Chemical EquilibriumHard

Question

Starting with 2 moles of SO2 and 1 mol of O2 in 1 L flask, the equilibrium mixture required 0.4 moles of MnO4– for complete reaction in acidic medium. The value of KC for the reaction: 2SO2(g) + O2(g) $\rightleftharpoons$2SO3(g) is

Options

A.2
B.0.5
C.0.25
D.4

Solution

2SO2(g) + O2(g) $\rightleftharpoons$ 2SO3(g)

Initial moles 2 1 0

Moles at equilibrium 2 – 2x 1–x 2x

From question neq SO2 = neq MnO4−

Or, (2 – 2x) × 2 = 0.4 × 5 ⇒ x = 0.5

$\therefore K_{C} = \frac{(2x)^{2}}{(2 - 2x)^{2} \times (1 - x)} = 2\text{ }\text{M}^{- 1}$

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