Consider the following system at equilibrium at 25°C:PCl₃(g) + Cl₂(g) PCl₅(g)
for which ΔH° = -92.5 kJ at 25°C.
-When the temperature of the system is raised, the ratio of the partial pressure of PCl₅ to the partial pressure of PCl₃ will

Question

Consider the following system at equilibrium at 25°C:PCl₃(g) + Cl₂(g)

Consider the following system at equilibrium at 25°C:PCl<sub>3</sub>(g) + Cl<sub>2</sub>(g) PCl<sub>5</sub>(g) for which ΔH° = -92.5 kJ at 25°C. -When the temperature of the system is raised, the ratio of the partial pressure of PCl<sub>5</sub> to the partial pressure of PCl<sub>3</sub> will A) increase. B) stay the same. C) It is impossible to tell without more information. D) decrease.

PCl₅(g)
for which ΔH° = -92.5 kJ at 25°C.
-When the temperature of the system is raised, the ratio of the partial pressure of PCl₅ to the partial pressure of PCl₃ will

Quizplus · Accepted Answer

Raising the temperature of the system will favor the endothermic direction of the reaction. If the decomposition of PCl5 into PCl3 and Cl2 is endothermic, the equilibrium will shift to produce more PCl3, thus decreasing the ratio of PCl5 to PCl3.

Consider the Following System at Equilibrium at 25°C:PCl3(g) + Cl2(g)

Consider the Following System at Equilibrium at 25°C:PCl₃(g) + Cl₂(g)