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 volume is decreased at constant temperature, 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 volume is decreased at constant temperature, the ratio of the partial pressure of PCl<sub>5</sub> to the partial pressure of PCl<sub>3</sub> will A) It is impossible to tell without more information. B) decrease. C) stay the same. D) increase.

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

Quizplus · Accepted Answer

According to Le Chatelier's principle, when the volume of a system in equilibrium is decreased, the equilibrium will shift towards the side with fewer moles of gas to relieve the pressure. In this case, PCl5 has one mole of gas while PCl3 has two moles of gas. Therefore, the equilibrium will shift towards the side with PCl5, causing an increase in its partial pressure and a decrease in the partial pressure of PCl3. Thus, the ratio of the partial pressure of PCl5 to the partial pressure of PCl3 will increase.

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)