The equilibrium constant for the following reaction is K_p = 4.1 x 10^-3
COCl₂(g) CO(g) + Cl₂(g)
Calculate the equilibrium pressure of CO in a closed vessel that initially contained 0.30 atm of COCl₂ and no CO or Cl₂.

Question

The equilibrium constant for the following reaction is K_p = 4.1 x 10^-3
COCl₂(g)

The equilibrium constant for the following reaction is K<sub>p</sub> = 4.1 x 10<sup>-3</sup> COCl<sub>2</sub>(g) CO(g) + Cl<sub>2</sub>(g) Calculate the equilibrium pressure of CO in a closed vessel that initially contained 0.30 atm of COCl<sub>2</sub> and no CO or Cl<sub>2</sub>.

CO(g) + Cl₂(g)
Calculate the equilibrium pressure of CO in a closed vessel that initially contained 0.30 atm of COCl₂ and no CO or Cl₂.

Quizplus · Accepted Answer

The Answer of The equilibrium constant for the following reaction is K_p = 4.1 x 10^-3 COCl₂(g) CO(g) + Cl₂(g) Calculate the equilibrium pressure of CO in a closed vessel that initially contained 0.30 atm of COCl₂ and no CO or Cl₂.

The Equilibrium Constant for the Following Reaction Is Kp =

The Equilibrium Constant for the Following Reaction Is K_p =