The elementary reaction 2 H 2 O ( g ) − ⇀ ↽ − 2 H 2 ( g ) + O 2 ( g ) proceeds at a certain temperature until the partial pressures of H 2 O , H 2 , and O 2 reach 0.025 atm, 0.0060 atm, and 0.0090 atm, respectively at equilibrium. What is the value of the equilibrium constant at this temperature?

The value of equilibrium constant = 0.005184

Explanation:

          According to the given reaction we consider Kp equation and find the value of equilibrium constant using partial pressure of individual gases.

                2 H 2 O ( g ) ⇄ 2 H 2 ( g ) + O 2 ( g )

                         Kp =      

                    Change of gaseous moles(Δn)

                                                               = 3 - 2

                                                                = 1

                        ⇒

          ∴  The value of equilibrium constant = 0.005184

idk i’m struggling too