Asample of o2(g) is placed in an otherwise empty, rigid container at 4224 k at an initial pressure of 4.97 atm, where it decomposes to o(g) by the reaction below.

o2(g) ⇄ 2 o(g)

at equilibrium, the partial pressure of o2 is 0.28 atm. calculate kp for this reaction at 4224 k.

The value of at 4224 K is 314.23.

Explanation:

Initially

4.97 atm            0

At equilibrium

4.97 - p               2p

At initial stage, the partial pressure of oxygen gas = =4.97 atm

At equilibrium, the partial pressure of oxygen gas =

So, 4.97 - p = 0.28 atm

p = 4.69 atm

At equilibrium, the partial pressure of O gas =

The expression of is given as :

The value of at 4224 K is 314.23.

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