What is Boyle’s Law?
Boyle’s law, also known as Mariotte’s law, describes the relationship between the compression and expansion of a gas at a constant temperature. This empirical relationship, developed in 1662 by the physicist Robert Boyle, asserts that the pressure (p) of a given quantity of gas changes inversely with its volume (v) at a constant temperature; i.e., pv = k, a constant. Edme Mariotte, a French scientist, also identified the association (1676).
Boyle’s Law Definition
Boyle’s Law is defined as the volume of a fixed mass of gas is inversely proportional to its pressure at a constant temperature. This statement describes the relationship between volume and pressure.
Boyle’s Law Expression and Derivation
According to Boyle’s law, every change in the volume occupied by a gas (at constant quantity and temperature) will result in a change in the pressure exerted by the gas. In other words, the product of a gas’s beginning pressure and initial volume corresponds to its ultimate pressure and ultimate volume (at constant temperature and number of moles). This law can be represented numerically as follows:
P1V1=constant ——(i) (For state 1)
P1V1=constant ——(i) (For state 1)
Comparing equations I and (ii), we obtain P1V1 = P2V2 ——- (T = constant).
A hyperbola represents a plot of volume versus the pressure of a gas at a constant temperature (isotherm), whereas a straight line represents a plot of volume against 1/P.
Boyle’s Law Experiment Diagram
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