A) Use the following reaction data to determine the general form of the rate law

Question

A) Use the following reaction data to determine the general form of the rate law for the reaction A + B --> products.

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

1) 0.050 0.050 0.00077

2) 0.025 0.050 0.00039

3) 0.050 0.100 0.00077

B) For the experiment run in question 1, what is the overall order of the reaction? I

C) if a reaction is first order and the concentration of the reactant is doubled, what happens to the rate?

D) In this lab, the absorbance measurement is being used instead of concentration for each reactant. Will this affect the results for the orders determined by the reaction? Why or why not?

Explanation / Answer

A) For experiment runs 1 and 2, the concentration of [A] is halved and [B] is kept same. The rate also decreases by half. So, the order of the reaction with respect to A is 1.

For experiment runs 1 and 3, the concentration of [B] is doubled and [A] is kept same. The rate remained same. So, the order of the reaction with respect to B is 0.

Rate law:

rate = k [A]1 [B]0

B) overall Order = 1+ 0 = 1

C) If the order of the reaction is one and the concentration of the reactant is doubled, then the rate will also double.

D) If the absorbance measurement is done instead of concentration, even then the order determined will be same. Because the absorbance is directly proportional to concentration according to Beer Lambert Law. As the concentration changes, the absorbance will also change with same magnitude.

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