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The Nature of Gases – Part 2 - PowerPoint PPT Presentation

Gas Pressure. The Nature of Gases – Part 2. Objectives. When you complete this presentation, you will be able to: describe gas pressure in terms of the motion of gas particles. describe the invention of the barometer. describe the derivation of the units of pressure.

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The Nature of Gases – Part 2

• When you complete this presentation, you will be able to:

• describe gas pressure in terms of the motion of gas particles.

• describe the invention of the barometer.

• describe the derivation of the units of pressure.

• convert between the units of pressure.

• Gas pressure is the result of the force of gas molecules exerted on a surface.

• The force of a single molecule of gas in insignificant, but the force of trillions of molecules becomes measurable.

• A vacuumis a volume where there are no gas molecules bouncing off a surface.

• Atmospheric pressure results from the collision of air molecules with objects.

• We measure the pressure of a gas by using an instrument called a barometer.

• The barometer was invented in 1643by the Italian physicist Evangelista Torricelli.

• He made a barometer from a tube of glass (sealed at one end) and a trough of mercury.

• We measure the pressure of a gas by using an instrument called a barometer.

• The barometer was invented in 1643by the Italian physicist Evangelista Torricelli.

• He made a barometer from a tube of glass (sealed at one end) and a trough of mercury.

• We measure the pressure of a gas by using an instrument called a barometer.

• The barometer was invented in 1643by the Italian physicist Evangelista Torricelli.

• He made a barometer from a tube of glass (sealed at one end) and a trough of mercury.

• The airpressure on the Hg held the column up.

• The air pressure in a barometer is measured by measuring the heightof the mercury column.

• Under standard conditions, a column of mercury will be 760 mmin height.

• So, we say that 1 atmosphere of pressure (1 atm) is equal to 760 mm Hg.

760 mm

• Another unit for pressure uses SI units for force (newtons, N) per area (m2) which is called a Pascal, (Pa).

• Under standard conditions, 1 atm of pressure is equal to 101,300 Pa = 101.3 kPa.

• Our conversions are:

1.000atm = 760.0 mm Hg = 101.3 kPa

A container of oxygen gas has a pressure of 0.450 atm. Find the pressure in mm Hg and kPa.

Conversions:

1.000 atm = 760.0 mm Hg = 101.3 kPa

Solution:

0.450 atm

760.0 mm Hg

101.3 kPa

342 mm Hg

=

×

×

1.000 atm

1.000 atm

1

1

0.450 atm

45.6 kPa

=

A container of nitrogen gas has a pressure of 855 mm Hg. Find the pressure in atm and kPa.

Conversions:

1.000 atm = 760.0 mm Hg = 101.3 kPa

Solution:

855 mm Hg

1.000 atm

101.3 kPa

1.13 atm

=

×

×

760.0 mm Hg

760.0 mm Hg

1

1

855 mm Hg

114 kPa

=

A container of hydrogen gas has a pressure of 97.3 kPa. Find the pressure in atm and mm Hg.

Conversions:

1.000 atm = 760.0 mm Hg = 101.3 kPa

Solution:

97.3 kPa

1.000 atm

760.0 mm Hg

0.961 atm

=

×

×

1

1

101.3 kPa

101.3 kPa

97.3 kPa

730 mm Hg

=

Fill in the blanks for each of the following pressures

Conversions:

1.000 atm = 760.0 mm Hg = 101.3 kPa

• Gas pressure is the result of the force of gas molecules exerted on a surface.

• Atmospheric pressure results from the collision of air molecules with objects.

• We measure the pressure of a gas by using an instrument called a barometer invented in 1643 by the Italian physicist Evangelista Torricelli.

• Our conversions are:

1.000 atm = 760.0 mmHg = 101.3 kPa