1. Section 14.3 The Ideal Gas Law

2. Objectives  Relate the amount of gas present to its pressure, temperature, and volume by using ideal gas law  Compare the properties of real an ideal gases

3. Key Terms  Ideal gas constant, R  Ideal gas law

4. Ideal Gas Law:  PV = nRT  n= number of moles  R is a constant

5. Table 14-1 Numerical Values of the Gas Constant, R Units of RValue of R Units of PUnits of VUnits of TUnits of n L*atm Mol*K 0.0821atmLKmol L *kPa Mol*K 8.314kPaLKmol L*mm Hg Mol*K 62.4Mm HgLKmol

6. Real vs Ideal Gases  Ideal  particles do not take up space; no intermolecular forces  Follows all gas laws always  Real  Particles have some volume; some forces  Approximately follows laws

7. Finding molar mass  n = m/M  m is mass  M is molar mass  PV = mRT OR M = mRT M PV

8. Practice Problems  Page 437  41-42  Page 438  46-47