Gas Laws

• Robert Boyle used a J-shaped glass tube partially filled with mercury. He published the original law in 1662. He discovered that doubling the pressure of gas while keeping its temperature constant caused the volume to be reduced by half.
• Boyle's law states that the volume of the gas varies inversely with pressure. It can be mathematically expressed as P1V1 = P2V2.
• Boyle's law application

  • working on medical syringe
  • storage of gas under pressure
  • inflating tire using pump
  • scuba diving
  • breathing of air
• Jacques Charles was remembered for his pioneering work with gases and hydrogen balloon flights.
• Charle's law states that the volume of a fixed amount of gas maintained at constant pressure is directly proportional to its absolute kelvin temperature. It can be mathematically expressed as V1T2=V2T1.
• Charles' law application

  • baking bread
  • fixing a dented ping-pong ball
  • exploding tires during summer
  • blasting of balloons on a hot day
  • flying hot air balloon
• Joseph Louis Gay-Lussac is credited with the determination of the temperature-pressure relationship in gases at constant volume.
• • Gay-Lussac's law states that at constant volume, the pressure of a fixed mass of gas is directly proportional to the absolute temperature. It can be mathematically expressed as P1T2=P2T1.
• Ideal Gas Law is also known as the general gas equation. For a gas to be "ideal", there are four governing assumptions. The gas particles: have negligible volume, are equally sized, do not have intermolecular forces (attraction or repulsion), and move randomly.
• Benoit Paul Emile Clapeyron discovered the ideal gas law equation in 1834 by combining several gas laws.
• Avogadro's law states that the number of moles is directly proportional to the volume of a gas.
• Ideal gas law can be mathematically expressed as PV=nRT.