Boyle's law

Examples of Boyle's law in the following topics:

• Boyle's Law: Volume and Pressure

  • Boyle's Law describes the inverse relationship between the pressure and volume of a fixed amount of gas at a constant temperature.
  • Boyle's Law (sometimes referred to as the Boyle-Mariotte Law) states that the absolute pressure and volume of a given mass of confined gas are inversely proportional, provided the temperature remains unchanged within a closed system.
  • The law was named after chemist and physicist Robert Boyle, who published the original law in 1662.
  • An animation of Boyle's Law, showing the relationship between volume and pressure when mass and temperature are held constant.
  • An introduction to the relationship between pressure and volume, and an explanation of how to solve gas problems with Boyle's Law.

• Equations of State

  • The ideal gas law is the equation of state of a hypothetical ideal gas (in which there is no molecule to molecule interaction).
  • The ideal gas law is the equation of state of a hypothetical ideal gas (an illustration is offered in ).
  • It was first stated by Émile Clapeyron in 1834 as a combination of Boyle's law and Charles' law.
  • Boyle's law states that pressure P and volume V of a given mass of confined gas are inversely proportional:
  • Therefore, we derive a microscopic version of the ideal gas law

• The Mechanics of Human Breathing

  • Boyle's Law is the gas law which states that in a closed space, pressure and volume are inversely related.
  • Due to this increase in volume, the pressure is decreased, based on the principles of Boyle's Law.
  • This graph of data from Boyle's original 1662 experiment shows that pressure and volume are inversely related.

• Isothermal Processes

  • (This is historically called Boyle's law. ) However, the cases where the product PV is an exponential term, does not comply.
  • In other words, the ideal gas law PV = nRT applies.
  • From the first law of thermodynamics, it follows that $Q =-W$ for this same isothermal process.

• Charles' and Gay-Lussac's Law: Temperature and Volume

  • Charles' and Gay-Lussac's Law states that at constant pressure, temperature and volume are directly proportional.
  • Charles' Law describes the relationship between the volume and temperature of a gas.
  • This extrapolation of Charles' Law was the first evidence of the significance of this temperature.
  • The lower a gas' pressure, the greater its volume (Boyle's Law), so at low pressures, the fraction \frac{V}{273} will have a larger value; therefore, the gas must "contract faster" to reach zero volume when its starting volume is larger.
  • Discusses the relationship between volume and temperature of a gas, and explains how to solve problems using Charles' Law.

• Kinetic Molecular Theory and Gas Laws

  • Kinetic Molecular Theory explains the macroscopic properties of gases and can be used to understand and explain the gas laws.
  • Charles' Law states that at constant pressure, the volume of a gas increases or decreases by the same factor as its temperature.
  • Boyle's Law states that at constant temperature, the absolute pressure and volume of a given mass of confined gas are inversely proportional.

• Adiabatic Processes

  • (This is historically called Boyle's law. ) However, the cases where the product PV is an exponential term, does not comply.
  • In other words, the ideal gas law PV = nRT applies.
  • From the first law of thermodynamics, it follows that $Q =-W$ for this same isothermal process.

• Isotherms

  • For an ideal gas, the product PV (P: pressure, V: volume) is a constant if the gas is kept at isothermal conditions (Boyle's law).
  • According to the ideal gas law, the value of the constant is NkT, where N is the number of molecules of gas and k is Boltzmann's constant.

• Adjustments at High Altitude

  • Due to Boyle's Law, at higher altitude the partial pressure of oxygen in the air is lower, and less oxygen is breathed in with every breath.

• Dalton's Law of Partial Pressure

  • Dalton's Law of Partial Pressure states the total pressure exerted by a mixture of gases is equal to the sum of the partial pressure of each individual gas.
  • Dalton's Law (also called Dalton's Law of Partial Pressures) states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases.
  • We know from Boyle's Law that the total pressure of the mixture depends solely on the number of moles of gas, regardless of the types and amounts of gases in the mixture; the Ideal Gas Law reveals that the pressure exerted by a mole of molecules does not depend on the identity of those particular molecules; Dalton's Law now allows us to calculate the total pressure in a system when we know each gas individual contribution.
  • From the Ideal Gas Law, we can easily calculate the measured pressure of the nitrogen gas to be 0.763 atm.