How are the macroscopic characteristics of a gas related to the behaviour of individual molecules?
What assumptions and observations lead to universal gas laws?
How can models be used to help explain observed phenomena?
How does the concept of force and momentum link mechanics and thermodynamics?
How does a consideration of the kinetic energy of molecules relate to the development of the gas laws?
How can gas particles of high kinetic energy be used to perform work?
What other simplified models are relied upon to communicate the understanding of complex phenomena? (NOS)
pressure as given by P = F/A, where F is the force exerted perpendicular to the surface
the amount of substance n, and the relationship between the number of moles, molecules and the Avagadro constant
that ideal gases are described in terms of the kinetic theory and constitute a modelled system used to approximate the behaviour of real gases
that the ideal gas law equation can be derived from the empirical gas laws for constant pressure, constant volume and constant temperature as given by PV/T = constant
the equations governing the behaviour of ideal gases as given by PV = NkBT and PV = nRT
that the change in momentum of particles due to collisions with a given surface gives rise to pressure in gases and, from that analysis, pressure is related to the average (translational speed)2 of molecules as given by P =(1/3)ρv2
the relationship between the internal energy U of an ideal monatomic gas and the number of molecules or amount of substance as given by U =(3/2)NkT or U =(3/2)RnT
the temperature, pressure and density conditions under which an ideal gas is a good approximation of a real gas.
