Consider the reaction given below:A + 2 B lon | vedclass

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(A) For the reaction $A + 2 B \longrightarrow 3 C + 2 D$,the rate of reaction $(r)$ is given by:$r = -\frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt} =

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$1:3$

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(A) For the reaction $A + 2 B \longrightarrow 3 C + 2 D$,the rate of reaction $(r)$ is given by:$r = -\frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} = \frac{1}{2} \frac{d[D]}{dt}$Given that the rate of disappearance of $B$ is $-\frac{d[B]}{dt} = x 	imes 10^{-2} \ mol \ L^{-1} \ s^{-1}$.Substituting this into the rate expression:$r = -\frac{1}{2} \frac{d[B]}{dt} = \frac{1}{2} (x 	imes 10^{-2}) = 0.5x 	imes 10^{-2} \ mol \ L^{-1} \ s^{-1}$.The rate of appearance of $C$ is $\frac{d[C]}{dt}$.From the rate expression,$r = \frac{1}{3} \frac{d[C]}{dt}$,so $\frac{d[C]}{dt} = 3r$.The ratio of the rate of reaction $(r)$ to the rate of appearance of $C$ $(\frac{d[C]}{dt})$ is:$\frac{r}{\frac{d[C]}{dt}} = \frac{r}{3r} = \frac{1}{3}$.

$t/s$	$0$	$50$	$100$	$150$	$200$	$300$	$400$	$700$	$800$
$[C_{4}H_{9}Cl]/mol\ L^{-1}$	$0.100$	$0.0905$	$0.0820$	$0.0741$	$0.0671$	$0.0549$	$0.0439$	$0.0210$	$0.017$

Consider the reaction given below:
$A + 2 B \longrightarrow 3 C + 2 D$.
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:

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Consider the reaction given below:$A + 2 B \longrightarrow 3 C + 2 D$.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: