A reaction $S_{8 (g)} ⇌ {4S}_{2 (g)}$ is carried out by taking 2 moles of $S_{8 (g)}$ and 0.2 moles of $S_{2 (g)}$ in a
reaction vessel of 1 litre at 627°C. If $K_{C} = 6.3 \times 10^{- 6}$ ; select the correct statements :

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Reaction proceeds in backward direction

Reaction proceeds in forward direction

Reaction quotient is 8.0 × $10^{- 4}$

$K_{P} {2.55 atm}^{3}$

answer is A, B, D.

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Detailed Solution

$Q = \frac{{[S_{2}]}^{4}}{[S_{8}]} = \frac{{(0.2)}^{4}}{(2)} {= 8.0 × 10}^{-4} {; K}_{C} {= 6.3×10}^{-6} {, K}_{p} {= K}_{c} × {(RT)}^{Δn}$

${= 6.3 × 10}^{-6} × {(0.0821 × 900)}^{3} {= 2.55 atm}^{3}$

Thus, reaction proceed in backward direction, since ${Q > K}_{C}$

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