The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.65 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 7.10 atm of HBr is introduced into a sealed container at this temperature.

6.97 atm was the equilibrium pressure of HBr .

Explanation:

The value of the equilibrium constant =

Initially:

0             0                 7.10 atm

At equilibrium

x              x                 (7.10-2x)

The expression of equilibrium constant can be written as:

Solving for x:

x = 0.065

Partial pressure of HBr at equilibrium :(7.10 - 2 × 0.065) atm = 6.97 atm

6.97 atm was the equilibrium pressure of HBr .

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