Diffusion of gases
A few drops of liquid bromine are put into a gas jar and the lid is replaced. The liquid bromine evaporates easily. Liquid bromine is highly volatile. After a short time, the brown gas begins to spread throughout the jar. The jar becomes full of brown gas. Bromine vaporises easily and its gas will completely fill the container. Gases diffuse to fill all the space available to them. Diffusion is important for our ‘sensing’ of the world around us. It is the way that smells reach us.
Diagram info
In the digram there are 2 containers in which the brown liquid was poured called the bromine , bromine is volatile , it easily evaporates , this diagram shows the gas filled in the container
Particle info about fast moving particles slowing down
The atoms or molecules in gases move at high speeds. We are being bombarded constantly by nitrogen and oxygen molecules in the air, which are travelling at about 1800 km / hour.
However, these particles collide very frequently with other particles in the air (many millions of collisions per second), so their path is not direct. These frequent collisions slow down the overall rate of diffusion from one place to another.
The pressure of a gas is the result of collisions of the fast-moving particles with the walls of the container.
Main points in kinetic particle theory
• heavier gas particles move more slowly than lighter particles at the same temperature
• larger molecules diffuse more slowly than smaller ones
• the rate of diffusion is inversely related to the mass of the particles
• the average speed of the particles increases with an increase in temperature.
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