Intro-to-Gasses-and-Gas-laws

• The pressure exerted by the gas is directly proportional to its density.
• Density can be calculated using the formula: Density = Mass / Volume
• Pressure = Density x Acceleration due to gravity
• States of Matter


  • The forces (inter/intramolecular) holding particles together
  • The kinetic energy present (the energy an object possesses due to its motion of the particles)
• Kinetic Energy


  Tends to 'pull' particles apart
• As temperature increases


  Gas particles move faster, and thus kinetic energy increases
• Gases


  • Expand to fill any container
  • Random motion, no attraction
  • Fluids (like liquids), no attraction
  • Very low densities, no volume = lots of empty space
• Charles's law states that the volume occupied by a given mass of gas varies directly with absolute temperature (Kelvin scale) when the pressure remains constant.
• According to Dalton's Law, the total pressure of a mixture of gases is equal to the sum of pressures that would have been produced if each gas were alone at the same temperature and volume.
• Charles' law states that when the pressure on a fixed mass of gas remains constant, the volume occupied by the gas varies directly as the absolute temperature.
• Boyle's law states that when the pressure on a fixed mass of gas remains constant, the volume occupied by the gas varies inversely with the absolute pressure.
• Boyle's law states that when the pressure on a fixed mass of gas increases, the volume decreases proportionally; conversely, as the pressure decreases, the volume increases.
• According to Dalton's Law, when two or more gases are mixed together at constant temperature and volume, their total pressure will equal the sum of the partial pressures of all individual gases present.
• Partial Pressure (P) = Partial Pressure of Gas A + Partial Pressure of Gas B + ...
• Total Pressure (Pt) = P1 + P2 + ...
• Avogadro's hypothesis states that all gases contain the same number of molecules per unit volume under similar conditions of temperature and pressure.
• According to Dalton's Law, the total pressure of a mixture of gases is equal to the sum of pressures that would have been produced if each gas were alone at the same temperature and volume.
• Boyle’s Law states that the pressure exerted by a fixed amount of gas held at a constant temperature is inversely proportional to the volume it occupies.
• Boyle’s law states that the pressure exerted by a confined gas is inversely proportional to its volume; or, the product of the pressure and volume of an enclosed gas is always a constant quantity.
• Avogadro's hypothesis states that all gases contain an equal number of molecules per unit volume under identical conditions of temperature and pressure.
• The total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of its constituent gases.
• Avogadro's number is approximately 6.02 x 10^23 particles per mole.
• Avogadro’s hypothesis states that all gases contain the same number of molecules per unit volume under similar conditions of temperature and pressure.
• Dalton's Law states that the total pressure exerted by a mixture of nonreactive gases is equal to the sum of the partial pressures of each component gas.
• The ideal gas equation relates the pressure, volume, amount of substance, and temperature of a gas according to PV=nRT where P is pressure, V is volume, n is moles, R is the universal gas constant, T is temperature.
• The equation for Charles' Law is V1/T1=V2/T2.
• The ideal gas equation relates the pressure, volume, and temperature of a gas through the following formula: PV=nRT
• Charles' Law states that as the temperature of a gas increases, its volume also increases, provided that the pressure remains constant.
• Charles’ Law states that when a gas is kept at a constant pressure, its volume increases as its absolute temperature rises.
• The equation for Boyle's law is P1V1=P2V2.
• The ideal gas equation is represented by the formula PV=nRT.
• Dalton’s Law of Partial Pressure states that when two or more gases are mixed together in a container, the total pressure exerted by the mixture is equal to the sum of the individual partial pressures of each component gas.