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Consider the reaction
$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g) for which$ $K_{c} = 278 M^{- 1}$ 0.001 mole of each of the reagents SO₂(g), $O_{2} (g) and {SO}_{3} (g)$ are mixed in a 1.0 L flask. Determine the
reaction quotient of the system and the spontaneous direction of the system :

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Q_c = 0.001; the equilibrium shifts to the right

Q_c.= 1000; the equilibrium shifts to the right

Q_c.= 1000; the equilibrium shifts to the left

Q_c = 0.001; the equilibrium shifts to the left

answer is B.

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Detailed Solution

$Q_{C} = \frac{{[{SO}_{3} (g)]}^{2}}{{[{SO}_{2} (g)]}^{2} {[O_{2} (g)]}^{1}} = 1000 > K_{c}$
i.e., reaction moves backward also if volume increases pressure decreases
$\Rightarrow Q_{c} ↑$

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