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Chapter 11a Gas Laws I. According to the kinetic molecular theory, the kinetic energy of a gas depends on. temperature and pressure. The kinetic-molecular theory states that gas particles are very far apart. What properties of a gas does this idea explain?. the fluidity and compressibility.

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Presentation Transcript
according to the kinetic molecular theory the kinetic energy of a gas depends on
According to the kinetic molecular theory, the kinetic energy of a gas depends on
  • temperature and pressure
slide3
The kinetic-molecular theory states that gas particles are very far apart. What properties of a gas does this idea explain?

the fluidity and compressibility

true or false
True or false
  • According to the kinetic-molecular theory, particles of a gas collide?
  • According to the kinetic-molecular theory, particles gain and lose energy after an elastic collision?
  • According to the kinetic-molecular theory, particles of a gas attract each other?
  • According to the kinetic-molecular theory, particles of a gas repel each other?

True

False

False

False

Gas particles neither attract nor repel each other, but they do collide in a elastic collision.

Elastic Collisions result in NO net loss of energy.

slide6

A pressure of 700. kPa is equal to

_____ mm Hg.

700. kPa * __1 atm_ * 760 mmHg =

101.3kPa 1 atm

  • 5250.
slide7

The average atmospheric pressure in Denver is 0.830 atm. What is this pressure in kPa?

0.830atm * 101.3kPa = 84.1atm

1 atm

slide8

If the temperature remains constant, V1 and P1 represent the original volume and pressure, and V2 and P2 represent the new volume and pressure, what is the mathematical expression for Boyle’s law?

P1V1 =P2V2

slide11
The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to

Avogadro

slide12

Gay-Lussac recognized that the pressure of a fixed mass of gas at constant volume is directly proportional to the Kelvin temperature. Mathematically, Gay-Lussac’s law is expressed as

P = k

T

slide13

Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures?

Dalton

slide14

What happens to temperature during the compression of a gas?

In terms of pressure describe why?

  • The temperature rapidly increases

pressure and temperature are directly proportional .

slide15

The values for the standard temperature and pressure (STP) are

  • P = 1 atmosphere, 760 torr
  • T = 0°C, 273 Kelvins
slide16

Convert a pressure of 1.75 atm to kPa and to mm Hg.

Convert a pressure of 570. torr to atmospheres and to kPa.

Convert a pressure of 550 mm of Hg into atm and Pa

Convert a pressure of 150. KPa to mm of Hg and atm

slide17

Convert each of the following Celsius temperatures to Kelvin temperatures

0.°C

27°C

-75.°C

-310°C.

slide19

The End!

The End!

The End!

The End!

The End!

The End!

The End!