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A mixture of 6.92e-02 mol of Cl2, 2.15e-02 mol of H2O, 6.78e-02 mol of HCl, and...

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Chemistry

A mixture of 6.92e-02 mol of Cl2, 2.15e-02 mol of H2O, 6.78e-02mol of HCl, and 5.04e-02 mol of O2 is placed in a 1.0-L steelpressure vessel at 1447 K.

The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4HCl(g) + O2(g)

At equilibrium 1.43e-02 mol of H2O is found in the reactionmixture.

Calculate the equilibrium pressures of all gases in the reactionvessel and the value of KP for the reaction.

Pick the correct statement from the multiple choices.

Use the value R = 0.0821 L-atm/mol-K for the gas constant.

a) The equilibrium constant is KP = 2.7e-03 .

b) The equilibrium pressure of O2 is PO2 = 6.42 atm.

c) The equilibrium pressure of HCl is PHCl = 6.34 atm.

d) The equilibrium pressure of Cl2 is PCl2 = 9.07 atm.

e) The equilibrium constant is KP = 7.4e+01 .

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