1. Chapter 13 States of Matter
13.1 The Nature of Gases

2. Today we are learning to:- 1. Describe the kinetic theory of gases
Chemistry
Today we are learning to:- 1. Describe the kinetic theory of gases
2. Interpret gas pressure in terms of the kinetic theory
3. Define the relationship between the Kelvin temperature scale and average kinetic energy

3. The Kinetic Theory of Gases
The energy an object has because of its motion is called kinetic energy.
The kinetic theory states that all matter consists of tiny particles that are in constant motion.
The kinetic theory states:
Particles of a gas are assumed to be small, hard spheres with an insignificant volume.
The motion of the particles in a gas is rapid, constant, and random.
Collisions between particles in a gas are perfectly elastic.

5. Gas Pressure
Gas pressure results from the force exerted by a gas per unit surface area of an object.
Empty space with no particles and no pressure is called a vacuum.
Atmospheric pressure results from the collisions of atoms and molecules in air with objects.
Gas pressure is the result of simultaneous collisions of billions of rapidly moving particles in a gas with an object.

6. Gas Pressure
A barometer is a device that is used to measure atmospheric pressure.

7. Gas Pressure The SI unit of pressure is the Pascal (Pa).
One standard atmosphere (atm) is the pressure required to support 760 mm of mercury in a mercury barometer at 25°C.

8. 13.1
Gas Pressure

9. 13.1
Gas Pressure

10. for Sample Problem 13.1
Gas Pressure
What pressure in kilopascals and in atmospheres, does a gas exert at 385 mm Hg?
The pressure at the top of mount Everest is 33.7 kPa. Is that pressure greater than or less than 0.25 atm?
What pressure in mm Hg and atm, does a sample of neon gas exert at 75.0 kPa?

11. Kinetic Energy and Temperature
Atoms or molecules at a given temperature have
a wide range of kinetic energies.
most have kinetic energies somewhere in the middle of this range.
Average kinetic energy is therefore used to describe motion of particles in a substance
At a given temperature all substances have the same average kinetic energy

12. Kinetic Energy and Temperature
There is a relationship between the average kinetic energy of atoms or molecules in a sample and its temperature.
Higher kinetic energy means higher temperatures.

13. Average Kinetic Energy
Absolute zero (0 K, or –273°C) is the temperature at which the motion of particles theoretically ceases.
Particles would have no kinetic energy at absolute zero.
Absolute zero has never been produced in the laboratory.
0K = -273°C
The temperature in Kelvin of a substance is directly proportional to the average kinetic energy of the particles of the substance.

14. 1.According to the kinetic theory, the particles in a gas
13.1 Section Quiz.
1.According to the kinetic theory, the particles in a gas
are attracted to each other.
are in constant random motion.
have the same kinetic energy.
have a significant volume.

15. 2. The pressure a gas exerts on another object is caused by
13.1 Section Quiz.
2. The pressure a gas exerts on another object is caused by
the physical size of the gas particles.
collisions between gas particles and the object.
collisions between gas particles.
the chemical composition of the gas.

16. Fahrenheit temperature. Kelvin temperature.
13.1 Section Quiz.
3. The average kinetic energy of the particles in a substance is directly proportional to the
Fahrenheit temperature.
Kelvin temperature.
molar mass of the substance.
Celsius temperature.

17. END OF SHOW