GAS LAWS 4TH

• Boyle's Law states that at a fixed temperature, the product of pressure and volume remains constant when one changes while the other stays the same.
• Chemical equation


  Describes a chemical change
• Parts of a chemical equation


  • Reactant
  • Reaction symbol
  • Product
• Reactant


  The chemical(s) you start with before the reaction, written on the left side of the equation
• Product


  The new chemical(s) formed by the reaction, written on the right side of the equation
• Subscript


  Shows how many atoms of an element are in a molecule
• Coefficient


  Shows how many molecules there are of a particular chemical
• A chemical reaction


  Matter is neither created nor destroyed, the number and type of atoms going into the reaction must be the same as the number and type of atoms coming out
• If an equation obeys the Law of Conservation, it is balanced
• Unbalanced equation


  • CH4 + O2 → CO2 + H2O
• Rules for balancing chemical equations


  • Matter cannot be created or destroyed
  • Subscripts cannot be added, removed, or changed
  • You can only change coefficients
  • Coefficients can only go in front of chemical formulas, never in the middle
• Gay-Lussac's Law states that if the volume is kept constant, then the pressure will increase with increasing temperatures.
• Charles' Law states that as the temperature increases, the volume also increases proportionally.
• Boyle's Law


  The volume of a gas decreases with an increase of pressure, and vice versa

  
• Robert Boyle


  • 17th-century pioneer of modern chemistry
  • Discovered Boyle's law
• Robert Boyle was born


  1627
• Robert Boyle passed away


  1619
• Laws


  Generalizations or universal relationships related to the way that some aspect of the natural world behaves under certain conditions
• Ideal gas


  Volume x Pressure = Constant

  
• Hypothesis


  A tentative explanation that forms the foundation for further investigations
• Real gas


  Volume x Pressure = Constant

  
• Theory


  A broad explanation that has been supported with data and is a well substantiated, consistent explanation for a natural occurrence
• Simulation


  • http://www.physics-chemistry-interactive-flash-animation.com/matter_change_state_measurement_mass_volume/pressure_volume_boyle_mariotte_law_ideal_gas_closed_system_MCQ.htm

  
• Postulates of the Kinetic Theory of Gases


  • Particles in a gas have no volume and are very far apart
  • Particles in a gas move in straight line paths and random directions
  • Particles in a gas collide frequently with the sides of the container and less frequently with each other. All collisions are elastic (no energy is gained or lost as a result of the collisions)
  • Particles in a gas do not attract or repel one another. There is no intermolecular attractions
  • The average kinetic energy of all of the gas particles in a sample is proportional to the temperature of that gas sample
• Temperature


  A measure of the average kinetic energy of a substance

  
• Converting between Celsius and Kelvin


  1. Celsius to Kelvin: K = oC + 273

  2. Kelvin to Celsius: oC = K - 273
• Converting temperature


  • -167oC to Kelvin
  • 1100oC to Kelvin
  • 321 Kelvin to Celsius

  
• Units of pressure


  • 1 atmosphere (atm)
  • 760 mm Hg
  • 14.7 psi
  • 101.3 kPa

  
• Converting pressure units


  1. 1.55 atm to kPa

  2. 1.45 atm or 1000 mm Hg

  3. 753 psi to atmospheres
• Standard Temperature & Pressure (STP)


  1 atm at 0°C
• Pressure and the number of gas molecules


  Doubling the number of molecules of a gas, doubles the pressure
• Pressure and volume


  In a smaller container, molecules have less room to move & hit the sides of the container more often, creating pressure
• Temperature and pressure/volume


  Increase in temperature causes gas molecules to hit the walls of the container harder, resulting in either increased pressure or increased volume
• Dalton's Law of Partial Pressure

  The total pressure inside a container is equal to the partial pressure due to each gas

  
• Dalton's Law of Partial Pressure


  • Finding the total pressure in a balloon filled with air if the pressure of the oxygen is 170mmHg and the pressure of nitrogen is 620 mmHg
  • Finding the pressure of oxygen if the total pressure is 1.3 atm and the pressure of nitrogen is 720 mmHg