Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation:

PCl5(g) ? PCl3(g) + Cl2(g)

At 250° 0.375 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?

[PCl5] = 4.61 M, [PCl3] = 4.23 M, and [Cl2] = 4.23 M

[PCl5] = 0.188 M, [PCl3] = 0.581 M, and [Cl2] = 0.581 M

[PCl5] = 0.0564 M, [PCl3] = 0.319 M, and [Cl2] = 0.319 M

[PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M

The Kp for the reaction below is 1.49 × 108 at 100.0°C:

CO(g)+Cl2(g)->COCl2(g)

In an equilibrium mixture of the three gases, Pco = Pcl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is __________ atm.

6.67 × 1011
3.02 × 1015
3.31 × 104
3.31 × 10-16
7.34