Question

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.

Answer 1

Answer: The equilibrium partial pressure of phosgene is 7.34 atm

Explanation:

The given chemical equation follows:

                    $CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)$

The expression of $K_p$ for above equation follows:

$K_p=\frac{p_{COCl_2}}{(p_{CO})\times (p_{Cl_2})}$

We are given:

Equilibrium partial pressure of CO = $2.22\times 10^{-4}atm$

Equilibrium partial pressure of chlorine gas = $2.22\times 10^{-4}atm$

$K_p=1.49\times 10^8$

Putting values in above equation, we get:

$1.49\times 10^8=\frac{p_{COCl_2}}{(2.22\times 10^{-4})\times (2.22\times 10^{-4})}\\\\p_{COCl_2}=7.34atm$

Hence, the equilibrium partial pressure of phosgene is 7.34 atm