Which of the following changes alone would cause increase in the value of the equilibrium constant of the reaction?
\(PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g); \Delta H>0\)
Which of the following changes alone would cause increase in the value of the equilibrium constant of the reaction?
\(PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g); \Delta H>0\)
Show Hint
- Increasing the volume of the reaction vessel
- Decreasing the volume of the reaction vessel
- ddition of catalyst to equilibrium mixture
- Addition of \(PCl_5(g)\) to the equilibrium mixture
- Increasing the temperature
The Correct Option is
Solution and Explanation
Step 1: The reaction \(PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g)\) is endothermic (\(\Delta H>0\)).
Step 2: According to Le Chatelier’s Principle, increasing the temperature of an endothermic reaction shifts the equilibrium to the right, favoring the formation of products.
Step 3: This shift increases the equilibrium constant \(K\), as \(K\) is a measure of product favorability at equilibrium.
Step 4: Therefore, increasing the temperature is the only option listed that will increase the equilibrium constant for this reaction.
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