CONVERSIONS
Temperature:
Volume:
Pressure:
K = C + 273
1 L = 1000 mL
1 atm = 760 mmHg
1000 L = 1 m3
1 atm = 760 Torr
1 cm3 = 1 mL
1 atm = 101326 Pa
1 atm = 101.326 kPa
DALTON’S LAW- all pressures of different gasses added together in one
container equals total pressure. P = pressure
PT (pressure total) = P1 + P2 + P3………. (you will not always have the same
number of partial pressures)
BOYLE’S LAW- when temperature is @ a constant. Pressure and volume are
inversely proportional. P = pressure / V = volume
P1 V1 = P2 V2
Multiply your P1 and V1 and divide by your P2 or V2 (whichever it gives you in the
problem)
CHARLE’S LAW- when temperature is @ a constant. Volume and temp are
inversely proportional. V = volume / T = temperature
V1 = (V2)(T1)
T2
V2 = (V1)(T2)
T1
T1 = (T2)(V1)
V2
T2 = (T1)(V2)
V1
AVAGADRO’S LAW- if temp and pressure are constant, volume and # of moles
are directly proportional. V = volume / N = # of moles
V1 = (V2)(N1)
N2
V2 = (V1)(N2)
N1
N1 = (V1)(N2)
V2
N2 = (N1)(V2)
V1
IDEAL GAS LAW- the product of P and V of 1 gram of a molecule will equal the
product of the absolute temp. and the universal gas constant. P = pressure / V =
volume / N = # of moles / R = match to the pressure unit / T = temp in kelvin
P = (N)(Rt)
V
V = (N)(Rt)
P
N = Pv
Rt
T = Pv
nR