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 SO_2(g), O_2(g) and SO_3(g) are mixed in a 1.0L, flask. Determine the reaction quotient of the system and the spontaneous direction of the system:

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Q_c = 1000; the equilibrium shifts to the left

Q_c = 0.001; the equilibrium shifts to the right

Q_c = 0.001; the equilibrium shifts to the left

Q_c = 1000; the equilibrium shifts to the right

answer is B.

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Detailed Solution

$\begin{array}{l} Q_{c} = \frac{{[{SO}_{3}]}^{2}}{{[{SO}_{2}]}^{2} [O_{2}]} = \frac{(0 .001)^{2}}{(0 .001)^{2} \times 0 .001} \\ Q_{c} = 1000 \end{array}$

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