Boyle's Law

• Gas


  One of the three forms of matter, has neither a fixed shape nor a fixed volume, and has weight
• Properties of gases


  • Most gases exist as molecules (in case of inert gases as individual atoms)
  • The molecules of gases are randomly distributed and are far apart
  • Gases can be easily compressed, the molecules can be forced to be closed together resulting to lesser space between them
  • The volume or space occupied by the molecules themselves is negligible as compared to the total volume of the container so that the volume of the container can be taken as the volume of the gas
  • Gases have lower densities than solids and liquids
  • The attractive forces between molecules (intermolecular) are negligible
  • Most substances that are gaseous at normal conditions have low molecular mass

  
• Measurable properties of gases

  • Pressure
  • Volume
  • Temperature
  • Amount of gas
  • Density

  
• Standard Temperature and Pressure (STP) or Standard Conditions (SC)


  T = 0 0C = 273 0K, P = 1 atm or its equivalents
• Kinetic Molecular Theory


  All matter is made of constantly moving atoms or molecules, they possess kinetic energy, they collide with one another and with the sides of the container, the average kinetic energy of the molecules is directly proportional to the absolute temperature

  
• Boyle's Law

  The relationship between the volume and pressure of a gas sample at constant temperature: volume is inversely proportional to pressure

  
• Boyle's Law Equation

  V ∝ 1/P at constant T and n
• Boyle's Law Working Formula

  P1V1 = P2V2
• Practical applications of Boyle's Law


  • Inflating tyres
  • Breathing
  • Soda bottle
  • Working of a syringe
• At a given temperature, the product of the pressure and volume of a gas must be constant. If the pressure is increased, the volume must decrease to maintain the constant product.