Gas Laws

Question 1

Charles Law

Answer 1

V1/T1=V2/T2

Question 2

Combined Gas Law

Answer 2

P1V1/n1T1=P2V2/n2T2

Question 3

Gay Lussac Law

Answer 3

P1/T1=P2/T2

Question 4

Ideal Gas Law

Answer 4

PV=nRT

Question 5

Universal Gas Constant

Answer 5

.08206

Question 6

Dalton’s Law of Partial Pressures

Answer 6

P(total)=P1+P2+P3…

Question 7

Avogadro’s Law

Answer 7

V1n1=V2n2

Question 8

Density (g/L)=

Answer 8

PMM/RT

MM=molar mass

Question 9

4 factors

Answer 9

Pressure
Volume
Temperature
Moles

Question 10

Mole fraction

Answer 10

Moles of element/total moles

Question 11

Kinetic Molecular Theory of Gases

Answer 11

Gases consist of tiny particles (atoms/molecules)
Particles are so small compared to the distance between them that the volume of them can be assumed to be negligible
The particles are in constant random motion colliding with the walls of the container (pressure)
Particles are assumed not to attract or repel each other
The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature of the gas
Pressure and volume increases as temperature increases because the particles speed up

Question 12

Real Gases

Answer 12

Gases don’t behave ideally under conditions of high pressure and low temperature

Question 13

Boyles Law

Answer 13

P1xV1=P2xV2

Question 14

1 atm=

Answer 14

760torr= 760mm Hg= 101.325kPa= 14.696