SCIENCE

• Kinetic molecular theory


  Helps us understand the different properties of gases at the molecular level
• Kinetic molecular theory


  • Gases are composed of molecules
  • Distances between molecules are far greater than the molecules' dimensions
  • Molecules are in constant random motion
  • Molecules frequently collide with one another
  • Collisions between molecules are perfectly elastic
  • Attractive and repulsive forces are absent
  • Average kinetic energy of gas molecules is directly related to temperature
• Avogadro's law


  Relates the number of moles and volume of a gas, which are directly related when pressure and temperature are held constant
• Ideal gas law


  Combines Boyle's law, Charles' law, and Avogadro's law into a single equation: pV = nRT
• Units for ideal gas law: p in atm, V in L, n in mol, T in K, R = 0.0821 L·atm/mol·K
• Solids


  • More compact in nature
• Liquids


  • Particles slightly far apart compared to solids, take the shape of their container
• Gases


  • Particles very far apart, take up all the space in the container
• Properties of gases

  • Pressure (P)
  • Volume (V)
  • Temperature (T)
  • Amount (n)
• Pressure


  Force acting on a specific area
• Units of pressure


  • atm (atmosphere)
  • mmHg (millimeter mercury)
  • Torr
  • psi (pounds per square inch)
  • kPa (kilopascals)
• Volume


  Three-dimensional space occupied by a gas
• Units of volume

  • milliliters
  • liters
  • cubic meters
  • cubic centimeters
• Temperature


  Measure of the average kinetic energy of the particles in an object
• Units of temperature

  • Fahrenheit
  • Celsius
  • Kelvin
• in our calculations we will be using Kelvin as the standard unit for temperature
• Quantity


  Measured in moles, one mole is equal to 6.022 x 10^23 units of a substance
• Boyle's law relates pressure and volume at constant temperature and amount of substance
• Boyle's law


  Pressure is inversely proportional to volume at constant temperature
• Volume increases


  Pressure decreases
• Volume decreases


  Pressure increases
• Boyle's law formula


  P1 * V1 = P2 * V2
• Applications of Boyle's law

  • Action of a syringe
  • Chips bag at higher altitude
  • Breathing (diaphragm movement)
• Charles law relates volume and temperature at constant pressure
• Charles law

  Volume and temperature are directly proportional
• Volume increases


  Temperature increases
• Volume decreases


  Temperature decreases
• Charles law formula


  V1/T1 = V2/T2 (temperatures must be in Kelvin)
• Biomolecule


  Any molecule that is produced by a living organism and includes large macromolecules such as proteins, polysaccharides, lipids and nucleic acids
• Biomolecules are obtained from food
• Four main types of biomolecules

  • Carbohydrates
  • Proteins
  • Nucleic acids
  • Lipids
• Carbohydrates


  The primary energy source of our body, which are sugars
• Monomer


  Building block or smaller unit from which larger molecules are made
• Types of carbohydrate monomers (monosaccharides)

  • Glucose
  • Fructose
  • Galactose
• Disaccharide


  Double sugar formed by combining two monosaccharides
• Disaccharides


  • Maltose
  • Lactose
  • Sucrose
• Polysaccharide

  Complex sugar made up of many monosaccharides
• Polysaccharides


  • Starch
  • Glycogen
  • Cellulose
  • Chitin
• Iodine test for starch


  1. Add iodine

  2. Observe colour change to violet
• Benedict's test for simple carbohydrates

  1. Add Benedict's solution

  2. Observe colour change from blue to green, yellow, orange, red or brick red