Chp 8 Gas Laws and equation Flashcards
Gas Law and volatile liquid experiment
Boyle’s law
For a fixed mass of a gas at constant temperature the pressure of the gas is inversely proportional to it’s volume
PV=K
P ₁V ₁=P₂V₂
Charles’ Law
For a fixed mass of a gas at constant pressure the volume of the gas is directly proportional to its temperature in Kelvins
V/T=K
V₁/T₁=V₂/T₂
Combined gas law
PV/T=K
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 te same teamperature and pressure
Ideal gases
A gas which obeys the kinetic theory of gases at all conditions of temperature and pressure
PV=nRT
Kinetic Theory of Gases
1st
Gas particles are in rapid, random straight line motion colliding with each other and with the wall of the container
Kinetic Theory of Gases
2nd
The collisions between gas particles are elastic - Particles don’t lose energy when they collide
Kinetic Theory of Gases
4th
The average kinetic energy of gas particles is directly proportional to their temperature in Kelvin.
Kinetic Theory of Gases
3rd
The distance between gas particles are so large relative to the volume of the gas particles, that we say that gas particles don’t have a volume. They are called point masses
Kinetic Theory of Gases
5th
There are no forces of attraction or repulsion between gas particles
Volatile
Evaporates easier
Avogadro’s Law
states that equal volumes of gases contain equal numbers of molecules under the same conditions of temperature and pressure
Relative atomic mass
The average of the masses of all the naturally occurring isotopes of an atom, taking into account their abundance relative to 1/12th of the mass of a carbon 12 atom
