Ideal Gas Laws

1st notes on Unit 3

what units does everything need to be for the ideal gas equation

atm, Liters (L), mol, Kelvin. (K)

equation to turn celcius into kelvin

T_k= T_c +273.15

Combined gas law (when n is constant)

P₁V₁/T₁ = P₂V₂/T₂

Boyle’s Law : describes the relationship between volume and pressure

P₁V₁= P₂V₂

relationship between volume and pressure in boyles law

inverse relationship: as volume increases, pressure decreases

Charles Law (when n and P are constant aka the same)

V₁/T₁ = V₂/T₂

relationship between volume and temperature (charles law)

when volume increases, temperature increases

Gay-lussac’s law (when n and V is constant)

P₁/T₁ = P₂/T₂

relationship between pressure and temperature

direct realtionship: as pressure goes up , temperature goes up

avogadros law. (when P and T are constant)

V₁/n₁ = V₂/n₂

realtionship between volume and mols

direct relationship: as volume increases, mols incerease

how to find mol (n)

find the atomic mass. when it is a diatmoic moluemole multiple by 2. when its a compound add everything togther

equation for n

Mass (M)/Molemar Mass (MM)

how to calcualte the density (ρ) of a gass

P(MM)/R(T)

how to idenfity a gas

calculate the molar mass (MM)

STP meaning

standard temperature and pressure

what are the STP units

T= 273K (0 c)

P=1 atm

n=1 mol

V= 22.4 L

Daltons Law of partial pressures

P_t = n_t (RT/V)

Daltons law states

that the total pressire of a gas is equal to the partial pressures ( P_T= P₁ + P₂+ P₃…)

Under what conditions do gases act the most ideal?

High temperature and low pressure

1st assumptin when dealing with ideal gas

the moleucles of an ideal gas do no interact with one another

2nd assumptin when dealing with ideal gas

the combined volume of the molecules is much smaller than the volume of the gas ccupes (volume occuiped by the moleuclule is negliable)

molecular weight versus density

Density is the measure of mass of an atom per volume. molecular weight refers to the mass of a single molecule of a substance,

How to find the total pressure

P_t= P₁ +P₂ + P₃ +….P_n

mole fraction

Xi= # of mol of gas i/ total # of mol

Daltons Law of partial pressures

Pi = Xi * Pt(atm)

how to convert grams to moles

grams/ molar mass

relationship beween P and MW

When P increases, MW decreases (inverse)

relationship between m and MW

When m increases, MW increases