A_{(g)} + 2B_{(g)} to product is an elementar | vedclass

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(D) For an elementary reaction $A_{(g)} + 2B_{(g)} 	o 	ext{product}$,the rate law is given by $Rate = K[A][B]^2$.Since the order with respect to $A$

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If $[A]$ is in excess,it is a Pseudo second-order reaction.

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(D) For an elementary reaction $A_{(g)} + 2B_{(g)} 	o 	ext{product}$,the rate law is given by $Rate = K[A][B]^2$.Since the order with respect to $A$ is $1$ and with respect to $B$ is $2$,the overall order is $3$.If $[B]$ is in excess,$[B]$ remains approximately constant,so the rate becomes $Rate = K'[A]$,where $K' = K[B]^2$. This is a Pseudo first-order reaction.For a first-order reaction,$t_{1/2} = \frac{0.693}{K'}$,which is independent of the initial concentration of $A$.If $[A]$ is in excess,the rate becomes $Rate = K''[B]^2$,where $K'' = K[A]$. This is a Pseudo second-order reaction.Therefore,all statements $A, B, C,$ and $D$ are technically correct descriptions of the kinetics under the given conditions. However,in the context of standard multiple-choice questions,if one must be chosen as 'incorrect' due to a potential typo in the question's premise,option $B$ is often cited in textbooks regarding the dependence of $t_{1/2}$ on the rate constant $K'$,but strictly speaking,none are incorrect. Given the options,$D$ is the most standard description of a pseudo-order reaction.

$S.NO.$	$[A] \ mol \ L^{-1}$	$[B] \ mol \ L^{-1}$	$Rate \ mol \ L^{-1} \ sec^{-1}$
$I$	$1 \times 10^{-2}$	$2 \times 10^{-2}$	$2 \times 10^{-4}$
$II$	$2 \times 10^{-2}$	$2 \times 10^{-2}$	$4 \times 10^{-4}$
$III$	$2 \times 10^{-2}$	$4 \times 10^{-2}$	$8 \times 10^{-4}$

$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?

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