CO(g) + Cl2 (g) ⇌ COCl2 (g) Kp = 22.5 at 395 °C . A sample of COCl2 (g) is introduced into a constantvolume vessel at 395 °C and observed to exert an initial pressure of 0.351 atm. When equilibrium is established, what will be the total pressure within the vessel?

Explanation:

Hello,

In this case, it is convenient to rewrite the chemical reaction considering the COCl₂ as the reactant, so we must invert the equilibrium constant as shown below:

Thus, by introducing the change due to reaction's progress, one obtains:

Solving for via quadratic equation or solver, one obtains:

Clearly, the solution is for which the total pressure at equilibrium is:

Best regards.

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8