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For the reaction PCl(5)(g)hArrPCl(3)(g)+...

For the reaction `PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g),` the forward reaction at constant temperature favorrd by :

A

introducing an inert gas at constant volume

B

introducing chlorine gas at constant volume

C

introducing an inert gas at constant pressure

D

increasing the volume of the container

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The correct Answer is:
To solve the question regarding the reaction \( \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \) and the conditions that favor the forward reaction at constant temperature, we will analyze each option provided. ### Step-by-Step Solution: 1. **Understanding the Reaction**: The reaction involves the dissociation of phosphorus pentachloride (\( \text{PCl}_5 \)) into phosphorus trichloride (\( \text{PCl}_3 \)) and chlorine gas (\( \text{Cl}_2 \)). The forward reaction produces two moles of gas from one mole of gas. 2. **Applying Le Chatelier's Principle**: According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will adjust to counteract that change and restore a new equilibrium. 3. **Analyzing Each Option**: - **Option A: Introducing an inert gas at constant volume**: - Adding an inert gas at constant volume does not change the partial pressures of the reactants or products. Therefore, it has no effect on the equilibrium position. **This option does not favor the forward reaction.** - **Option B: Introducing chlorine gas at constant volume**: - Increasing the concentration of \( \text{Cl}_2 \) will shift the equilibrium to the left (backward reaction) to reduce the concentration of \( \text{Cl}_2 \). **This option does not favor the forward reaction.** - **Option C: Introducing an inert gas at constant pressure**: - When an inert gas is added at constant pressure, the volume of the system increases. This increase in volume shifts the equilibrium towards the side with more moles of gas. In this case, the products side has 2 moles (1 mole of \( \text{PCl}_3 \) and 1 mole of \( \text{Cl}_2 \)), while the reactants side has only 1 mole (\( \text{PCl}_5 \)). Therefore, the forward reaction is favored. **This option favors the forward reaction.** - **Option D: Increasing the volume of the container**: - Similar to option C, increasing the volume of the container will shift the equilibrium towards the side with more moles of gas. Again, the products side has 2 moles, which favors the forward reaction. **This option also favors the forward reaction.** 4. **Conclusion**: The forward reaction is favored by options C (introducing an inert gas at constant pressure) and D (increasing the volume of the container). ### Final Answer: The forward reaction at constant temperature is favored by: - **C: Introducing an inert gas at constant pressure** - **D: Increasing the volume of the container**
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