75.0 g of PCl₅(g) is introduced into a 3.00 L vessel containing 10.0 g of Cl₂(g) , and the system is allowed to reach equilibrium at 250ºC.PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)
If K_p = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium

Question

Quizplus · Accepted Answer

To find the total pressure at equilibrium, first calculate the initial moles of PCl5 and Cl2. Then, use the equilibrium constant Kp to find the change in moles and calculate the equilibrium moles of each gas. Finally, use the ideal gas law to find the total pressure. The correct answer is 8.85 atm.

750 G of PCl5(g) Is Introduced into a 3

750 G of PCl₅(g) Is Introduced into a 3