Question

The reaction: A2+ B2 → 2AB, is bound to obey
the following mechanism
A2——> A+A (fast)
A+B2——->AB + B (slow)
A+
B —->AB (fast)
The order of overall reaction is
(1) 3
(2) 2
(3) 2.5
(4) 1.5

Answer 1

1.5 is the order of the overall reaction.

Explanation:

Given reaction,

$A_{2} + B_{2}$ → 2AB

As we observe the given mechanism, we see that 'A' is the intervening reactive strain whose congregation will be determined using the equilibrium step.

A.T.Q.

A+ $B_{2}$ → AB + B (slow)

so,

r = k[A] $B_{2}$

by using the equilibrium step,

$A_{2}$ ⇌ A + A(fast)

Since, $K_{eq}$ = $[A]^2$/[$A_{2}$]

∵ [A] = ($K_{eq}$ [$A_{2}$]^1/2)

by putting the value of A in the above equation,

r = k.$K_{eq.}$^1/2 [$A_{2}$]^1/2[$B_{2}$]

Thus,

The reaction's order = 1/2 + 1

= 1.5

Learn more: Chemical reaction

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