The document discusses the ideal gas law PV=nRT and its application to real gases. It defines the four variables in the equation, describes how the ideal gas law relates these variables, and explains how to derive the gas constant R. While real gases deviate from ideal behavior, the ideal gas law can still adequately describe gases at low pressures and temperatures near room conditions. Two examples are given applying the ideal gas law to calculate pressure and temperature.

3. Alteration of combined gas law IGL calculates the number of moles of a gas in a fixed volume at a known temperature and pressure Relates Moles, Pressure, Volume, & Temperature

4. Describes the behavior of an “ideal” gas Cannot be used when a gas is at its critical points (Extreme Temperatures & Pressures or Phase Changes)

6. Real Gasses? Gases in the real world A gas that cannot be explained or described by the Ideal Gas Law Take into account: Compressibility Specific heat capacity Van der Waals forces

7. Defined in an environment in which all collisions between molecules or atoms are perfectly elastic (no intermolecular forces) An ideal gas has no forces of attraction between molecules (IM forces) The molecules in the gas occupy “no volume” There is no such thing as an “Ideal Gas”

10. But what does PV=nRT mean? Four Variables P = pressure (must be converted to kPa or atm) V = volume (must be converted to Liters) T = temperature (must always be in K) n = moles Universal Gas Constant R = 0.0821 L atm/ K mole or -Used to interrelate the variables of a gas

12. Derived from Boyle’s, Charle’s and Avagadro’s law from the Ideal Gas Law Constant n & T = Boyle’s Law Constant n & P = Charles’s Law Constant P & T = Avogadro’s Law Constant n & V = Gay Lusac’s Law

15. We can calculate the value of R from the other variables in the ideal gas equation. At STP (O degrees C or 273.15 K) and a pressure of 1 atm at the standard molar volume (22.414 L) We can solve for R R= 0.0821 L atm/ K mole

17. Can be used to describe the behavior of real gases at pressures around or less than 1 atm and temperatures around room temperature Gases like this behave close enough to an ideal gas such that PV=nRT can adequately describe their behavior

19. A 1.50 mole sample of Helium is placed in a 15.0 L container at 400K. What is the pressure in the container? Answer: 332 kPa

20. Evan has 23.7 grams of nitrogen gas in a 30.8 L container with a pressure of 1.5 atm. What is the temperature of the gas? Answer: 670 K

21. Pratheek has 2.03 moles of Helium in a 400.1 mL container at 282 degrees Celsius. What is the pressure of this gas in kPa? Answer: 23400 kPa