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

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a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.