Ideal Gas Law

Ideal Gas Follows all gas laws under all conditions of temperature and pressure Follows all conditions of the Kinetic Molecular Theory (KMT) An ideal gas does not exist in real life

Real Gas Follows some gas laws under some conditions of temperature and pressure Does not conform to the Kinetic Molecular Theory. Real gases have a volume and attractive and repulsive forces A real gas differs from an ideal gas the most at low temperature and high pressure

Ideal Gas law equation PV = nRT P= pressure (atm, torr, mmHg, kPa) V= volume (L, mL) n = # of moles (mol) R = Ideal Gas Constant T = temperature in Kelvin (K, ˚C +273)

Ideal gas constant * Use the same unit as your given pressure R = 0.0821L atm = 8.314 L kPa = 62.4 L mmHg = 62.4 L torr mol K mol K mol K mol K * Use the same unit as your given pressure

Example 1 Calculate the number of moles of gas contained in a 3.00L vessel at 298K with a pressure of 1.50 atm. V = 3.00L T = 298K P = 1.50atm n = ? R = 0.0821 L atm mol K PV=nRT (1.50)(3.00) = n (0.0821) (298) n= 0.184 mol

Example 2 What will the pressure (in kPa) be when there are 0.400 mol of gas in a 5.00L container at 17.0˚C? V = 5.00L T = 17.0˚C = 290K P = ? kPa n = 0.400 mol R = 8.314 L atm mol K PV=nRT P(5.00) = (0.400)(8.314) (290) P= 193 kPa