Lecture10_S08

Lecture10_S08 - Feb 11 2008 Lecture 10 Chapter 15...

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Feb. 11, 2008 Lecture 10, Chapter 15: Equilibrium In the previous chapter we discussed reactions that went to “completion” after a certain amount of time A B [A] time Initial concentration At some time later [A] t 0 Rate = k[A] m We could quantify how fast by finding the rate law: Found by comparing rates with different initial concentrations ln [A] time To find k, do plots…. Straight line = 1 st order Slope = -k If not straight line then rxn is NOT 1 st order
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k = Ae -Ea/RT Activation Energy Whole term = fraction of molecules with energy greater than activation barrier energy energy Time Time A B A B E a forward exothermic endothermic A B E a forward E a reverse E a reverse Or (rxn coordinate) Or (rxn coordinate) If enough energy is present (as is typical for endothermic cases) the reactions will run backwards as well! This is a fairly common situation in exothermic reactions as well Some overall both processes are normally active in most reactions A B k f k rev
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Lecture10_S08 - Feb 11 2008 Lecture 10 Chapter 15...

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