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17 Cards in this Set
- Front
- Back
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Integrated Rate Law - 0 Order
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[A] = [A]o - Kt
Concentration = inital concentration - (rate constant * time (sec)) |
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Integrated Rate Law - 1st Order
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[A] = [A]0 *e^-kt
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Integrated Rate Law - 2nd Order
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1/[A] = kt + 1/[A]o
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Rate = ?
In terms of concentration |
Rate = k[A]^n
Where n = the order of the reactant |
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Units for 0 order reactants
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Ms^-1
or M/s |
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Units for 1st order reactants
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s^-1
or 1/s |
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Units for 2nd order reactants
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s^-1M^-1
or 1/sM |
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Rate / Concentration relationship
0 order, concentration doubles. |
Rate remains unchanged.
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Rate / Concentration relationship
1st order, concentration doubles. |
Rate doubles
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Rate / Concentration relationship
2nd order, concentration doubles. |
Rate quadruples
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Arrhenius equation
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k = Ae^-Ea/RT
Or ln(k) = ln(A) - Ea/RT |
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0 Order straight line graph
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[A] vs t
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1st Order straight line graph
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ln([A]) vs t
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2nd Order straight line graph
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1/[A] vs t
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Straight line graph, temperature change
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ln(k) vs 1/T(Temp)
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Henderson Hasselbalch equation
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Factors that facilitate reactions (Kinetics)
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Molecules must collide to react
Molecules must collide with sufficient energy Molecules must react with the correct orientation. |
