For the reaction 2A + B rightarrow 3C + D,whi | vedclass

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(B) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d

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$\frac{1}{3} \frac{d[C]}{dt}$

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(B) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$. For the given reaction $2A + B \rightarrow 3C + D$,the rate is: Rate $= -\frac{1}{2} \frac{d[A]}{dt} = -\frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} = \frac{d[D]}{dt}$. Comparing this with the options,option $B$ is incorrect because it includes a negative sign for a product $(C)$,which is physically incorrect as the concentration of products increases over time.

For the reaction $2A + B \rightarrow 3C + D$,which of the following options does not represent the correct rate of the reaction?

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