NCERT Class XI Chemistry Equilibrium Solutions

Question : 27

Total: 73

The equilibrium constant for the following reaction is 1.6 × 105 at 1024 K.
H2(g)+Br2(g) ⇌ 2HBr(g)
Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

Solution:

H2(g)+Br2(g) ⇌ 2HBr(g) ; Kp = 1.6 × 105
For the reaction 2HBr(g) ⇌ H2(g)+Br2(g)
Kp =

1.6×105

= 6.25 × 10−6
2HBr(g) ⇌ H2(g)+Br2(g)

Initial‌presuure	10.0	0	0
At‌equilibrium	10.0−2x	x	x

∴ Kp =

pH2×pBr2

pHBr2

6.25 × 10−6 =

(10.0−2x)2

10.0−2x

= 2.5 × 10−5
and x = 2.5 × 10–2 So, pH2 = pBr2 = 2.5 × 10–2 bar
pHBr = 10.0 – 5.0 × 10–2 ≈ 10.0 bar

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