Chem unit 1: Gases

carbonate

CO₃²⁻

bicarbonate

HCO₃⁻

phosphate

PO₄⁻³

hydoxide

OH⁻

peroxide

O₂²⁻

cyanide

CN⁻

sulfate

SO₄²⁻

sulfite

SO₃²⁻

nitrate

NO₃⁻

nitrite

NO₂⁻

ammonium

NH₄⁺

acetate

C₂H₃O₂⁻ or CH₃COO⁻

charles law

V₁/T₁=V₂/T₂

avagadros law

V₁/n₁=V₂/n₂

boyles law

P₁V₁=P₂V₂

Lussac's Law

P₁/T₁ = P₂/T₂

Liters per mole at STP

22.4

density units

g/L

Density equation

p(mm)/RT or n(mm)/V

total pressure

((n1+n2)(RT))/V

daltons law

Ptotal=P₁+P₂+P₃...

mole fraction equation

(#moles)/total moles=Xa

partial pressure

Pa = (Ptotal)(Xa)

Kinetic Molecular Theory

1. gases are very small and spaced far apart
2.molecules are in constant random straight line motion
3. any collisions are perfectly elastic and no energy is lost or gained
4. the gas particles do not attract each other there are no intermolecular forces

kinetic energy formula

KE = 1/2 MV² (V= speed)
mass is in kg
V is in m/s
and KE is in J

kinetic energy

KE=3/2 RT

root mean square velocity

Vrms = sqrt(3RT/MolarMass)
molar mass is in kg/mol, use this for diffusion/effusion problems

Graham's law of effusion

V1/V2 = square root of mm2/mm1
2 gases must be at the same temp
can be in grams per mol
or
rate of cold/rate of hot=sqrt Tcold/T-hot
1 gas, 2 temp
temp is in kelvin

Hard Sphere Model

p(v-nb)=nrt
larger molecules will have larger b

van der waals equation

(P+n²a/V²)(V-nb)=nRT
a is for attractions

at high temp

KMT breaks down

molarity of 2 gases at the same temp and pressure

will be the same