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Characteristics of Equilibrium Constant

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Question

Starting with one mole of $O_{2}$ and two moles of $S O_{2}$ , the equilibrium for the formation of $S O_{3}$ was established at a certain temperature. If $V$ is the volume of the vessel and $2 x$ is the number of moles of $S O_{3}$ present, the equilibrium constant will be:

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Solution

$2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$
At $t = 0 : -$ $\frac{1}{V}$ $\frac{2}{V}$ $0$
At equilibrium:- $(\frac{1}{V} - 2 x)$ $(\frac{2}{V} - x)$ $2 x$
Now, $K_{C} = \frac{2 x}{(\frac{1}{V} - 2 x) (\frac{2}{V} - x)} = \frac{2 x}{(1 - 2 x V) (2 - x V)}$
Therefore, the equilibrium constant will be $\frac{2 x}{(1 - 2 x V) (2 - x V)}$ .

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Similar questions

S O_{3}

was placed in a litre reaction vessel at a certain temperature , the following equilibrium was established,

2 S O_{3} ⇌ 2 S O_{2} + O_{2}

. At equilibrium 0.6 moles of

S O_{2}

were formed. The equilibrium constant of the reaction will be:

S O_{3}

was placed in a 1 lit. reaction vessel at a constant temperature. The following equilibrium was established:

2 S O_{3} \Leftrightarrow 2 S O_{2} + O_{2}

. At equilibrium, 0.6 moles of

S O_{2}

were formed. The equilibrium constant of the reaction will be:

S O_{3}

was placed in a vessel of

1

L capacity at a certain temperature when the following equilibrium was established.

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

At equilibrium,

0.6

S O_{2}

were formed. The equilibrium constant

K_{c}

for the reaction will be:

Q. A mixture of

S O_{3}, S O_{2}

O_{2}

gases are maintained at equilibrium in 10 litre flask at a temperature at which

K_{c}

for the reaction,

2 S O_{2} (g) + O_{2} (g) \Leftrightarrow 2 S O_{3} (g)

m o l^{- 1}

litre. At equilibrium,

a) If no of mole of

S O_{3}

S O_{2}

in the flask are same, how many moles of

O_{2}

are present?
b) If no. of mole of

S O_{3}

in the flask are twice the no of mole of

S O_{2}

, how many moles of

O_{2}

Q. A mixture of

{S O}_{3}, {S O}_{2}

O_{2}

gases is maintained in a

10 L

flask at a temperature at which the equilibrium constant for the reaction is

100

and the reaction is,

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

.
(i) If the number of moles of

{S O}_{2}

{S O}_{3}

in the flask are equal, how many moles of

O_{2}

are present?
(ii) If the number of moles of

{S O}_{3}

in the flask is twice the number of moles of

{S O}_{2}

, how many moles of oxygen are present?

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