Chemistry 1B Kinetics

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  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
Updated:
2016-02-03 23:40:46
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Chemistry 1B Kinetics
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Chemistry 1B Kinetics
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Chemistry 1B Kinetics
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