lesson 7 ppt

• Activity


  Rate of Reaction
• Reaction rate


  A measure of the change in the concentration of reactants or products over time in a chemical reaction
• Collision Theory


  • Explains how chemical reactions occur and why reaction rates differ from different reaction
• Factors Affecting Reaction Rate


  • Concentration Effects
  • Temperature Effects
  • Particle Size Effects
  • Catalyst Effects
• Concentration Effects


  The reaction rate usually increases as the concentration of the reactants increases
• Temperature Effects


  As the average kinetic energy increases, the particles move faster and collide more frequently per unit time and posses greater energy when they collide
• Particle Size Effects


  As particle size decreases, the rate of the reaction increases
• Catalyst


  A substance which speeds up a reaction but is chemically unchanged at its end
• Biological Catalyst


  Known as enzymes
• Stoichiometry


  A section of chemistry that involves using relationships between reactants and or products in a chemical reaction to determine desired quantitative data
• Balancing Equation


  It is necessary that there are the same number of atoms on the left side of the equation as the right
• If the equation is not balanced, do not change the formulas
• 6 basic types of reactions

  • Combustion
  • Combination (synthesis)
  • Decomposition
  • Single Displacement
  • Double Displacement
  • Acid-base
• Combination Reactions


  • Carbon + oxygen → carbon dioxide

  Iron fillings + sulfur powder → Iron (II) Sulfide

  Calcium Oxide + water → Calcium Hydroxide
• Decomposition Reactions


  • Potassium Chlorate → Potassium Chloride + Oxygen

  Barium Carbonate → Barium Oxide + Carbon Dioxide
• Replacement Reactions


  • Copper + silver nitrate → Copper (II) nitrate + Silver

  Bromine + Potassium Iodide → Potassium Bromide + Iodine

  Zinc + Hydrochloric Acid → Zinc Chloride + Hydrogen
• Double Replacement Reactions


  • Iron (II) Sulfide + hydrochloric Acid → Iron (II) Chloride + Hydrogen Sulfide

  Silver Nitrate + Hydrochloric Acid → Silver Chloride + Nitric Acid
• Units of Measurement


  • A ream of white bond paper (500 pcs)
  • A dozen of eggs (12 pcs)
  • A pair of hair pins (2 pcs)
  • A gross of bath soap (144 pcs)
  • A case of soft drinks (24 pcs)
• The given data have the same number or unit number of materials but different masses
• Mole Analogy


  1 mole is equal to 6.023 X10^23 particles. It could be a mole of horses, a mole of people, a mole of cars, a mole of marbles, or a mole of rice, a mole of dusts.
• Mole


  Contains the same number of particles (atom, ion, molecules). It is a specific number of chemical units.
• Molar Mass


  Useful chemical ratio between mass and moles. Atomic mass unit (amu)
• Molar Mass Calculations


  • What is the molar mass of H2O?

  What is the molar mass of NH3?

  What is the molar mass of HCl?

  What is the molar mass of KCl?
• 1 mole = 6.02X10^23 atoms, ions, molecules
• Molar Masses


  • N2O2: 28g/mol

  CO2: 44g/mol
• Mole


  Contains the same number of particles (atom, ion, molecules). It is a specific number of chemical units. It contains Avogadro's number of units or particles, which is equal to 6.02 X 10^23
• Molar Mass


  • H2O
  • NH3
  • HCl
  • KCl
• Exercise in Molar Mass


  1. Compound

  2. Elements Present

  3. No. of atoms of each element in formula X atomic mass

  4. Total mass

  5. Cu(NO3)2

  6. AgNO3

  7. SiO2

  8. C6H12O8
• 1 mole of


  • Carbon atom = 6.02 X 10^23 atoms of carbon
  • H2O = 6.02 X 10^23 molecules of water
  • NH3 = 6.02 X 10^23 molecules of NH3
• • If there is 6.02X10^23 atoms of nitrogen its mass would be 14g
  • If there is 6.02X10^23 molecules of H2O its mass would be 18g
  • If there is 6.02X10^23 molecules NH3 its mass would be 17g
• No. of Molecules


  1. 1 mol N2 = 6.02 X 10^23

  2. 1 mol O2 = 6.02 X 10^23

  3. 1 mol CO2 = 6.02 X 10^23
• No. of Moles


  1. 10g N2 = 0.36 mol

  2. 10g O2 = 0.31 mol

  3. 10g CO2 = 0.23 mol
• Mass


  1. 1 mol N2 = 28g

  2. 1 mol O2 = 32g

  3. 1 mol CO2 = 44g
• Problem Solving


  48g of ozone, 9.03 X 10^23 atoms

  2. 0.5 mol H2, 2.0 mol Ca

  3. 0.25 mol H2O, 5 mol Ca(OH)2

  4. 2.25 mol NaCl

  5. NaCl, Ca(OH)2, Cu(SO4)
• Percent by volume


  volume of solute / volume of solution x 100%
• Percent by mass


  mass of solute / mass of solution x 100%
• Molarity


  moles of solute / liters of solution
• A solution is diluted when it has a lower concentration, and concentrated when it has a higher concentration
• Percent by mass solute is the mass of solute per 100 grams of solution
• Percent by volume solute is the volume of solute per 100 mL of solution