CO2(g) + H2(g) « H2O(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.                                      [H2]  = 0.20 mol/L                                   [CO2]  = 0.30 mol/L                      [H2O] = [CO]  = 0.55 mol/L (a)   What is the mole fraction of CO(g) in the equilibrium mixture? (b)   Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction. (c)   Determine Kp in terms of Kc for this system.

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CO2(g) + H2(g) « H2O(g) + CO(g)

When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.

                                     [H2]  = 0.20 mol/L

                                  [CO2]  = 0.30 mol/L

                     [H2O] = [CO]  = 0.55 mol/L

(a)   What is the mole fraction of CO(g) in the equilibrium mixture?

(b)   Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction.

(c)   Determine Kp in terms of Kc for this system.

 

Note: Please answer A, B, and C. Thank you

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