Consider the reaction.
2A(g)−⇀↽−B(g) Kp=7.80×10−5
at 500 K If a sample of A(g) at 5.40 atm is heated to 500 K, what is the pressure of B(g)at equilibrium?

0.00227 atm is the pressure of B(g)at equilibrium.

Explanation:

The value of equilibrium constant =

Partial pressure of A before heating = 5.40 atm

Initially

5.40 atm         0

at equilibrium

(5.40-2p)atm       p

The expression of an equilibrium constant can be given as

Solving for p ;

p = 0.00227 atm

Partial pressure of B at 500 K = 0.00227 atm

0.00227 atm is the pressure of B(g)at equilibrium.

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