States of matter
• Gaseous state:
1. Kinetic particle theory of gases: all particles are in constant random
motion with the highest kinetic energy. Particles collide with one another
called elastic collision ( energy of particles remain constant and no
reaction takes place). If a particle is hitting other particles one has 10 J
energy and other has 2 J energy so after the collision the sum of energy
will still remains constant. Particles of gas are far apart and possess
negligible forces of attraction between them.
2. Size or volume of particle of gas is negligible compared to the volume of
the gas. It means there is for example 100 cm3 gas in a gas jar but the
volume of one particle in that will be much smaller.
3. Particles of gas when collide on the walls of container causes pressure.
• Gas laws:
1. Boyles law: at constant temperature of fixed mass of a gas the volume
is inversely proportional to the pressure on the gas.v=k/p so v*p=k so
boyles says that the product of pressure and volume stays constant
Given that p2 is greater than p1 so remember that p1v1=p2v2 as p1v1=k and p2v2 =k so
both are equal.
, The graph of PV is constant straight line as it is k and k remains constant.
2. Charles law: at constant pressure and for a fixed amount of gas
volume of gas is directly proportional to the temperature of the gas.
V=kT so k=V/T. Increasing the temperature increases the volume and
we can derive thus: V1/T1=V2/T2
3. Avogadros law: at constant temperature and pressure volume of the
gas is directly proportional to the number of moles of the gas.V=kn so
v/n=k hence v1/n1=v2/n2.
• Gaseous state:
1. Kinetic particle theory of gases: all particles are in constant random
motion with the highest kinetic energy. Particles collide with one another
called elastic collision ( energy of particles remain constant and no
reaction takes place). If a particle is hitting other particles one has 10 J
energy and other has 2 J energy so after the collision the sum of energy
will still remains constant. Particles of gas are far apart and possess
negligible forces of attraction between them.
2. Size or volume of particle of gas is negligible compared to the volume of
the gas. It means there is for example 100 cm3 gas in a gas jar but the
volume of one particle in that will be much smaller.
3. Particles of gas when collide on the walls of container causes pressure.
• Gas laws:
1. Boyles law: at constant temperature of fixed mass of a gas the volume
is inversely proportional to the pressure on the gas.v=k/p so v*p=k so
boyles says that the product of pressure and volume stays constant
Given that p2 is greater than p1 so remember that p1v1=p2v2 as p1v1=k and p2v2 =k so
both are equal.
, The graph of PV is constant straight line as it is k and k remains constant.
2. Charles law: at constant pressure and for a fixed amount of gas
volume of gas is directly proportional to the temperature of the gas.
V=kT so k=V/T. Increasing the temperature increases the volume and
we can derive thus: V1/T1=V2/T2
3. Avogadros law: at constant temperature and pressure volume of the
gas is directly proportional to the number of moles of the gas.V=kn so
v/n=k hence v1/n1=v2/n2.
