Chapter 10

Question 0

Ideal gas

Answer 0

Imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory.

Question 1

Kinetic-Molecular Theory

Answer 1

-idea that particles of matter are always in motion.

Theory of moving molecules in gases.

Question 2

5 parts of the Kinetic-Molecular Theory.

Answer 2

1. Gas are made up of a large number of really tiny particles that are really far apart.
2. Particles are in constant (random) motion.
3. Particles undergo elastic collisions.
4. There are no attractive or repulsive forces between particles.
5. The average kinetic energy of the particles depend on the temperature.

Question 3

5 Properties of Gas

Answer 3

1. Expansion and Contraction
2. Fluidity
3. Low Density
4. Diffusion
5. Effusion

Question 4

Parts of Kinetic-Molecular Theory that go with:

Expansion and Contraction. (3)

Answer 4

1. They are really far apart; we can push them together.
2. No forces of attraction and repulsion.
3. Elastic collisions; bounce apart

• gases has no definite shape; allow them to fill a container
• move is all directions

Question 5

Parts of Kinetic-Molecular Theory that go with:

Fluidity. (3)

Answer 5

1. Elastic Collisions
2. No attractive or repulsive forces
3. Constant motion

Question 6

Parts of Kinetic-Molecular Theory that go with: low density. (2)

Answer 6

1. Really far apart (big volume)

2. Really tiny particles (small mass)

Question 7

Parts of Kinetic-Molecular Theory that go with:

Diffusion and effusion. (3)

Answer 7

1. Elastic collisions
2. Constant motion
   Effusion
3. Tiny particles

Question 8

Fluidity

Answer 8

Anything that flows.

Question 9

Diffusion

Answer 9

Spontaneous (starts itself) mixing of particles caused by random movement.

Question 10

Effusion

Answer 10

Process by which has particles under pressure pass through tiny openings.

Question 11

Real gas

Answer 11

Gas that does not behave completely according to the assumptions of the kinetic- molecular theory.

Question 12

Rate of diffusion. (2)

Answer 12

Speed- temperature

Mass-smaller, lighter particles diffuse faster

Question 13

SI unit for force.

Answer 13

Newton

Question 14

Pressure

Answer 14

Force per unit area on a surface.
P=F/A
Particles colliding with walls of the container create pressure/ colliding with surface of substance.

Question 15

Barometer

Answer 15

Device used to measure atmospheric pressure.

Evangelista Torricceli

Question 16

Millimeters of Mercury.
Atm pressure.
Pascal.

Answer 16

Mm Hg, common unit of pressure.
Equivalent to 760 mm Hg. Torr is the same.
Pressure exerted by a force of one Newton acting on an area per square meter. 101,325
kPa 101.325
29.92 in Hg

Question 17

Standard Temperature and Pressure.

Answer 17

0 degrees Celsius; 273K

1 atm

Question 18

Gas Laws

Answer 18

Simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas.

Question 19

Johannes Van Der Waals

Answer 19

1. Showed that gas Pericles DO have attractions.
   They are only significant under extreme low temperature or high pressure
2. Not a problem under normal conditions
   Discussion of gases it’s contain condition
   (No pressure, not useable)

Question 20

Manometer

Answer 20

Measures gas pressures. Same as barometer but not open to atmosphere.

Question 21

Robert Boyle

Answer 21

1600
English
If the amount and temperature of a gas are held constant, the volume varies inversely with the pressure.
V1P1=V2P2

Question 22

Jacques Charles

Answer 22

1787
The volume of a fixed quantity of gas at a constant pressure is directly proportional to its Kelvin temperature.
V1/T1=V2T2

Question 23

Absolute zero

Answer 23

0K

Question 24

Joseph Gay-Lussak

Answer 24

1802 If the volume and amount of a gas remain constant. The Kelvin temperature varies directly with pressure. P1/T1=P2/T2

Question 25

Combined gas law.

Answer 25

Expresses the relationship between pressure,volume, and temperature of a fixed amount of gas. V1P1/T1=V2P2/T2

Question 26

Dalton's Law of Particle Pressures.

Answer 26

The total pressure of a mixture of gases is equal to the sum of their practical pressures of the component gases. (Lower level; higher pressure) This is P1. Hints to this problem: collected over water Or just the tots pressure of a mixture of gases is equal to the sum of their partial pressures.

Question 27

How much farther are gases in solids than liquids?

Answer 27

10x | 1000x more volume in a gas

Question 28

Elastic collisions.

Answer 28

Total conservation of kinetic energy.

Question 29

Atmospheric pressure.

Answer 29

Weight of air.

Question 30

Are we ever out of gas?

Answer 30

No just not enough pressure crashing against the surface to push it out.