1. Charles’ Law V 1 = V 2 T 1 T 2 Volume is directly proportional to temp (Pressure constant) Boyle’s Law P 1 V 1 = P 2 V 2 Pressure is inversely proportional to volume (temp constant) Ideal gas law PV=nRT For all gas laws Temp must always be in kelvin Combined gas law P 1 V 1 = P 2 V 2 T 1 T 2 Gay-Lussac’s Law P 1 = P 2 T 1 T 2 Pressure is directly proportional to temp (Volume constant) Gases 1

2. Dalton’s Law of Partial Pressures

7. P total = P + P + P

8. Mole fraction = # moles Total # moles

9. P = Mole fraction X P Total

10. P = # moles X P Total Total # moles

11. Dalton’s Law of Partial Pressures

12. Ideal Gas Law Where R is the universal gas constant R = 0.0821 L ● atm/mol ● K

13. Pt = p1 + p2 + p3 …….. nRT V Pt = (nRT/V) 1 + (nRT/V ) 2 + (nRT/V) 3 ……..

14. Summary of Daltons law of partial pressures equations P t =P 1 +P 2 +P 3 & P 1 = X 1.Pt X= moles of A. total moles of gas in the mixture. Mass of A GFM of A

15. Every mole contains 6.022 x 10 23 Particles. They can be Atoms Ions, Molecules or even electrons n = PV RT Moles = Mass in grams GFM Mole to Mole conversions can be done using the coefficients from a balanced equation Moles One Mole of any gas at Standard temperature 273.15 K and pressure 1 Atmosphere (101.3kPa) occupies 22.4 Liters

16. Partial Pressure Pressure each gas in a mixture would exert if it were the only gas in the container Dalton's Law of Partial Pressures The total pressure exerted by a gas mixture is the sum of the partial pressures of the gases in that mixture. P T = P 1 + P 2 + P 3 +.....

17. Partial Pressures The total pressure of a gas mixture depends on the total number of gas particles, not on the types of particles. P 1 = X 1.Pt STP P = 1.00 atm P = 1.00 atm 1.0 mol He 0.50 mol O 2 + 0.20 mol He + 0.30 mol N 2

18. How would you calculate the number of moles of a gas when given the mass of the gas? How could you calculate the moles of a gas when given temperature, volume and pressure? What is the equation to calculate mole fraction? CFU

19. A gaseous mixture made from 6.00g O 2 and 9.00 grams CH 4 is placed in a 15.0L vessel at 0 o C. What is the partial pressure of each gas and what the total pressure in the vessel Q we need to calculate the pressure of two different gases in the same volume and same temperature U atms O2 and Atm CH4 I Mass of O 2 Mass of CH 4 Total Volume 15.0L Temp 273.15K Daltons’ Law of Partial Pressures

20. A gaseous mixture made from 6.00g O 2 and 9.00 grams CH 4 is placed in a 15.0L vessel at 0 o C. What is the partial pressure of each gas and what the total pressure in the vessel Moles O 2 6 1 mole Moles CH 4 9 1 mole 32 16 Ans 0.188 0.563 PO 2 = nO 2 RT PCH 4 = n CH 4 RT V V 0.281 Atm 0.841 Atm

21. WWWWWe Do A study of the effects of certain gases on plant growth requires a synthetic atmosphere composed of 1.5 mol percent CO 2, 18 mol percent O 2 and 80.5 mol percent Ar Calculate the partial pressure of O 2 if the total pressure is 745 Torr

22. Daltons’ Law of Partial Pressures The % of gases in air Partial pressure (STP) 78.08% N 2 593.4 mmHg 20.95% O 2 159.2 mmHg 0.94% Ar 7.1 mmHg 0.03% CO 2 0.2 mmHg P AIR = P N + P O + P Ar + P CO = 760 mmHg 2 2 2 Total Pressure760 mm Hg

23. 23 CFU A. If the atmospheric pressure today is 745 mm Hg, what is the partial pressure (mm Hg) of O 2 in the air? 1) 35.6 2) 156 3) 760 B. At an atmospheric pressure of 714, what is the partial pressure (mm Hg) N 2 in the air? 1) 557 2) 9.143) 0.109

24. Solution A. If the atmospheric pressure today is 745 mm Hg, what is the partial pressure (mm Hg) of O 2 in the air? 2) 156 B. At an atmospheric pressure of 714, what is the partial pressure (mm Hg) N 2 in the air? 1) 557