2.2.4 The ideal gas equation

explain the kinetic theory of gases

that molecules in gases are constantly moving assuming

• molecules move very fast/randomly

• molecules have hardly any volume

• molecules do not attract/repel as no intermolecular forces

• no kinetic energy is lost when there are elastic collisions

• temperature is related to the average kinetic energy

define ideal gases

gases that folllow the kinetic theory of gases BUT in reality gases do not fit this description but the ones that are close are called real gases

explain how an ideal gas’ volume relies on other factors [e.g. pressure and temperature]

• when a gas is heated at constant pressure the particles gain more kinetic energy and undergo more collisions with wall

• the keep pressure constant the moleules must get further apart so volume increases

• therefore volume is directly proportional to temperature [at constant pressure]

explain the limitations of the ideal gas law

• molecules are close together

• there’s an instantanous dipole forces between molecules which pull away from container’s wall

• volume of molecules not neglible

explain why realgases do not obey the kinetic theory assumptions at low temp and high pressures

• the assumption there is zero attraction is wrong

• the assumption the gas molecule volume can be ignored is wrong

ideal gas equation

PV = nRT

pressure [Pa] x volume [m³] = moles x gas constant [8.314] x temp [K]