Consider the following data showing the initial rate of a reaction (a→products) at several different concentrations of a. [a](m) initial rate (m/s) 0.15 0.014 0.30 0.113 0.60 0.905. what is the order of the reaction? express your answer as an integer.

Given:

A → Products

         [A] M            Rate(M/s)

1.        0.15            0.014

2.       0.30           0.113

3.       0.60           0.905

To determine:

Order of the reaction

Explanation:

The rate of the given reaction can be expressed as:

Rate = k [A]ⁿ(1)

where k = rate constant

[A] = concentration of A

n = reaction order

Based on equation (1) the Rates 1 and 2 can be expressed as:

0.014 = k[0.15]ⁿ (3)

0.113 = k[0.30]ⁿ(4)

Dividing eq (4) by (3) we get:

0.113/0.014 = [0.30/0.15]ⁿ

8 = 2ⁿ

i.e. 2³ = 2ⁿ

n = 3

Ans: Thus, the order of the reaction is 3

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.