$Δ G$ for the reaction, $X + Y ⇌ Z$ is $- 4.606 k c a l$ . The equilibrium constant for the reaction at $227$ is :

100

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0.01

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Solution

The correct option is A 100
As we know,
$Δ G = - 2.303 R T log K$
$- 4.606 \times 10^{3} = - 2.303 \times 2 \times 500 log K$
$K = 100$

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Similar questions

$Δ G^{\circ}$ 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^{o}

x + y ⇌ z

- 4.606 k c a l

227^{o} C

R = 2.0 c a l . {m o l}^{- 1} K^{- 1}

△ G^{0}

x + y ⇌ Z

- v e 4.606 k c a l

227^{0}

Δ G^{\circ} = + 1.7 k J .

25^{0} C

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

Δ G^{\circ}

δ G

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