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Reactivity 2. How much, how fast and how far?

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  1. 2.1 Amount of chemical change

    1. 2.1.1Chemical equations

      • Show ratio of reactants and products • Deduce balanced equations, including state symbols, from named reactants and products

    2. 2.1.2Mole ratio

      • Determine masses, volumes, concentrations • Use balanced equations for reacting quantity calculations

    3. 2.1.3Limiting reactant

      • Determines theoretical yield • Identify limiting and excess reactants from given data

    4. 2.1.4Percentage yield

      • (Experimental yield / Theoretical yield) × 100% • Solve problems involving theoretical, experimental, and percentage yields

    5. 2.1.5Atom economy

      • Measure of green chemistry efficiency • Calculate atom economy and link low atom economy to waste

  2. 2.2 Rate of chemical change

    1. 2.2.1Rate of reaction

      • Change in concentration per unit time • Determine rates from tangents of concentration, volume, or mass graphs

    2. 2.2.2Collision theory

      • Sufficient energy + proper orientation required • Kinetic energy and temperature (Kelvin) • Explain successful collisions using activation energy and orientation

    3. 2.2.3Factors affecting rate

      • Pressure, concentration, surface area, temperature, catalyst • Predict and explain rate changes when conditions change

    4. 2.2.4Activation energy (Ea)

      • Minimum energy for successful collision • Maxwell-Boltzmann distribution curves • Use Maxwell-Boltzmann curves to show temperature effects on successful collisions

    5. 2.2.5Catalysts

      • Provide alternative pathway with lower Ea • Energy profiles with/without catalysts • Explain catalyst effects on energy profiles and Maxwell-Boltzmann distributions

  3. 2.3 Extent of chemical change

    1. 2.3.1Dynamic equilibrium

      • Forward rate = backward rate (closed system) • Describe physical and chemical systems at equilibrium

    2. 2.3.2Equilibrium law

      • K determined from stoichiometry • Deduce K expressions for homogeneous reactions

    3. 2.3.3Equilibrium constant (K)

      • Magnitude indicates extent of reaction • Temperature dependent • Kreverse = 1/Kforward • Interpret K << 1, K < 1, K = 1, K > 1, and K >> 1

    4. 2.3.4Le Châtelier's principle

      • Predict effects of changes in concentration, temperature, pressure • Include effects on K and equilibrium composition