OBJECTIVES: RATE LAW, ORDER OF REACTION, k

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KINETICS -REACTION RATES

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OBJECTIVES: RATE LAW, ORDER OF REACTION, k KINETICS LESSON 4/2/07 OBJECTIVES: RATE LAW, ORDER OF REACTION, k EXAMPLE: For the reaction below, use the experimental data provided in the table to calculate the rate law and k. 2 NO(g) + Br2(g)  2 NOBr(g) TRIAL [NO] [Br2] INITIAL RATE (MOL/Ls) #1 0.10 12 #2 0.20 24 #3 0.30 36 #4 48 #5 108

TRIAL [NO] [Br2] INITIAL RATE (MOL/Ls) #1 0.10 12 #2 0.20 24 #3 0.30 36 #4 48 #5 108 Between experiments 1 and 4 [NO] doubles. Between experiments 1 and 4 [Br2] is constant. Between experiments 1 and 4 RATE quadruples factor of 4) Between experiments 1 and 4 with [Br2] constant and [NO] doubling, the rate quadruples, NO is second order.

TRIAL [NO] [Br2] INITIAL RATE (MOL/Ls) #1 0.10 12 #2 0.20 24 #3 0.30 36 #4 48 #5 108 THE [NO] IS CONSTANT. THE [Br2] IS DOUBLED. THE RATE DOUBLES. Between experiments 1 and 2 [Br2] DOUBLES (and [NO] is constant) as the rate doubles, Br2 is first order.

CALCULATE k FROM ANY TRIAL. RATE = k[NO]2[Br2] CALCULATE k FROM ANY TRIAL. RATE = k[NO]2[Br2] USING TRIAL #1 (12 MOL L-1s-1) =k(0.10 MOL L-1)2(0.10 MOL L-1) k = 1.2 * 104 L2 /MOL2 s (♪NOTE: k has units!)