Lec 02 Jan 7 Wed

# Lec 02 Jan 7 Wed - To determine the order of the reaction...

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To find m, ratio law from exp. 1 and 3 where [Cl 2 ] is the same 0.189 0.021 = k (0.300) m (0.100) n k (0.100) m (0.100) n 9.00 = (3.00) m m = 2 2) To find n, ratio law from exp. 1 and 2 0.042 0.021 = k (0.100) 2 (0.200) n k (0.100) 2 (0.100) n 2.00 = (2.00) n n = 1 1.4 Therefore: Rate law = k [NO] 2 [Cl 2 ] It just happened that m and n are also the coefFcients in the reaction … BUT you can’t assume this is always true! Notice that you may have used another set of coefFcients, e.g. NO(g) + 1/2 Cl 2 (g) NOCl(g) ) Rate law is: Rate = k [NO] m [Cl 2 ] n 2 NO (g) + Cl 2 (g) 2 NOCl (g) Initial : [NO] [Cl 2 ] Initial Rate (M/s = mol/Ls) Expt 1 0.100 0.100 0.021 2 0.100 0.200 0.042 3 0.300 0.100 0.189 To determine the order of the reaction, run several experiments under different reactant concentrations, and measure the initial rates. *** Sometimes you don’t have two experiments with the same concentration for a species. Put the different values into the rate laws, and solve for the exponent.

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Lec 02 Jan 7 Wed - To determine the order of the reaction...

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