The rate of formation of SO3 in the reaction 2SO2+O2→2SO3 is 100g min−1 . Hence rate of disappearance of O2 in g/min is

Rate of formation of SO3=100g/min=10080mole/minRate of disappearance of O2=?2SO2(g)+O2(g)⇌2SO3(g)Rate of disappearance of O2−11ddtO2=+12ddtSO3=12×10080 mole /min∴rate of dissappearence of O2=12×10080×32g/min=20g/min

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The rate of formation of ${SO}_{3}$ in the reaction $2 {SO}_{2} + O_{2} \to 2 {SO}_{3}$ is $100 g \min^{- 1}$ . Hence rate of disappearance of $O_{2}$ in g/min is

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Detailed Solution

Rate of formation of ${SO}_{3} = 100 g / \min = \frac{100}{80} mole / \min$
Rate of disappearance of $O_{2} = ? 2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g)$
Rate of disappearance of $O_{2} - \frac{1}{1} \frac{d}{dt} [O_{2}] = + \frac{1}{2} \frac{d}{dt} [{SO}_{3}] = \frac{1}{2} \times \frac{100}{80} mole / min$
$∴$ rate of dissappearence of $O_{2} = \frac{1}{2} \times \frac{100}{80} \times 32 g / \min = 20 g / \min$