For the reaction 2 A + B longrightarrow D + E | vedclass

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(B) The overall reaction is $2 A + B \longrightarrow D + E$. The proposed mechanism is: $1. A + B \longrightarrow C + D$ (slow step) $2. A + C \longri

Vedclass · Accepted Answer

$r = K[A][B]$

Vedclass · Answer

(B) The overall reaction is $2 A + B \longrightarrow D + E$. The proposed mechanism is: $1. A + B \longrightarrow C + D$ (slow step) $2. A + C \longrightarrow E$ (fast step) The rate of a reaction is determined by the slowest step,known as the Rate Determining Step ($R$.$D$.$S$). Since the first step $(A + B \longrightarrow C + D)$ is the slow step,the rate law is derived from the reactants involved in this step. Therefore,the rate law is $r = K[A][B]$.

For the reaction $2 A + B \longrightarrow D + E$,the following mechanism has been proposed: $A + B \longrightarrow C + D$ (slow) and $A + C \longrightarrow E$ (fast). Determine the rate law.

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