Question

In the formation of sulfur trioxide by the contact process $2S{O}_2\left(g\right)+O_2\left(g\right)\to 2S{O}_3\left(g\right)$. The rate of reaction is expressed as $-\frac{d\left(O_2\right)}{dt}=2.5\times {10}^{-4}mol{L}^{-1}se{c}^{-1}$. The rate of disappearance of $\left(S{O}_2\right)$ will be:

• A. $5\times {10}^{-4}mol{L}^{-1}{S}^{-1}$
• B. $-2.25\times {10}^{-4}mol{L}^{-1}{S}^{-1}$
• C. $3.75\times {10}^{-4}mol{L}^{-1}{S}^{-1}$
• D. $50.0\times {10}^{-4}mol{L}^{-1}{S}^{-1}$

Answer 1

The correct option is A $5\times {10}^{-4}mol{L}^{-1}{S}^{-1}$

$\frac{-d\left[O_2\right]}{dt}=-\frac{1}{2}\frac{d\left[S{O}_2\right]}{dt}=2.5\times {10}^{-4}=-\frac{1}{2}\frac{d\left[S{O}_2\right]}{dt}\frac{d\left[S{O}_2\right]}{dt}=5\times {10}^{-4}mol{L}^{-1}se{c}^{-1}$

So answer is A.