For the reaction,2 SO_{2} + O_{2} rightlefth | vedclass

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(B) For the reaction,$2 \ SO_{2} + O_{2} ightleftharpoons 2 \ SO_{3}$.The rate of reaction is given by: $	ext{Rate} = -\frac{1}{2} \frac{d[SO_{2}]}

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

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(B) For the reaction,$2 \ SO_{2} + O_{2} ightleftharpoons 2 \ SO_{3}$.The rate of reaction is given by: $	ext{Rate} = -\frac{1}{2} \frac{d[SO_{2}]}{dt} = -\frac{d[O_{2}]}{dt} = +\frac{1}{2} \frac{d[SO_{3}]}{dt}$.Given that the rate of disappearance of $O_{2}$ is $-\frac{d[O_{2}]}{dt} = 2 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$.We need to find the rate of appearance of $SO_{3}$,which is $\frac{d[SO_{3}]}{dt}$.From the rate expression: $-\frac{d[O_{2}]}{dt} = \frac{1}{2} \frac{d[SO_{3}]}{dt}$.Therefore,$\frac{d[SO_{3}]}{dt} = 2 	imes (-\frac{d[O_{2}]}{dt}) = 2 	imes (2 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}) = 4 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

For the reaction,$2 \ SO_{2} + O_{2} \rightleftharpoons 2 \ SO_{3}$,the rate of disappearance of $O_{2}$ is $2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of appearance of $SO_{3}$ is

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