NCERT Class XI Chemistry Equilibrium Solutions

Question : 15

Total: 73

At 700 K, equilibrium constant for the reaction : H2(g)+I2(g) ⇌ 2Hl(g) is 54.8. If 0.5 mol‌L–1 of HI(g) is present at equilibrium at 700 K, what are theconcentration of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K?

Solution:

2Hl(g) ⇌ H2(g)+I2(g)

Initial‌concentration	a	0	0
At‌equilibrium	0.5	x	x

Kc =

[H2][I2]

[HI]2

or ,

54.8

x×x

(0.5)2

or x2 =

0.25

54.8

⇒ x = 0.068
∴ [H2] = [I2] = 0.068 mol‌litre−1

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