Temperature and number of molecules remain constant Boyle's law is a gas law, stating that the pressure and volume of a gas have an inverse relationship If volume increases, then pressure decreases and vice versa, when the temperature is held constant. Boyle’s law, a relation concerning the compression and expansion of a gas at constant temperature This empirical relation, formulated by the physicist robert boyle in 1662, states that the pressure of a given quantity of gas varies inversely with its volume at constant temperature. Scientists noted that for a given amount of a gas (usually expressed in units of moles [n]), if the temperature (t) of the gas was kept constant, pressure and volume were related
As one increases, the other decreases. Boyle's law states that, at a constant temperature, the volume occupied by a certain quantity of gas is inversely proportional to its pressure. Boyle's law is a fundamental principle in physics that describes the relationship between the pressure and volume of a gas at a constant temperature It states that the pressure of a gas is inversely proportional to its volume, provided the temperature and the amount of gas remain constant. It is summarized in the statement now known as boyle’s law The volume of a given amount of gas held at constant temperature is inversely proportional to the pressure under which it is measured.
P ∝ (1/v) where p is the pressure exerted by the gas and v is the volume occupied by it This proportionality can be converted into an equation by adding a constant, k P = k* (1/v) ⇒ pv = k. Boyle’s law states that the pressure of a gas is inversely proportional to its volume, when the temperature is kept constant In other words, as the volume of a gas decreases, the pressure increases, and vice versa. Boyle’s law is an experimental gas law that explains the relationship between pressure and volume
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