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(A) The rate of the reaction is determined by the slowest step,which is step $(ii)$.Rate $r = k[A][B_2]$.Since $A$ is an intermediate,we use the equil

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$1.5$

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(A) The rate of the reaction is determined by the slowest step,which is step $(ii)$.Rate $r = k[A][B_2]$.Since $A$ is an intermediate,we use the equilibrium from the fast step $(i)$:$K_{eq} = \frac{[A]^2}{[A_2]} \implies [A] = K_{eq}^{1/2} [A_2]^{1/2}$.Substituting this into the rate expression:$r = k 	imes K_{eq}^{1/2} [A_2]^{1/2} [B_2] = k'[A_2]^{1/2} [B_2]^1$.The overall order of the reaction is the sum of the exponents of the concentration terms:Order $= 0.5 + 1 = 1.5$.

The order of the reaction occurring by the following mechanism should be:
$(i)$ $A_2 \to A + A$ (fast)
$(ii)$ $A + B_2 \to AB + B$ (slow)
$(iii)$ $A + B \to AB$ (fast)

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The order of the reaction occurring by the following mechanism should be:$(i)$ $A_2 \to A + A$ (fast)$(ii)$ $A + B_2 \to AB + B$ (slow)$(iii)$ $A + B \to AB$ (fast)