For the reaction 2SO_2 + O_2 to 2SO_3,the rat | vedclass

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Question

(B) The given reaction is $2SO_2 + O_2 	o 2SO_3$. The rate expression for this reaction is given by: $-\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_2]

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$4.0 	imes 10^{-4} \ mol \ L^{-1}s^{-1}$

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(B) The given reaction is $2SO_2 + O_2 	o 2SO_3$. The rate expression for this reaction is given by: $-\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_2]}{dt} = \frac{1}{2} \frac{d[SO_3]}{dt}$. We are given the rate of disappearance of $O_2$,which is $-\frac{d[O_2]}{dt} = 2.0 	imes 10^{-4} \ mol \ L^{-1}s^{-1}$. From the rate expression,we have: $-\frac{d[O_2]}{dt} = \frac{1}{2} \frac{d[SO_3]}{dt}$. Therefore,the rate of appearance of $SO_3$ is: $\frac{d[SO_3]}{dt} = 2 	imes (-\frac{d[O_2]}{dt}) = 2 	imes (2.0 	imes 10^{-4} \ mol \ L^{-1}s^{-1}) = 4.0 	imes 10^{-4} \ mol \ L^{-1}s^{-1}$.

Time $t$ $(s)$	$0$	$5$	$10$	$20$	$30$
Concentration $(mol \ L^{-1})$	$160 \times 10^{-3}$	$80 \times 10^{-3}$	$40 \times 10^{-3}$	$10 \times 10^{-3}$	$3.5 \times 10^{-3}$

For the reaction $2SO_2 + O_2 \to 2SO_3$,the rate of disappearance of $O_2$ is $2.0 \times 10^{-4} \ mol \ L^{-1}s^{-1}$. The rate of appearance of $SO_3$ is:

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