gases

• Gases

  • Described as not having a definite shape and volume
  • Have lower density
  • Gas particles collide with one another
• Force produced when the particles collide with a surface creates pressure
• Barometer – measures the atmospheric pressure
• Manometer or pressure gauge – measures the pressure in a closed system
• KINETIC MOLECULAR THEORY (KMT) OF GASES - describes the nature of gases and the behavior of the particles that comprise them; The gas consists of a minute particles (atoms or molecules)
• BOYLE’S LAW - Formulated by Irish scientist Robert Boyle; States that the pressure of a fixed amount of gas is inversely proportional to its volume at constant temperature
• GAY - LUSSAC’S LAW - Named after French chemist and physicist Joseph Gay -Lussac; States that the pressure of a fixed amount of gas is directly proportional to its absolute temperature at a constant volume
• CHARLE’S LAW - French scientist Jacques Charles together with Gay-Lussac; States that the volume of a gas is directly proportional to its absolute temperature at a constant pressure
• AVOGADRO’S LAW - By Amadeo Avogadro known for the Avogadro’s number; States that the volume of a gas is directly proportional to the number of particles at the same pressure and absolute temperature, regardless of the nature of the gas
• IDEAL GAS AND IDEAL GAS EQUATION - In relation to the Avogadro’s law ideal gas equation links all three variables (volume, temperature, and pressure) to the amount of a gas expressed in mole
• DALTON’S LAW OF PARTIAL PRESSURES - States that the total pressure of a mixture of gases in a container is equal to the sum of the partial pressures of the individual gases