Question

Considering the following rate data, what is the order of the reaction with respect to [A] in the reaction? A+B -> 30 Trial [A] (M) 1 0.20 2 0.40 3 0.20 [B] (M) 0.10 0.10 0.20 [C] (M/min) 5.0 20. 10. C 2nd order C 4th order C 3rd order C 1st order zero order

Answer 1

The reaction is as follows:

A + B $\rightarrow$ 3C

The rate of the reaction is expressed as follows:

Rate = k [A]^x [B]^y ------Here, x and y are the order of the reaction with respect to A and B respectively.

Use trial (1) and trail (2) and determine the value of x as follows:

Rate₂ / Rate₁ = k [A₂]^x [B₂]^y / k [A₁]^x [B₁]^y

Substitute 20 for Rate₂, 5.0 for Rate₁, 0.40 for A₂, 0.10 for B₂, 0.20 for A₁ and 0.10 for B₁. Determine the value of x as follows:

20. / 5.0 = k [0.40]^x [0.10]^y / k [0.20]^x [0.10]^y

4 = [2]^x

2² = 2^x

x = 2

Thus, from the rate law, x is the order of reaction with respect to A.

Thus, the reaction is 2^nd order(second-order) with respect to reactant A.