Boyle’s law graph?
The relationship between volume and pressure (Boyle-Mariotte’s Law)
The law Boyle describes the relationship between pressure and volume of a gas. It stipulates that, at constant temperature, the volume occupied by a certain quantity of gas is inversely proportional to its pressure.
The Irish physicist and chemist Robert Boyle (1627-1691) and the French physicist Edme Mariotte (1620-1684) have shown that there is a relationship between the pressure and the volume of a gas. At a constant temperature and for the same number of molecules, they observed that the pressure of a gas increases when its volume decreases, and vice versa. The opposite is also true: a decrease in the volume of a gas results in an increase in its pressure. This relationship is called Boyle-Mariotte’s Law.
The volume of a gas is therefore inversely proportional to its pressure. For example, doubling the gas pressure will reduce the volume by half. This variation can be explained by the kinetic theory of gas . At constant temperature, if the external pressure exerted on a gas increases, the volume of it decreases. As a result, the gas particles become closer and clash further. As a result, collisions are more frequent, which increases the pressure. Conversely, if the volume of the container is increased, the collision frequency is lower and the pressure of the gas becomes lower.
The graph of pressure versus volume forms a typical curve of an inversely proportional relationship. We can therefore say that the pressure is directly proportional to the inverse of the volume. Mathematically, we can write this relation as follows:
As the product of the pressure by the volume is equal to a constant, one can compare two situations for the same gas, as long as the quantity of gas and the temperature do not vary. This results in the following relation: