the ideal gas law equation what does R represent?

Answer 15

Universal Gas Constant

If using KPa: 8.314 KPa•L/ mol•K

If using atm: 0.0821 atm•L/mol•K

Question 16

Combined Gas Law

Answer 16

The pressure and volume of a given amount of gas are inversely proportional to each other and directly proportional to the Kelvin temperature of the gas.

Question 17

What is the equation for the combined gas law?

Answer 17

P1V1 = P2v2

__________

T1 = T2

Question 18

Avagadros Law

Answer 18

Equal volumes of all ideal gases at the same temperature and pressure contain the same number of molecules.

Question 19

Molar Volume

Answer 19

The amount of space occupied by 1 mol of an ideal gas

STP: 22.4 L/mol

Question 20

What is the temperature and pressure at STP and SATP?

Answer 20

STP: 0ºC and 101.325 kPa

SATP: 25ºC and 100 kPa

Question 21

Partial Pressure

Answer 21

The pressure of a gas in a mixture would exert if it was the only gas present in the same volume and temperature.

Question 22

Daltons Law of Partial Pressure

Answer 22

The total pressure of a mixture of nonreacting gases is equal to the sum of the partial pressures of the individual gases.

P_total= P1 + P2 + P3

Question 23

Law of Combining Volumes

Answer 23

When meaured at the same temperature and pressure, volumes of gaseous reactants and products of chemical reactions are always in simples ratios of whole numbers.