1. Chapter 5 Gas Laws

2. Scuba Diving

3. Dive Belize

4. Air… The atmosphere is

5. Diving Issues Nitrogen Narcosis –Nitrogen narcosis is a condition that occurs in divers breathing compressed air. When divers go below depths of approximately 100 ft, increase in the partial pressure of nitrogen produces an altered mental state similar to alcohol intoxication.

6. The Bends Decompression sickness nitrogen from the air will dissolve in the water in his or her body. If the diver were to swim quickly to the surface, it is just like uncorking a bottle of soda -- the gas is released. This can cause a very painful condition, and it is sometimes fatal.

7. Increased pressure The pressure on divers increases by one atmosphere for every 33 feet of depth At 100 feet, some people say it is difficult to breathe

8. Decompression If divers do not decompress as they surface, they can develop the bends. Stops at various intervals as they rise to the surface, sometimes for 15 to 20 minutes or more.

9. Pressure Defined as the force per area Equation:

10. How is pressure measured? Barometers Manometers p 123, fig 5.2 Units:

11. Gas Properties The physical volume of the molecules is negligible compared to the container

12. Gas Properties Average kinetic energy is related to the absolute temperature

13. The Gas Laws Boyle’s Charles’ Guy-Lussac’s Avogadro’s Combined Ideal Molecular mass Dalton’s partial pressures

14. Boyle’s Relates pressure and volume Equation: – Temperature and number of molecules fixed –

15. Charles’ Relates volume and temperature Equation: – Pressure and number of molecules fixed –

16. Guy_Lussac’s Relates Pressure and Temperature Equation –P/T = Constant Volume and number of molecules fixed –

17. Avogadro’s Relates number of molecules and volume Equation –V/n = constant Pressure and temp are fixed –

18. Combined Relates P, V, and T Equation –PV/T = constant –Number of molecules is fixed –

19. Ideal Gas Law Combines all of the above Equation: – –Use Standard Temperature and Pressure,

20. Molecular Mass Determine the molar mass of a gas n = g/M n = PV/RT g/M = PV/RT M = gRT/PV

21. Dalton and Partial Pressure P total = P 1 + P 2 + …

22. Henry’s Law Relates solubility and pressure Equation: Volume gas dissolved Volume of liquid = C H x P g

23. Practice What is the volume of 2.40 moles of O 2 under a pressure of 5.00 atm at a temperature of 755 K?