Consider the following system at equilibrium at $25^{\circ} \mathrm{C}$ : $$\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g) \quad \Delta G^{\circ}=-92.50 \mathrm{~kJ}$$ What will happen to the ratio of partial pressure of $\mathrm{PCl}_{5}$ to partial pressure of $\mathrm{PCl}_{3}$ if the temperature is raised? Explain completely.

          Consider the following system at equilibrium at $25^{\circ} \mathrm{C}$ :
$$\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g) \quad \Delta G^{\circ}=-92.50 \mathrm{~kJ}$$
What will happen to the ratio of partial pressure of $\mathrm{PCl}_{5}$ to partial pressure of $\mathrm{PCl}_{3}$ if the temperature is raised? Explain completely.

Added by Ashley J.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

11/21/2023

Step 1

According to Le Chatelier's principle, a system at equilibrium will shift in a direction that opposes any change in conditions. In this case, raising the temperature is a change in conditions, so the system will shift in a direction that absorbs heat, which is the Show more…

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Consider the following system at equilibrium at $25^{\circ} \mathrm{C}$ : $$\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g) \quad \Delta G^{\circ}=-92.50 \mathrm{~kJ}$$ What will happen to the ratio of partial pressure of $\mathrm{PCl}_{5}$ to partial pressure of $\mathrm{PCl}_{3}$ if the temperature is raised? Explain completely.