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(B) The given rate law is $	ext{Rate} = K[A]^1[B]^2$. $1$. If $[B]$ is constant and $[A]$ is doubled,$	ext{Rate}' = K[2A]^1[B]^2 = 2 	imes 	ext{Ra

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If $[A]$ is kept constant and $[B]$ is reduced to one-fourth,the rate becomes one-fourth of the original rate.

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(B) The given rate law is $	ext{Rate} = K[A]^1[B]^2$. $1$. If $[B]$ is constant and $[A]$ is doubled,$	ext{Rate}' = K[2A]^1[B]^2 = 2 	imes 	ext{Rate}$. This is correct. $2$. If $[A]$ is constant and $[B]$ is reduced to $1/4$,$	ext{Rate}' = K[A]^1[B/4]^2 = K[A]^1[B]^2 / 16 = 	ext{Rate} / 16$. The statement says the rate becomes half,which is incorrect. $3$. If both $[A]$ and $[B]$ are doubled,$	ext{Rate}' = K[2A]^1[2B]^2 = K 	imes 2 	imes 4 	imes [A]^1[B]^2 = 8 	imes 	ext{Rate}$. This is correct. $4$. The overall order of the reaction is $1 + 2 = 3$. This is correct. Thus,the incorrect statement is option $B$.

For the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?

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