Iron(III) oxide and hydrogen react to form iron and water, like this: Fe_2O_3(s) + 3H_2(g) rightarrow 2Fe(s) + 3H_2O(g) At a certain temperature, a chemist finds that a 5.4 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: Calculate the value of the equilibrium constant K_c for this reaction. Round your answer to 2 significant digits.

Complete Question

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The equilibrium constant is  

Explanation:

      From  the question we are told that

              The chemical reaction equation is

The voume of the misture is    

  The molar mass of   is a constant with value of  

    The molar mass of      is a constant with value of  

    The molar mass of      is a constant with value of  

Generally the number of moles  is mathematically given as

    For  

     For  

       For  

Generally the concentration of a compound  is mathematicallyrepresented  as

      For  

       For  

      For  

  The equilibrium constant  is mathematically represented as

  Considering

            And      

At  equilibrium the

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.