week 2 Day 3

Question 1

Boyle’s Law

Answer 1

Volume pressure inverse

volume increases, pressure decreases

Question 2

Charle’s Law

Answer 2

Volume temperature linear

temperature increases, volume increases

Question 3

Guy-Lussac’s Law

Answer 3

pressure temperature linear

temperatur increases, pressure increases

Question 4

Avogadro’s Law

Answer 4

increase number of particles, increase volume

Question 5

ideal gas law

Answer 5

PV=nRT

Question 6

STP

Answer 6

Standard temperature and pressure

0°C

1 bar

1 mole of gas??

Question 7

Volume of one mole of any gas at STP

Answer 7

22.7L

Question 8

Dalton’s Law

Answer 8

Total pressure is the sum of all the partial pressures of the components of the gas

P_i = X_i * P_total

Question 9

Relative humidity

Answer 9

amount of water in the air/ solubility of water in air

partial pressure of water/vapor pressure of water

Question 10

dew point

Answer 10

temperature below which water droplets begin to condense and dew forms

Question 11

Kinetic molecular theory of gasses

Answer 11

1. gas molecules are small compared to the volume of the gas, so we can ignore the size of the molecules
2. gal molecules are in constant, random motion
3. gas molecules show a range of kinetic energies but the average depends on the temperature.
4. gas molecules are not attracted or repulsed from each other, so all collisions are elastic.

Question 12

Graham’s Law of Effusion

Answer 12

KE = 1/2 * m * v²

m = molecular weight / Avogadro’s number

*only divide by avogadro’s if you use the constant that had avogadros number involved.

Question 13

rate of effusion

Answer 13

square rood of (Temperature/Molecular weight)

Question 14

Real gases

Answer 14

at very high pressure and very low temperature real gases do not behave like ideal gases.

use van der Waals equation for real gases