The equilibrium constant of the reaction SO2g - 1-2 O2g - SO3g is 4 - 10- 3 atm- 0-5- The equilibrium constant of the reaction 2SO3g - 2SO2g - O2g would be-

$S O_{2 (g)} + \frac{1}{2} O_{2} (g) ⇋$ SO_3_{(g)}~is~4 \times 10^{-3}atm .The equilibrium constant of the reaction 2SO_3_(g) $⇋$ 2SO_2_{(g)}+O_2(g)\) would be :

Q. The equilibrium constant of the reaction,

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

is 0. 15 at 900 K. Calculate the equilibrium constant for

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

Q. The equilibrium constant of the reaction;

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

; is

0.20 m o l e^{\frac{1}{2}} . l i t r e^{\frac{- 1}{2}}

1000 K

. Calculate equilibrium constant for

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

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The equilibrium constant of the reaction SO2(g)+1/2O2(g)⇌SO3(g) is 4×10−3 atm−0.5. The equilibrium constant of the reaction 2SO3(g)⇌2SO2(g)+O2(g) would be:

The correct option is C 6.25×104 atmSO2(g)+1/2O2(g)⇌SO3(g) K1=4×10−3 atm−0.5.2SO3(g)⇌2SO2(g)+O2(g) To get the equilibrium constant of the required equation:K1=[SO3][SO2][O2]1/2K2=[SO2]2[O2][SO3]K2=(1K1)2=1(4×10−3)2=6.25×104Hence, the correct answer is option D.

The equilibrium constant of the reaction $S O_{2} (g) + 1 / 2 O_{2} (g) ⇌ S O_{3} (g)$ is $4 \times 10^{- 3}$ $a t m^{- 0.5}$ . The equilibrium constant of the reaction $2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)$ would be: