Gases

Question 1

Kinetic molecular theory

Answer 1

a gas can be understood as tiny particles bouncing around in a space. the pressure on the walls of a container result in of elastic collisions.

Question 2

Average kinetic energy equation

Answer 2

U= 3/2RT
R= constant
T= temperature

Question 3

Brownian motion

Answer 3

random particle movement

Question 4

Ideal gas

Answer 4

assumptions:
- gas particles have no volume (do not take up space)
- gas particles experience no attractive or repulsive forces

Question 5

Ideal gas behvavior

Answer 5

a high temperature, large volume, and low pressure makes them more like a gas

Question 6

Boyle’s Law

Answer 6

pressure and volume of a gas are inversely related

P1V1=P2V2

Question 7

Charle’s law

Answer 7

volume and temperature of a gas are directly related

V1/T1=V2/V2

Question 8

Avogadro’s law

Answer 8

Volume of gas is directly related to the number of moles of a gas particle
V1/n1=V2/n2

Question 9

At STP (273 K and 1 atm)….

Answer 9

1 mole of gas= 22.4 L of space

this is the molar volume

Question 10

Ideal gas law equation

Answer 10

PV=nRT
R= 0.08 L atm/molK
or 8.31 J/molK

Question 11

Real gases

Answer 11

-acknowledge gas have size and there are interactions

Question 12

Real gases equation (Van Der Waals equation)

Answer 12

(P + a/Vm^2) (Vm - b) =RT
a= attractive intermolecular forces
b=size of particles

Question 13

Real gases under extreme pressure or low tempueratire

Answer 13

have a high pressure when compared to ideal gas and a low pressure when compared to an ideal gas at low temperatures

Question 14

Dalton’s law

Answer 14

total pressure is equal to individual pressures of each gas present in the solution
pgas= (xgas)(ptotal)
xgas= mole fraction

Question 15

Graham’s law

Answer 15

when a gas is diffusion, smaller and lighter particles will escape faster
r1?r2=SQRT (m2/m1)