Question

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions:

Experiment	[A] (M)	[B] (M)	Rate (M/s)
1	0.8	0.8
2	1.6	0.8

(a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]^x [B]^y? Choose all correct possibilities.

[A] = 3.2 and [B] = 0.8

[A] = 0.8 and [B] = 2.4

[A] = 4.0 and [B] = 0.8

[A] = 1.6 and [B] = 0.8

[A] = 0.8 and [B] = 1.6

[A] = 1.6 and [B] = 2.4

[A] = 2.4 and [B] = 0.8

[A] = 1.6 and [B] = 1.6

(b) For a reaction of the form, A + B + C --> Products, the following observations are made: doubling the concentration of A increases the rate by a factor of 2, doubling the concentration of B has no effect on the rate, and doubling the concentration of C increases the rate by a factor of 2. Select the correct rate law for this reaction from the choices below.

Rate = k[A][B][C]

Rate = k[A][C]   

Rate = k[A]² [C]

Rate = k[A][C]²

Rate = k[A]² [C]²

Rate = k[A]³ [C]

Rate = k[A][C]³

(c) By what factor will the rate of the reaction described in part (b) above change if the concentrations of A, B, and C are all halved (reduced by a factor of 2)?

The rate will be the original rate multiplied by a factor of  .

Answer 1

(a rate = K[A]" (BJY CAJ=1.6M, [B] = 0.89 (b) concentration of A double = rate double order with respect to A= 1 concentration of B double = no effect order with respect to B =0

concentration of cdouble a rate double them, order with respect to c= 1 rate = k LAJ'CB7°lgt rate = kCAJ[J concentraction of A, B, C are halved. rate' = K CAL] [%] ratés k CAICO rate'- I KCA] [c] Irate'= txfrate?