Problem: The elementary reaction 2 H2O(g) ↔ 2 H2(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?

FREE Expert Solution

Recall that the equilibrium constant is the ratio of the products and reactants

We use Kp when dealing with pressure and Kc when dealing with concentration:

Kp =PproductPreactant Kc =[Product][Reactant]

Note that solid and liquid compounds are ignored in the equilibrium expression.


Since we’re given the pressure of each compound, we use Kp


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Problem Details
The elementary reaction 2 H2O(g) ↔ 2 H2(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?

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