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How does the equilibrium constant (K) change with temperature for the same reversible reaction?
- a)K remains constant at all temperatures.
- b)K increases with increasing temperature.
- c)K decreases with increasing temperature.
- d)K becomes zero at high temperatures.
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
How does the equilibrium constant (K) change with temperature for the ...
The equilibrium constant (K) can have varying values at different temperatures for the same reversible reaction. It increases with increasing temperature.
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How does the equilibrium constant (K) change with temperature for the ...
Understanding Equilibrium Constant (K) and Temperature
The equilibrium constant (K) of a reversible reaction is influenced by temperature changes. This is crucial for understanding reaction dynamics in chemistry, especially for NEET preparation.
Effect of Temperature on K
- Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
- Exothermic vs. Endothermic Reactions:
- Exothermic Reactions: For reactions that release heat (e.g., A + B ⇌ C + heat), increasing temperature shifts the equilibrium to the left, decreasing K.
- Endothermic Reactions: For reactions that absorb heat (e.g., A + B + heat ⇌ C), increasing temperature shifts the equilibrium to the right, increasing K.
Conclusion: Why K Increases with Temperature
- Endothermic Nature of Reactions: Most biological and chemical processes relevant to NEET involve endothermic reactions. Thus, as temperature rises, the equilibrium favors the formation of products, leading to an increase in K.
- Overall Impact: For most reactions studied in NEET, increasing temperature typically enhances product concentration, resulting in a higher K value.
Understanding this relationship helps in predicting how reactions will behave under different thermal conditions, making it essential for mastering equilibrium concepts in chemistry.
The equilibrium constant (K) of a reversible reaction is influenced by temperature changes. This is crucial for understanding reaction dynamics in chemistry, especially for NEET preparation.
Effect of Temperature on K
- Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
- Exothermic vs. Endothermic Reactions:
- Exothermic Reactions: For reactions that release heat (e.g., A + B ⇌ C + heat), increasing temperature shifts the equilibrium to the left, decreasing K.
- Endothermic Reactions: For reactions that absorb heat (e.g., A + B + heat ⇌ C), increasing temperature shifts the equilibrium to the right, increasing K.
Conclusion: Why K Increases with Temperature
- Endothermic Nature of Reactions: Most biological and chemical processes relevant to NEET involve endothermic reactions. Thus, as temperature rises, the equilibrium favors the formation of products, leading to an increase in K.
- Overall Impact: For most reactions studied in NEET, increasing temperature typically enhances product concentration, resulting in a higher K value.
Understanding this relationship helps in predicting how reactions will behave under different thermal conditions, making it essential for mastering equilibrium concepts in chemistry.
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