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Unformatted text preview: [1.00] y =   =  =  2 = 2 y y = 1 Rate2 k[NO] 2 x [Cl 2 ] 2 y 4.56 k[1.00] x [0.50] y 4.56 [0.50] y Rate law: Rate = k[NO] 2 [Cl 2 ] 1 The order in each reactant is the power to which that concentration is raised. Thus, this reaction is second order in NO and first order in Cl 2 . The over all order is the sum of the orders of the different reactants, thus 2 + 1 or third order over all. The value of k is found by solving the rate equation for k and then substituting in the numbers for a given trial. If the rate law is correct, all of the trials will give the same value of k Rate k =  For trial 1 k = 1.14/(0.50) 2 (0.50) = 9.12 [NO] 2 [Cl 2 ] Substituting in the data for trials 2 and 3 will also give the same value for the rate constant....
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This note was uploaded on 04/03/2008 for the course CHEM 114 taught by Professor Martin during the Spring '08 term at Moravian.
 Spring '08
 Martin
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