13 FoC Activation Energy

# 13 FoC Activation Energy - Learning from last time predict...

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1 1 Learning from last time: predict a rate law! What is the rate law predicted by the following mechanism for the reaction Cl 2 + CO COCl 2 assuming that equilibrium is established in both Steps 1 and 3. Step 1 fast: Cl 2 + CO COCl + Cl Step 2 slow: COCl + Cl 2 COCl 2 + Cl Step 3 very fast: Cl + Cl Cl 2 A) Rate = k[Cl 2 ] 3/2 [CO] B) Rate = k[COCl][Cl 2 ] C) Rate = k[Cl] 2 [CO][Cl] 1 D) Rate = k[Cl 2 ][CO] 2 Solution Step 1 fast: Cl 2 + CO COCl + Cl Step 2 slow: COCl + Cl 2 COCl 2 + Cl Step 3 very fast: Cl + Cl Cl 2 ] [ ] [ / ] [ ] [ : ] [ ] [ : 3 ] [ ] ][ [ ] [ : ] ][ [ ] ][ [ : 1 ] ][ [ 2 2 / 3 2 2 / 1 3 2 / 1 2 2 2 3 2 1 2 1 2 2 CO Cl k Rate So K Cl Cl Substitute Cl Cl K m Equilibriu Step Cl CO Cl K COCl Substitute CO Cl Cl COCl K m Equilibriu Step Cl COCl k Rate Step eq eq eq eq

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2 3 Chemical Equilibrium Review Overall balanced reaction equation: aA + bB cC + dD Gibbs free energy change: G = G o + RTln(Q) At equilibrium G = 0, Q = K eq ln(K eq ) = – G o /RT      b a d c B A D C Q K cannot have units! 4 Overall balanced reaction equation: aA + bB cC + dD Equilibrium concentrations satisfy an equilbrium constant condition:      b a d c eq eq eq eq eq B A D C K Textbook uses K o eq to emphasize that the concentrations actually are activities, which = concentration / 1M
3 5 Chemical Kinetics Review How reactions occur and why they depend on concentration and temperature. How the Chemical Kinetics game is played! Measure how the reaction rate changes with

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## This note was uploaded on 03/29/2010 for the course CHE 132 taught by Professor Hanson during the Spring '08 term at SUNY Stony Brook.

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13 FoC Activation Energy - Learning from last time predict...

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