For the zero order reaction 2A rightarrow B + | vedclass

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

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$10.5 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$

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(B) For a reaction $aA ightarrow bB + cC$,the rate of reaction is given by: $Rate = -\frac{1}{a} \frac{d[A]}{dt} = \frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = K$ Given the reaction $2A ightarrow B + 3C$,the rate expression is: $Rate = \frac{1}{3} \frac{d[C]}{dt} = K$ Therefore,the rate of production of $C$ is: $\frac{d[C]}{dt} = 3 	imes K$ $\frac{d[C]}{dt} = 3 	imes (3.5 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}) = 10.5 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$ Thus,the correct option is $B$.

For the zero order reaction $2A \rightarrow B + 3C$,if the rate constant $K = 3.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,what will be the rate of production of $C$?

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