Import Question JSON

$\text{Hint: Follow Le Chatelier's principle}$ $\text{Let's analyze what happens when an inert gas is added to the equilibrium at constant pressure:}$ $\text{PCl}_5\text{(g)} \rightleftharpoons \text{PCl}_3\text{(g) + Cl}_2\text{(g)}$ $\text{1. When an inert gas is added at constant pressure, the total volume of the system must increase to maintain the same pressure.}$ $\text{2. This increase in volume causes the concentration (moles per unit volume) of all reactants and products to decrease.}$ $\text{3. According to Le Chatelier's principle, the equilibrium will shift in the direction that counteracts this change.}$ $\text{4. The system will favor the side with a greater number of moles of gas to counteract the decrease in concentration.}$ $\text{In this reaction:}$ $\text{Left side: 1 mole of gas (PCl}_5\text{)}$ $\text{Right side: 2 moles of gas (PCl}_3 \text{ and Cl}_2\text{)}$ $\text{Since there are more moles of gas on the right side (products), the equilibrium will shift toward the products to counteract the decrease in concentration.}$ $\text{When the equilibrium shifts toward the products, the degree of dissociation of PCl}_5 \text{ increases.}$ $\text{Therefore, the degree of dissociation will increase when an inert gas is added at constant pressure.}$ $\text{The correct answer is option 3: Increase.}$