When the molar concentrations of $S O_{2}, O_{2}$ and $S O_{3}$ at equilibrium at certain temperature are $0.5, 0.25, a n d 0.25 M$ respectively, $K_{c}$ for $S O_{3 (g)} ⇌ 2 S O_{2 (g)} + O_{2 (g)}$ is:

0.5 l i t . {m o l}^{- 1}

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1 {l i t}^{2} . {m o l}^{- 2}

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1 m o l {l i t}^{- 1}

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0.25 {m o l}^{2} {l i t}^{- 2}

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Solution

The correct option is B $1 m o l {l i t}^{- 1}$
$2 S O_{3} ⇌ 2 S O_{2} + O_{2}$
at $E q b^{m}$ $0.25 M$ $0.5 M$ $0.25 M$
$K_{C} = \frac{[O_{2}] [S O_{2}]^{2}}{[S O_{3}]^{2}}$
$\Rightarrow K_{C} = \frac{[0.25] [0.5]^{2}}{[0.25]^{2}} \frac{M^{3}}{M^{2}}$
$\Rightarrow K_{C} = 1 M = 1 m o l L^{- 1}$

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Similar questions

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

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What is K_c for the following equilibrium when the equilibrium concentration of each substance is: [SO₂]= 0.60 M, [O₂] = 0.82 M and [SO₃] = 1.90 M ?

2SO₂ (g) + O₂ (g) ⇌ 2SO₃ (g)

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

[S O_{2}] = 3.0 \times 10^{- 3} M, [O_{2}] = 3.5 \times 10^{- 3} M, [S O_{3}] = 5.0 \times 10^{- 2} M

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