How Much Pressure? Q - A balloon is filled with pure oxygen. What is the pressure of the oxygen in the balloon? A - Atmospheric pressure. If it wasn’t, then the balloon would expand or shrink. Q - A windbag is blown up with exhaled air. What is the pressure of oxygen in the bag? A – Around % of atmospheric pressure (O 2 is 16% of exhaled air, 21% of atmosphere) Q - A solid container is filled with pure oxygen. What is the pressure in the container? A - It could be anything. The container is solid and therefore cannot shrink or expand.

Summary Dalton found that the total pressure of mixed gases is equal to the sum of their individual pressures (provided the gases do not react). + 1 L oxygen 50 kPa 1 L nitrogen 100 kPa 1 L mixed gas 150 kPa = This works according to the KMT because at the same temperature molecules of different gases have the same Ek. It doesn’t matter if the molecules are O 2 or H 2. Both collide with the container or other molecules with the same force. Note: all of these volumes are the same

Dalton’s law of Partial Pressures The total pressure of a mixture of gases is the sum of the pressures of each of the individual gases. P T = P A + P B

Applying Daltons’ Law of Partial Pressures Example: What is the pressure contribution of Carbon dioxide to the atmospheric pressure on a very dry day when the barometer reads 0.98 atm ?

ComponentsPercentage Nitrogen78.08 Oxygen20.95 Argon0.93 Carbon dioxide0.03 Neon0.002 Other gases0.008

According to the previous table, carbon dioxide contributes 0.03% of the atmospheric pressure. If the total pressure is 0.98 atm, then x 0.98 atm = 2.9 x atm

Dalton’s law of partial pressures 1.In the 18 th century what did many scientists believe about the earth’s atmosphere? 2.The % of which component of air varies the most? 3.Argon makes up about 0.93% of dry air. List the other 3 gases present in dry air (with their %s). Around what % of dry air is made up by gases other than these 4? 4.Give Dalton’s law of partial pressures & the equation. 5.1 L of N 2 at 50 kPa is mixed with 1 L of O 2 at 60 kPa, to form a 1 L mixture of the gases. What is the resulting pressure? What are the partial pressures? 6.A balloon contains 75 kPa N 2, 15 kPa O 2, 5 kPa CO 2, and water vapour. If atmospheric pressure is 100 kPa what is the partial pressure of water vapour?

Dalton’s law of partial pressures 1.That the atmosphere was a single chemical compound. 2.Water 3.N 2 : 78.08%, O 2 : 20.95%, CO 2 : 0.04%. These add up to 100% of dry air, so there are almost no other gases (really, 0.002%). 4.The total pressure of a mixture of nonreacting gases is equal to the sum of the partial pressures of the individual gases (P total = P 1 + P 2 + P 3 + …) 5.Total pressure = 60 kPa + 50 kPa = 110 kPa ( ) = = 5 kPa

Vapour Pressure Defined Vapour pressure is the pressure exerted by a vapour. E.g. the H 2 O(g) in a sealed container. Yet, molecules both leave and join the surface, so vapour pressure also pushes molecules up. Eventually the air above the water is filled with vapour pushing down. As temperature , more molecules fill the air, and vapour pressure . To measure vapour pressure we can heat a sample of liquid on top of a column of Hg and see the pressure it exerts at different °C.

Measuring Vapour Pressure When the vapour pressure is equal to the atmospheric pressure (P atm ), the push out is enough to overcome P atm and boiling occurs. Vapour pressure Temperature Vapour pressure for H 2 O °CkPa°CkPa See pg. 464 for more Thus, water will boil at a temperature below 100 °C if the atmospheric pressure is reduced.

Collecting gases over water Many times gases are collected over H 2 O Often we want to know the volume of dry gas at STP (useful for stoichiometry). For this we must make 3 corrections: 1.The level of water inside and outside the tube must be level (so pressure inside is equal to the pressure outside). 2.The water vapour pressure must be subtracted from the total pressure (to get the pressure of the dry gas). 3.Finally, values are converted to STP using the combined gas law.

Sample calculation A gas was collected over 21°C H 2 O. After equal- izing water levels, the volume was 325 mL. Give the volume of dry gas at STP (P atm =102.9 kPa). Step 1: Determine vapour pressure (pg. 507) At 21°C vapour pressure is 2.49 kPa Step 2: Calculate the pressure of dry gas P gas = P atm - P H2O = = kPa Step 3: List all of the data T 1 = 294 K, V 1 = 325 mL, P 1 = kPa Step 4: Convert to STP (P 1 )(V 1 )(T 2 ) (P 2 )(T 1 ) V2=V2= (100.4 kPa)(325 mL)(273 K) ( kPa)(294 K) = = 299 mL

Assignment mL of O 2 is collected by the downward displacement of water at 24°C and an atmospheric pressure of kPa. What is the volume of dry oxygen measured at STP? 2.Try questions 8 – 10 on page mL of H 2 is collected over water at 22°C and at an atmospheric pressure of 99.8 kPa. What is the volume of dry H 2 at STP? 4.If H 2 is collected over water at 22°C and an atmospheric pressure of kPa, what is the partial pressure of the H 2 when the water level inside the gas bottle is equal to the water level outside the bottle?

1) V 1 = 37.8 mL, P 1 = kPa, T 1 = 297 K V 2 = ?, P 2 = kPa, T 2 = 273 K P1V1P1V1 T1T1 = P2V2P2V2 T2T2 (99.42 kPa)(37.8 mL) (297 K) = (101.3 kPa)(V 2 ) (273 K) (99.42 kPa)(37.8 mL)(273 K) (297 K)(101.3 kPa) =(V 2 )=34.1 mL Vapor pressure at 24  C = 2.98 kPa Pgas = Patm - Pvapor = kPa kPa = kPa = P 1

3) V 1 = 236 mL, P 1 = kPa, T 1 = 295 K V 2 = ?, P 2 = kPa, T 2 = 273 K P1V1P1V1 T1T1 = P2V2P2V2 T2T2 (97.16 kPa)(236 mL) (295 K) = (101.3 kPa)(V 2 ) (273 K) (97.16 kPa)(236 mL)(273 K) (295 K)(101.3 kPa) =(V 2 )=209 mL Vapor pressure at 22  C = 2.64 kPa Pgas = Patm - Pvapor = 99.8 kPa kPa = kPa = P 1

Answers 4 - Total pressure = P H 2 + P H 2 O kPa = P H kPa kPa kPa = P H 2 = kPa