Diffusion And Kinetic Theory Flashcards
Diffusion
It is the net movement of particles from a high to a low concentration. It does not require energy as it moves down the concentration gradient.
The affects of the rate of diffusion
Concentration Gradient
The greater the difference in concentration, the more rapid the diffusion.
Temperature
The higher the temperature, the more kinetic energy the particles will have, so they will move and mix more quickly .
Distance
If the diffusion distance is small, diffusion happens faster because the particles do not have as far to travel.
Surface Area
The larger the surface area the higher the number of particles that will be able to move in a given time so the faster the rate.
Shape and size
The smaller the molecules will diffuse quicker than larger molecules, and molecules with a more streamlined shape (long thin molecules) will diffuse quicker
The arrangement of particles in solids
Particles in solids are touching each other and in fixed positions.
In a solid the particles can vibrate in all directions but cannot move out of their fixed positions
Liquids
Particles in liquids are close together, rolling over each other and arranged randomly.
In a liquid, the particles move randomly can slide past each other, but they do not move far.
Gases
Particles in gases are far apart and arranged randomly.
In a gas, the particles move around quickly and can travel large distances in all directions. The molecules in a gas are constantly hitting each other and the walls of their container, causing them to change direction.
Kinetic theory
The kinetic theory is concerned with the motion of particles in solids, liquids and gases.
The particles in solids, liquids and gases at any temperature above absolute zero will all exhibit some form of movement. At absolute zero, all movement of particles stops.
Dynamic equilibrium
When two processes take place at the same rate there is no further change in concentration of the substances.
