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

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.