Carbon monoxide and chlorine gas react to produce phosgene (COCl2) gas according to the following reaction at 100.0C CO(g) + Cl2 (g) <-> COCl2 (g) Kp = 1.49x10^8 In an equilibrium mixture of the three gases, PCO = PCl2 = 2.55 x 10^-4 what is the equilibrium partial pressure (in atm) of Phosgene?
Express your answer below in decimal form (you will not be able to use scientific notation) to THREE significant figures. If your answer is negative include the sign.

0.000000000000000969 atm

Explanation:

Based on the reaction:

CO(g) + Cl2(g) ⇄ COCl2(g)

Where equilibrium constant, Kp, is defined as:

Kp = 1.49x10⁻⁸ = PCOCl2 / PCO * PCl2

As PCO = PCl2 = 2.55x10⁻⁴atm:

1.49x10⁻⁸ = PCOCl2 / PCO * PCl2

1.49x10⁻⁸ = PCOCl2 / 2.55x10⁻⁴atm * 2.55x10⁻⁴atm

9,69x10⁻¹⁶atm = PCOCl2

In decimal form:

I'll explain.

Explanation:

The molecules of two different elements, nitrogen and oxygen, make up about 99 percent of the air. The rest includes small amounts of argon and carbon dioxide. Oxygen is the life-giving element in the air. You can tell because they're on the periodic table which is a table for elements.