What is the correct form of the equilibrium constant for the reaction of hydrogen and oxygen to form water? the equation is: ?

Balanced chemical reaction: 2H₂(g) + O₂(g) ⇄ 2H₂O(g).
K = [H₂O]² / [O₂] · [H₂]².
[H₂O] is equilibrium concentration of water.
[O₂] is equilibrium concentration of molecule of oxygen.
[H₂] is equilibrium concentration of molecule of molecule of hydrogen.
The substances on the right side of the reaction are written at the top of the equilibrium constant expression and those on the left at the bottom.

Given data,temperature, t = 230°c = 503 kconsider the chemical reaction,ch₃oh(l) + 1/2 o₂(g)  → ch₂o(g) + h₂o(l)calculate the enthalpy change for the reaction: δh⁰rxn =  σnδh⁰f(products) -  σmδh⁰f(reactants)substitute the values from the table: δh⁰rxn = { -115.9 + (-285.8)} - {0+(-238.7)}              = -163.0 kjcalculate the entropy change for the reaction.δs⁰rxn = (219 + 70) - (127.2 + 1/2 x 205.2) = 59.2 j/kconsider the expression for free energy: δg⁰rxn =  δh⁰rxn - t  δs⁰rxnsubstitute the values in the above equationδg⁰rxn = -163 x 10³ - (503 x 59.2)              = -192777.6 j              = -192.777 kj

Electrons are evenly distributed in the water molecule.