Boyle’s Law describes the relationship between the change in pressure and volume of a gas. For an ideal gas, the pressure and volume are indirectly proportional if the number of moles and temperature are constant. Thus, this explains why the pressure increases as the volume of a gas decreases, regardless of their differing chemical properties. Boyle’s Gas Law is commonly written as: P*V = K where, P is the pressure of the gas V is the volume of the gas K is a constant For example, if the volume of molecular oxygen halves, with temperature and number of moles remaining constant, the pressure of this particular gas should double. This phenomenon should apply to all gases, as volume is indirectly proportional to pressure. So halving the volume of molecular hydrogen, should also double the pressure it exerts. Boyle’s Gas Law has been used in conjunction with Charles’ Law and Gay-Lussac’s Law to form the Combined Gas Law, which has itself been combined with Avogadro’s Law to form the Ideal Gas Law. The Ideal Gas Law still considers the relationship between pressure and volume, but it also includes the new variables of temperature and number of moles. Thus, understanding Boyle’s law is crucial to understand how the pressure and volume of a gas are related; and by extension its function in the Ideal Gas Law.
Boyle's law focuses on external pressure. What might be the case if it focuses on the internal pressure? How would this aspect change Boyle's law?
Math and a Graph for a Physics Lab - Boyle's Law