A following mechanism has been proposed for a reaction:2A+B⟶D+EA+B⟶C+D (slow)A+C⟶E (fast)The rate law expression for the reaction is

Slow step isA + B → C + D (slow)Hence, r = k[A][B]

Slow step isA + B → C + D (slow)Hence, r = k[A][B]

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A following mechanism has been proposed for a reaction:
$\begin{array}{l} 2 A + B ⟶ D + E \\ A + B ⟶ C + D (slow) \\ A + C ⟶ E (fast) \end{array}$
The rate law expression for the reaction is

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$r = k [A]^{2} [B]$

r = k[A][B]

r = k[A][C]

r = k[A]²

answer is B.

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Slow step is

A + B $\to$ C + D (slow)

Hence, r = k[A][B]

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