Question

Compounds 'A' and 'B' react according to the following
chemical equation.
A(g) + 2B(g) → 2C(g)
Concentration of either 'A' or 'B' were changed keeping the
concentrations of one of the reactants constant and rates
were measured as a function of initial concentration.
Following results were obtained. Choose the correct option
for the rate equations for this reaction.
Experiment Initial Initial Initial
concentration concentration concentration of
of [A]/mol L⁻¹ of [B]/mol L⁻¹ [C]/mol L⁻¹s⁻¹
1. 0.30 0.30 0.10
2. 0.30 0.60 0.40
3. 0.60 0.30 0.20
(a) Rate = k [A]²[B] (b) Rate = k [A] [B]²
(c) Rate = k [A] [B] (d) Rate = k [A]²[B]⁰

Answer 1

The rate equation for this reaction is Rate = k[A]  1  [B]  2

Option (B) is correct.

Explanation:

Let order with respect to AA and BB are x and y respectively.

Rate = k(A)  x  (B)  y

• 0.1 = k(0.3)   x  (0.3)  y  ....(1)
• 0.4 = k(0.3)  x  (0.6) y  ....(2)
• 0.2 = k(0.6)  x  (0.3)  y  ....(3)

Dividing (2) by (1):

0.4 / 0.1   =   (0.6)  y  / (0.3)  y

y = 2

Dividing (3) by (1):

0.2  / 0.1  = (0.6)  x  /  (0.3)  x

x = 1

Rate law will be:

Rate = k[A]  1  [B]  2

Thus the rate equation for this reaction is Rate = k[A]  1  [B]  2

Also learn more

In the following reaction :

A → B + C, rate constant = 0.001 Ms-1. If we  start with 1 M of A then conc. of A and B after 10  minutes respectively are

(1) 0.5 M, 0.5 M (2) 0.6 M, 0.4 M.

(3) 0.4 M, 0.6 M (4) 0.1 M, 0.9 M​

https://brainly.in/question/13814038

 

​