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Question

(A) For the reaction $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$,the rate of reaction is expressed as:$Rate = -\frac{1}{2} \frac{d[SO_2]}{dt} = -\f

Vedclass · Accepted Answer

$5 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}$

Vedclass · Answer

(A) For the reaction $2SO_{2(g)} + O_{2(g)} ightarrow 2SO_{3(g)}$,the rate of reaction is expressed as:$Rate = -\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_2]}{dt} = \frac{1}{2} \frac{d[SO_3]}{dt}$Given that $-\frac{d[O_2]}{dt} = 2.5 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}$.Equating the terms for $SO_2$ and $O_2$:$-\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_2]}{dt}$$-\frac{d[SO_2]}{dt} = 2 	imes (-\frac{d[O_2]}{dt})$$-\frac{d[SO_2]}{dt} = 2 	imes (2.5 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}) = 5 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}$.

In the contact process for the manufacture of sulfur trioxide,the reaction is $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$. If the rate of reaction is given by $-\frac{d[O_2]}{dt} = 2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$,what is the rate of disappearance of $SO_2$?

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