Chapter 8 - Gases

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created 6 years ago by kstrand
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Chemistry
Chapter 8
updated 6 years ago by kstrand
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1

Conversion factors for pressure

1 atm = 760 mmHg

760 torr = 760 mmHg

1 atm = 14.7 lb./in. (psi)

1 atm = 101.325 kPa

2

#1 Kinetic molecular theory of gas

A gas consists of small particles that move randomly with high velocities.

3

#2 Kinetic molecular theory of gas

The attractive forces between the particles of gas are usually very small.

4

#3 Kinetic molecular theory of gases

The actual volume occupied by gas molecules is extremely small compared with the volume that the gas occupies.

5

#4 Kinetic molecular theory of gases

Gas particles are in constant motion, moving rapidly in straight paths.

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#5 Kinetic molecular theory of gases

The average kinetic energy of gas molecules is proportional to the Kelvin temperature.

7

Boyle's Law

P1V1 = P2V2

Pressure and Volume

If pressure increases, volume decreases and vice versa.

8

Charle's Law

V1/T1 = V2/T2

Temperature and Volume

If temperature increases, then volume increases and vice versa.

9

Gay-Lussac's Law

P1/T1 = P2/T2

Temperature and Pressure

if temperature increases, then pressure increases, and vice versa.

10

The Combined Gas Law

P1V1/T1 = P2V2/T2

11

V1/n1 = V2/n2

Volume and Moles

12

Dalton's Law

PT = P1 + P2 + P3 + . . .

Partial Pressure

13

Molar Volume

22.4 L = 1 mole of gas at STP