Question

In the formation of sulphur trioxide by the contact process.
$2S{O}_{2\left(g\right)}+O_{2\left(g\right)}\rightleftharpoons 2S{O}_{3\left(g\right)}$
The rate of reaction is expressed as $-\frac{d\left(O_2\right)}{dt}=2.5\times {10}^{-4}mol{e}^{-1}{L}^{-1}se{c}^{-1}$
The rate of disappearance of $(SO{)}_2$ will be:

• A. $5.0\times {10}^{-4}mol{L}^{-1}{s}^{-1}$
• 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 $5.0\times {10}^{-4}mol{L}^{-1}{s}^{-1}$

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