The initial rates for the reaction A + B C at varyinginitial concentrations of A

Question

The initial rates for the reaction A + B C at varyinginitial concentrations of A and B are given below:
Exp. [A]0 (M) [B]0 (M) Initial Rate (M/s) 1 0.040 0.060 1.20×10-6 2 0.080 0.060 4.80×10-6 3 0.160 0.060 1.92×10-5 4 0.040 0.240 6.00×10-7 5 0.040 0.960 3.00×10-7 Determine the order of the reaction for reactantA and the overall reaction order.
Partial order of A:
Overall order: Incorrect. Tries 1/8 PreviousTries
Calculate the rate constant for the reaction.Remember that the units for the rate of the reaction should be inM/s, and the units for the rate constant are defined accordingly.If your answer is 1.0 M1/2·s-1, type:1.0 M^0.5*s^- Exp. [A]0 (M) [B]0 (M) Initial Rate (M/s) 1 0.040 0.060 1.20×10-6 2 0.080 0.060 4.80×10-6 3 0.160 0.060 1.92×10-5 4 0.040 0.240 6.00×10-7 5 0.040 0.960 3.00×10-7

Explanation / Answer

We Know that :       The given Reaction is :          A + B------> C          Rate = K [A]x [B]y      From the given experimental data:             Divide theexperimental value 2 by 1 we get         (2)x = 4                 = (2)2           bycomparing the values          x =2       Divide the experimental value 5by 4 we get :         (4)y = 1 / 2            (2 )2y = 2-1              y = - 1/ 2      From the values of x and y we canwrite the Rate law as :          Rate = K [A]2 [B]-1/2           Order with respect to A is 2           OverallOrder of the Reaction = 2 + (-1/2)                                                         = 3 / 2       K = Rate / [A]2 [B]-1/2             = 1.20 x 10-6 / [0.040]2[0.060]-1/2               = 1.84 x 10-4 M^-0.5.s^-               = 1.84 x 10-4 M^-0.5.s^-

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