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Standard XII

Chemistry

Effective Equilibrium Constant

The equilibri...

Question

The equilibrium mixture for $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ present in 1L vessel at $600^{o} C$ contains 0.50, 0.12, and 5.0 mole of $S O_{2}, O_{2} and S O_{3}$ respectively.
Calculate $K_{C}$ for the given change at $600^{o} C .$

675.23 m o l^{- 1} L

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765.32 m o l^{- 1} L

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833.33 m o l^{- 1} L

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801.23 m o l^{- 1} L

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Solution

The correct option is C $833.33 m o l^{- 1} L$
The equilibrium reaction is $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g) .$
The expression for the equilibrium constant, $K_{c} = \frac{[S O_{3}]^{2}}{[S O_{2}]^{2} [O_{2}]}$
Substituting given values in the above expression, we get,
$K_{c} = \frac{(5)^{2}}{(0.5)^{2} \times 0.12} = 833.33 m o l^{- 1} L$

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Similar questions

Q. The equilibrium mixture for

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

present in 1L vessel at

600^{o} C

contains 0.50, 0.12, and 5.0 mole of

S O_{2}, O_{2} and S O_{3}

respectively.
Calculate

K_{C}

for the given change at

600^{o} C .

Q. The equilibrium mixture for

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

present in 1L vessel at

600^{p} C

contains 0.50, 0.12, and 5.0 mole of

S O_{2}, O_{2} a n d S O_{3}

respectively.
Also calculate

K_{p}

Q. The equilibrium mixture for

{2 S O}_{2} + O_{2} ⇌ {2 S O}_{3}

present in I L vessel at 600C contains 0.50, 0.12, and 5.0 moles of

S O_{2}, O_{2}

and

S O_{3}

respectively.
A) Calculate

K_{C}

for the given change at

600^{0} C

.
B) Also calculate

K_{P}

Q. The equilibrium mixture for formation of sulphur trioxide from sulphur dioxide present in 1 litre vessel at

600^{\circ} C

contains 0.5, 0.12 and 5 mole of

S O_{2}

O_{2}

and

S O_{3}

A) Calculate

K_{c}

600^{\circ} C

B) Calculate

K_{p}

C) How many moles of

O_{2}

must be forced into reaction vessel at

600^{\circ} C

in order increase the concentration of

S O_{3}

to 5.2 moles?

Q. A mixture of

S O_{3}, S O_{2}

and

O_{2}

gases is maintained at equilibrium in 10 litre. flask at a temperature at which Kc for the reaction,

2 S O_{2} (g) + O_{2} (g) ⇀ ↽ 2 S O_{3} (g)

100 m o l^{- 1}

litre. At equilibrium.

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Effective Equilibrium Constant

Standard XII Chemistry

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The equilibrium mixture for 2SO2(g)+O2(g)⇌2SO3(g) present in 1L vessel at 600oC contains 0.50, 0.12, and 5.0 mole of SO2,O2 and SO3 respectively. Calculate KC for the given change at 600oC.

The correct option is C 833.33 mol−1L The equilibrium reaction is 2SO2(g)+O2(g)⇌2SO3(g). The expression for the equilibrium constant, Kc=[SO3]2[SO2]2[O2] Substituting given values in the above expression, we get, Kc=(5)2(0.5)2×0.12=833.33 mol−1L

The equilibrium mixture for $2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ present in 1L vessel at $600^{o} C$ contains 0.50, 0.12, and 5.0 mole of $S O_{2}, O_{2} and S O_{3}$ respectively.
Calculate $K_{C}$ for the given change at $600^{o} C .$