Chemistry 1B Kinetics

  1. reaction rates:
    the change of the concentration of the reactants and products over a given time
  2. rate orders:
    equation:
    parameter determined experimentally that relates reaction rates to concentration of the reactants
  3. rate constant (k):
    probability constant that relates reaction concentration to rate
  4. rate law:
    rate=k[A][B]2 (would be third order)

    an equation that defines the relationship between reaction concentration and rate
  5. equation to determine rate order for "hard case"
    chart?chf=bg,s,00000000&cht=tx&chl=n%3D%5Cfrac%7Blog%20%5Cfrac%7BRate%201%7D%7BRate%202%7D%7D%7Blog%5Cfrac%7B%5BB%5D_1%7D%7B%5BB%5D_2%7D%7D&chs=186x148
  6. 1st order reaction integrated rate law equation:
    Also, how to plot and what it would look like
    • chart?chf=bg,s,00000000&cht=tx&chl=ln%20A_%3D-kt%2Bln%20A_0&chs=258x36
    • •plot ln(A) vs time
    • if 1st order:  the slope is negative (-k) and it's a straight line
  7. half life 1st order reaction equation:
    chart?chf=bg,s,00000000&cht=tx&chl=t_1_%2F_2%3D%5Cfrac%7B0.693%7D%7Bk&chs=164x66
  8. 2nd order reaction integrated rate law:
    also, how to plot and what it would look like
    • chart?chf=bg,s,00000000&cht=tx&chl=%5Cfrac%7B1%7D%7BA%7D%3Dkt%2B%5Cfrac%7B1%7D%7BA_0%7D&chs=178x70
    • •plot 1/A vs time
    • if 2nd order: the slope is positive (+k) and it's a straight line
  9. half life 2nd order reaction equation:
    chart?chf=bg,s,00000000&cht=tx&chl=t_1_%2F_2%3D%5Cfrac%7B1%7D%7Bk%5BX%5D_0%7D&chs=172x80
  10. zero order reaction equation
    Also, plot
    • chart?chf=bg,s,00000000&cht=tx&chl=%5BA%5D%3D-kt%2B%5BA%5D_0&chs=248x46
    • •plot [A] vs time
    • if zero order slope is negative (-k) and linear
  11. half-life zero order reaction equation:
    chart?chf=bg,s,00000000&cht=tx&chl=t_1_%2F_2%3D%5Cfrac%7B%5BX%5D_0%7D%7B2k%7D&chs=156x82
  12. Arrhenius equation:
    • chart?chf=bg,s,00000000&cht=tx&chl=k%3DAe%5E%7B-Ea%2FRT%7D&chs=218x38
    • where R=8.314 J/mol K
    • T= temperature in K
    • Graphic Ea determination:chart?chf=bg,s,00000000&cht=tx&chl=ln%20k%20%3D%5Cfrac%7B-E_a%7D%7BR%7D(%5Cfrac%7B1%7D%7BT%7D)%2BlnA&chs=312x72
    • point method: chart?chf=bg,s,00000000&cht=tx&chl=ln(%5Cfrac%7Bk_1%7D%7Bk_2%7D)%20%3D%5Cfrac%7BE_a%7D%7BR%7D(%5Cfrac%7B1%7D%7BT_2%7D)-%5Cfrac%7BE_a%7D%7BR%7D(%5Cfrac%7B1%7D%7BT_1%7D)&chs=382x76

    chart?chf=bg,s,00000000&cht=tx&chl=ln(%5Cfrac%7Bk_1%7D%7Bk_2%7D)%3D%7B%5Cfrac%7BE_a%7D%7BR%7D(%5Cfrac%7B1%7D%7BT_2%7D-%5Cfrac%7B1%7D%7BT_1%7D)&chs=314x76
  13. define catalyst
    • increases rate of reaction without being consumed in reaction.
    • Also, you can increase your energy in the beginning and lower your transition state energy from different, more stable complexes
Author
kjel
ID
314992
Card Set
Chemistry 1B Kinetics
Description
Chemistry 1B Kinetics
Updated