Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700

Question

Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700 K the equilibrium constant is 5.10. Calculate the equilibrium concentrations of all species if 1.000 mole of each component (reactants and products) is mixed in a 1.000 L flask. (Note: Be sure to check Q to determine which way the reaction will proceed to come to equilibrium). Please show step by step, I'm lost. Thank you!
CO(g) + H2O(g) -> CO2(g) + H2(g)
Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700 K the equilibrium constant is 5.10. Calculate the equilibrium concentrations of all species if 1.000 mole of each component (reactants and products) is mixed in a 1.000 L flask. (Note: Be sure to check Q to determine which way the reaction will proceed to come to equilibrium). Please show step by step, I'm lost. Thank you!
CO(g) + H2O(g) -> CO2(g) + H2(g)
Carbon monoxide reacts with steam to produce carbon dioxide and hydrogen. At 700 K the equilibrium constant is 5.10. Calculate the equilibrium concentrations of all species if 1.000 mole of each component (reactants and products) is mixed in a 1.000 L flask. (Note: Be sure to check Q to determine which way the reaction will proceed to come to equilibrium). Please show step by step, I'm lost. Thank you!
CO(g) + H2O(g) -> CO2(g) + H2(g)

Explanation / Answer

          CO(g) + H2O(g) -> CO2(g) + H2(g)

I        1             1               1               1

C      -x           -x              +x               +x

E       1-x        1-x            1+x           1+x

        Kc = [Co2][H2]/[CO][H2O]

       5.1   = (1+x)*(1+x)/(1-x)*(1-x)

       5.1    = (1+x/1-x)2

       2.25    = 1+x/1-x

      2.25*(1-x) = 1+x

   x = 0.385

[CO2] = 1+x = 1+0.385 = 1.385M

[H2]    = 1+x = 1+0.385 = 1.385M

[CO]   = 1-x    = 1-0.385   = 0.615M

[H2O] = 1-x   = 1-0.385   = 0.615M

   

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