For the reaction: A + 2 B rightarrow C + D,th | vedclass

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Question

(A) 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

Vedclass · Accepted Answer

$\frac{-d[A]}{dt} = \frac{-1}{2} \frac{d[B]}{dt}$

Vedclass · Answer

(A) 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 $A + 2 B \rightarrow C + D$,the stoichiometric coefficients are $a=1$ and $b=2$. Substituting these values,the rate of reaction is: Rate $= -\frac{1}{1} \frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt}$. Thus,the correct expression is $\frac{-d[A]}{dt} = \frac{-1}{2} \frac{d[B]}{dt}$.

For the reaction: $A + 2 B \rightarrow C + D$,the expression for the rate of reaction is:

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