Chapter 9 Kinetic Theory of gases

Matter

Anything that occupies space and has mass

Brownian motion

The random irregular zig-zag and continuous movement of tiny particles suspended in a liquid.gas. Movement results from collisions of the tiny particles with the molecules of the liquid/gas.

Boyle’s Law

At constant temp, the volume of a fixed mass of gas is inversely proportional to its pressure

Charle’s Law

At constant pressure, the volume of a fixed mass of gas is directly proportional to its temperature measured on the kelvin scale

Combined gas law

p1v1/t1 = p2v2/t2

Ideal gas

A gas that follows all of the assumptions of kinetic theory of gases under all conditions of temp and pressure

Real gases

Real gases do not follow ideal gas law because forces of attraction/repulsion exist between molecules and the volume of a molecule compared to its volume in a gas is not negligible especially at high temperature where their volume is not negligible compared with the distances between them

Gay-Lussac’s Law of Combining Volumes

In a reaction between gases, the volumes of the reacting gases and the volumes of any gaseous products are in the ratio of small whole numbers, provided the volumes are measured at same temp and pressure

Gas

Substance that has no well defined boundaries but diffuses rapidly to fill any container in which it is placed

Diffusion

Process by which small particles move from an area of high concentration to an area of low concentration

Volatile liquid

Liquid with a low boiling pointA

Assumptions of kinetic theory of matter

All matter is made up of tiny particles that are invisible to the naked eye, these tiny particles are always in motion. The degree of motion depends on the state of the matter.

How diffusion provides evidence for the kinetic theory of matter

The observable evidence of diffusion shows that particles must be in constant motion, colliding with each other and spreading out to occupy all the available space as stated in the assumptions of the kinetic theory of matter. The only way to explain the reaction between HCL and ammonia in a closed tube is in terms of the kinetic theory of matter.