Consider the following reaction: PCI5(g) – PCI3(g) + Cl2(g) K, = 23.6 at 500 K a. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PPCI, = 0.560 atm and PpCl, = 0.500 atm. b. If more chlorine is added after equilibrium is reached, how will the concentrations of PCls and PC13 change?

Consider the following reaction: PCI5(g) – PCI3(g) + Cl2(g) K, = 23.6 at 500 K a. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PPCI, = 0.560 atm and PpCl, = 0.500 atm. b. If more chlorine is added after equilibrium is reached, how will the concentrations of PCls and PC13 change?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 62QRT

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