$Δ G^{o}$ for the reaction $x + y ⇌ z$ is $- 4.606 k c a l$ . The value of equilibrium constant of the reaction at $227^{o} C$ is:
( $R = 2.0 c a l . {m o l}^{- 1} K^{- 1}$ )

100

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10

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2

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1

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Solution

The correct option is D $100$
$Δ G^{o} = - R T \times 2.303 \times log K$

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10

Δ G^{o}

R = 8.314 {J K}^{- 1} {mol}^{- 1}; T = 300 K

$Δ G^{\circ}$ for the reaction $x + y ⇌ z$ is $- 4.606 k c a l$ . The value of equilibrium constant of the reaction at $227^{\circ} C$ is

Δ G

X + Y ⇌ Z

- 4.606 k c a l

227

{Δ G}^{o}

(R = 8.314 J K^{- 1} m o l^{- 1}

T = 300 K)

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

300 K

Δ G^{o}

- 690.9 R .

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