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# 11.10PartialPressures - PowerPoint PPT Presentation

A hyperbaric chamber is used in the treatment of certain diseases. Chapter 11 Gases. 11.10 Partial Pressure (Dalton’s Law). Partial Pressure. The partial pressure of a gas is the pressure of each gas in a mixture is the pressure that gas would exert if it were by itself in the container.

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Chapter 11 Gases

11.10

Partial Pressure (Dalton’s Law)

Partial Pressure diseases.

The partial pressure of a gas

• is the pressure of each gas in a mixture

• is the pressure that gas would exert if it were by itself in the container

Dalton’s Law of Partial Pressures diseases.

Dalton’s law of partial pressuresstates

that the total pressure

• depends on the total number of gas particles, not on the types of particles

• exerted by a gas mixture is the sum of the partial pressures of those gases

PT = P1 + P2 + P3 .....

Illustrating Partial Pressures

Under water, the pressure on a diver is greater than the atmospheric pressure.

Scuba Diving

• When a scuba diver is below the ocean surface, the increased pressure causes more N2(g)to dissolve in the blood.

• If a diver rises too fast, the dissolved N2 can form bubbles in the blood, a dangerous and painful condition called "the bends.”

• For deep descents, helium, which does not dissolve in the blood, is added to O2.

Solving for Partial Pressure atmospheric pressure.

Learning Check atmospheric pressure.

A scuba tank contains O2 with a pressure of 0.450 atm and He at 855 mmHg. What is the total pressure in mmHg in the tank?

Solution atmospheric pressure.

STEP 1 Write the equation for the sum of partial pressures.

Ptotal = Po2 + PHe

STEP 2Solve for the unknown pressure.

Convert the pressure in atm to mmHg to match units.

0.450 atm x 760 mmHg = 342 mmHg = PO2 1 atm

STEP 3Substitute known pressure and calculate the unknown.

Ptotal = 342 mmHg + 855 mmHg

= 1197 mmHg

A Nitrox mixture is used to fill scuba tanks. atmospheric pressure.

Learning Check

For some dives, scuba divers use a mixture of nitrogen and oxygen gases (Nitrox) with a pressure of 8.00 atm. If the oxygen in a tank of Nitrox has a partial pressure of 2190 mmHg, what is the partial pressure of the nitrogen?

1) 520 mmHg

2) 2040 mmHg

3) 3890 mmHg

Solution atmospheric pressure.

STEP 1 Write the equation for the sum of partial pressures.

Ptotal = PO2 + PN2

Ptotal = 8.00 atm x 760 mmHg = 6080 mmHg

1 atm

STEP 2Solve for the unknown pressure.

Ptotal = PO + PN2

2

PN2= Ptotal - PO2

Solution (continued) atmospheric pressure.

STEP 3Substitute known pressure and calculate the unknown.

PN2= Ptotal - PO2

PN2= 6080 mmHg - 2190 mmHg

= 3890 mmHg (3)

Gases Collected over Water atmospheric pressure.

A gas produced in the

laboratory

• usually contains water vapor

• PT = Pwater + Pgas

• has a partial pressure obtained by subtracting the vapor pressure of water from the PT

Gases Collected over Water atmospheric pressure.

Learning Check atmospheric pressure.

The decomposition of KClO3 produces O2 gas and solid KCl. If 124 mL of O2 is collected over water at 762 mmHg at 20.0 C, how many moles of O2 are produced? (Partial pressure water at 20.0 C = 18 mmHg.)

2KClO3(s) 2KCl(s) + 3O2(g)

Solution atmospheric pressure.

STEP 1 Obtain the vapor pressure of water.

Partial pressure of water at 20.0 C = 18 mmHg

STEP 2Subtract vapor pressure from total P of gas mixture to give partial pressure of needed gas.

PT = Pwater + Pgas

Pgas = PT - Pwater

PO2 = 762 mmHg - 18 mmHg = 744 mmHg

Solution (continued) atmospheric pressure.

STEP 3 Use ideal gas law to convert Pgasto moles or grams of gas collected.

PV = nRT

n = PV = (744 mmHg)(0.124 L) = 0.00505 mol of O2

RT (62.4 L • mmHg)(293 K)

mol • K

Gases We Breathe atmospheric pressure.

The air we breathe

• is a gas mixture

• contains mostly N2 and O2 and small amounts of other gases

Gas Exchange During Breathing atmospheric pressure.

Blood Gases atmospheric pressure.

• In the lungs, O2 enters the blood, while CO2 from the blood is released.

• In the tissues, O2 enters the cells, while CO2 is released into the blood.

Blood Gases atmospheric pressure.

In the body,

• O2 flows into the tissues because the partial pressure of O2 is higher in the blood and lower in the tissues

• CO2 flows out of the tissues because the partial pressure of CO2 is higher in the tissues and lower in the blood