week 2 Day 3

Volume pressure inverse volume increases, pressure decreases

Volume temperature linear temperature increases, volume increases

pressure temperature linear temperatur increases, pressure increases

increase number of particles, increase volume

PV=nRT

Standard temperature and pressure 0°C 1 bar 1 mole of gas??

22.7L

Total pressure is the sum of all the partial pressures of the components of the gas Pi = Xi * Ptotal

amount of water in the air/ solubility of water in air partial pressure of water/vapor pressure of water

temperature below which water droplets begin to condense and dew forms

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

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.

square rood of (Temperature/Molecular weight)

at very high pressure and very low temperature real gases do not behave like ideal gases. use van der Waals equation for real gases