The elementary reaction 2h20(g)< > 2h2(g)+o2(g) proceeds at a certain temperature until the partial pressures of h2o, h2, and o2 reach 0.0700 atm, 0.00200 atm, and 0.00600 atm respectively. what is the value of the equilibrium constant at this temperature?

4.9 x 10⁻⁶.

Explanation:

2H₂O(g) ⇄ 2H₂(g) + O₂(g),

'

P of H₂ = 0.002 atm, P of O₂ = 0.006 atm, and P of H₂O = 0.07 atm.

∴ The equilibrium constant (Kp) = (P of H₂)²(P of O₂)/(P of H₂O)² = (0.002 atm)²(0.006 atm)/(0.07 atm)² = 4.9 x 10⁻⁶.

thats how its supposed to be