Common gas conversions

1 Pa

N/m²

1 N/m²

kg(m)/s²

1 kPa = ____ Pa

1,000 Pa

1 bar = _____ Pa

100,000 Pa

1 mmHg = ___ torr

1 torr

1 atm = ___ torr

760 torr

1 atm = ____ psi

14.7 lb/in²

760 torr = ____ Pa

101,325 Pa

Patm > Pgas

Pgas= Patm (mmHg) - mmHg height

Pgas > Patm

Pgas= Patm (mmHg) + mmHg height

Boyles Law

moles & temperature are constant

volume & pressure change

Boyles Law Equation

PV = K or P1V1=P2V2

Charles Law

moles & pressure constant

volume & temp change

Charles Law Equation

V/T = K or V1/T1 = V2/T2

Avogadros Law

temperature & pressure are constant

volume & moles change

Avogadros Law Equation

V/n = K. or. V1/n1 = V2/n2

STP =

22.414 L, 0 degrees Celsius, 1 atm

Ideal Gas Law Equation

PV= nRT

Gas Density Equation

d= m/V = PM/RT

Concentration of a Partial Pressure equation

X = Moles of a component gas/ total moles in the mix of gases.  

OR

P(A) = X(A) x P(total)

Avg speed of gas molecule equation

V = (3RT/mNA)^1/2 or (3RT/M)^1/2

Avg distance between collisions is called…

mean free path

Graham’s Law (rate of effusion)

1/m^(1/2)