A mixture of 4.10e-02 mol of O2, 3.07e-02 mol of NOCl, 4.29e-02 mol of NO2, and 1.83e-01 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 627 K. The following equilibrium is established:
O2(g) + 2 NOCl(g) --> 2 NO2(g) + Cl2(g)
At equilibrium 1.97e-02 mol of NOCl is found in the reaction mixture. Calculate the equilibrium pressures of all gases in the reaction vessel 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 pressure of NO2 is PNO2 = 2.78 atm.
b) The equilibrium pressure of Cl2 is PCl2 = 9.16 atm.
c) The equilibrium pressure of O2 is PO2 = 2.39 atm.
d) The equilibrium constant is KP = 2.5e-02 .
e) The equilibrium constant is KP = 2.0e+02 .