The equilibrium constant for the reaction- SO3 g - SO2 g -1-2O2 g is Kc- 4-9-10-2- The value of Kc for the reaction 2SO2 g - O2 g - 2SO3 g will be -

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Law of Mass Action

The equilibri...

Question

The equilibrium constant for the reaction, $S O_{3} (g) ⇌ S O_{2} (g) + \frac{1}{2} O_{2} (g)$ is $K_{c} = 4.9 \times 10^{- 2}$ . The value of $K_{c}$ for the reaction $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$
will be :

9.8 \times 10^{- 2}

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4.9 \times 10^{- 2}

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416

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2.40 \times 10^{- 3}

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Solution

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Similar questions

K_{c} = 4.9 \times 10^{- 2}

{S O}_{3} (g) ⇌ {S O}_{2} (g) + \frac{1}{2} O_{2} (g)

K_{c}

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

S O_{3} (g) ⇌ S O_{2} (g) + \frac{1}{2} O_{2} (g)

K_{c} = 4.9 \times 10^{- 2}

K_{c}

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

K_{c}

S O_{3 (g)} ⇌

+ \frac{1}{2} O_{2} (g)

4.9 \times 10^{- 2}

K_{c}

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

S O_{3} (g) ⇌ S O_{2} (g) + \frac{1}{2} O_{2} (g); K_{c} = 4.9 \times 10^{- 2} m o l^{1 / 2} l i t r e^{- 1 / 2}

K_{c}

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

S O_{3} (g) ⇌ S O_{2} (g) + \frac{1}{2} O_{2} (g); K_{c} = 5 \times 10^{- 2}

K_{c}

2 {S O}_{2} (g) + O_{2} (g) ⇌ 2 {S O}_{3} (g),

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