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 16 - 21% of atmospheric pressure

(O2 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.

SummaryDalton 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 O2 or H2. 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.

PT = PA + PB

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?

Components Percentage

Nitrogen 78.08

Oxygen 20.95

Argon 0.93

Carbon dioxide 0.03

Neon 0.002

Other gases 0.008

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

0.03100

x 0.98 atm = 2.9 x 10-4 atm

Dalton’s law of partial pressures1. In the 18th 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 N2 at 50 kPa is mixed with 1 L of O2 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 N2, 15 kPa O2, 5 kPa CO2, and water vapour. If atmospheric pressure is 100 kPa what is the partial pressure of water vapour?

Dalton’s law of partial pressures1. That the atmosphere was a single chemical

compound.2. Water3. N2: 78.08%, O2: 20.95%, CO2: 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 (Ptotal = P1 + P2 + P3 + …)

5. Total pressure = 60 kPa + 50 kPa = 110 kPa6. 100 - (75 + 15 + 5) = 100 - 95 = 5 kPa

Vapour Pressure Defined• Vapour pressure is the pressure exerted by a

vapour. E.g. the H2O(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 (Patm), the push out is enough to overcome Patm and boiling occurs.

Vapo

ur p

ress

ure

Temperature

Vapour pressure for H2O°C kPa °C kPa10 1.23 50 12.3320 2.34 75 38.5430 4.17 100See pg. 464 for more

101.3

• 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 H2O• 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 calculationA gas was collected over 21°C H2O. After equal-izing water levels, the volume was 325 mL. Give the volume of dry gas at STP (Patm=102.9 kPa).Step 1: Determine vapour pressure (pg. 507)

At 21°C vapour pressure is 2.49 kPaStep 2: Calculate the pressure of dry gas

Pgas = Patm - PH2O = 102.9 - 2.49 = 100.41 kPaStep 3: List all of the data

T1 = 294 K, V1 = 325 mL, P1 = 100.41 kPaStep 4: Convert to STP

(P1)(V1)(T2)

(P2)(T1)V2=

(100.4 kPa)(325 mL)(273 K)(101.325 kPa)(294 K)

=

= 299 mL

Assignment1. 37.8 mL of O2 is collected by the downward

displacement of water at 24°C and an atmospheric pressure of 102.4 kPa. What is the volume of dry oxygen measured at STP?

2. Try questions 8 – 10 on page 465.3. 236 mL of H2 is collected over water at 22°C

and at an atmospheric pressure of 99.8 kPa. What is the volume of dry H2 at STP?

4. If H2 is collected over water at 22°C and an atmospheric pressure of 100.8 kPa, what is the partial pressure of the H2 when the water level inside the gas bottle is equal to the water level outside the bottle?

1)

V1 = 37.8 mL, P1 = 99.42 kPa, T1 = 297 K

V2 = ?, P2 = 101.3 kPa, T2 = 273 K

P1V1

T1

=P2V2

T2

(99.42 kPa)(37.8 mL)(297 K)

=(101.3 kPa)(V2)

(273 K)

(99.42 kPa)(37.8 mL)(273 K)(297 K)(101.3 kPa)

=(V2) = 34.1 mL

Vapor pressure at 24C = 2.98 kPaPgas = Patm - Pvapor

= 102.4 kPa - 2.98 kPa= 99.42 kPa = P1

3)

V1 = 236 mL, P1 = 97.16 kPa, T1 = 295 K

V2 = ?, P2 = 101.3 kPa, T2 = 273 K

P1V1

T1

=P2V2

T2

(97.16 kPa)(236 mL)(295 K)

=(101.3 kPa)(V2)

(273 K)(97.16 kPa)(236 mL)(273 K)

(295 K)(101.3 kPa)=(V2) = 209 mL

Vapor pressure at 22C = 2.64 kPaPgas = Patm - Pvapor

= 99.8 kPa - 2.64 kPa= 97.16 kPa = P1

Answers4 - Total pressure = PH2 + PH2O

100.8 kPa = PH2 + 2.64 kPa

100.8 kPa - 2.64 kPa = PH2 = 98.16 kPa