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

$t / s$	$0$	$30$	$60$	$90$
$[A] / mol \ L^{-1}$	$0.55$	$0.31$	$0.17$	$0.085$

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

Similar Questions

In a pseudo first order reaction in water,the following results were obtained:

$t / s$ $0$ $30$ $60$ $90$

$[A] / mol \ L^{-1}$ $0.55$ $0.31$ $0.17$ $0.085$

Calculate the average rate of reaction between the time interval $30$ to $60 \ s$.

In the reaction $2 N_{2}O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$,the ratio of the rate of formation of $NO_{2(g)}$ to the rate of formation of $O_{2(g)}$ is:

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$A + 2 B \longrightarrow 3 C + 2 D$.
If the rate of disappearance of $B$ is $x \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$,the ratio of the rate of reaction and the rate of appearance of $C$ is:

What is the rate of reaction?

What is the average rate of reaction when the change in concentration of product is $0.05 \ M$ in $20 \ s$ (in $M \ s^{-1}$)?

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