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On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?
- a)K will remain same
- b)K will decrease
- c)K will increase
- d)More than one of the above
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
On increasing the pressure, in which direction will the gas phase reac...
Effect of Increasing Pressure on the Equilibrium of Gas Phase Reaction
Increasing the pressure on a system at equilibrium will cause the system to shift in a direction that reduces the total pressure. This is in accordance with Le Chatelier's principle, which states that a system at equilibrium will respond to a stress by shifting the equilibrium position to counteract the stress.
Application to the Given Reaction
In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), an increase in total pressure will cause the system to shift in a direction that reduces the total pressure. Since there are fewer moles of gas on the product side of the reaction (2 moles of NH3) compared to the reactant side (1 mole of N2 + 3 moles of H2), the equilibrium will shift towards the side with fewer moles of gas to decrease the total pressure.
Effect on Equilibrium Constant (K)
Since the equilibrium constant (K) is a ratio of the concentrations of products to reactants at equilibrium, changing the total pressure (without changing the temperature) will not alter K. The concentrations of the species at equilibrium may change to re-establish equilibrium, but the ratio of concentrations (K) will remain the same.
Therefore, in this case, the equilibrium constant (K) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) will remain the same when the total pressure is increased without changing the temperature.
Increasing the pressure on a system at equilibrium will cause the system to shift in a direction that reduces the total pressure. This is in accordance with Le Chatelier's principle, which states that a system at equilibrium will respond to a stress by shifting the equilibrium position to counteract the stress.
Application to the Given Reaction
In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), an increase in total pressure will cause the system to shift in a direction that reduces the total pressure. Since there are fewer moles of gas on the product side of the reaction (2 moles of NH3) compared to the reactant side (1 mole of N2 + 3 moles of H2), the equilibrium will shift towards the side with fewer moles of gas to decrease the total pressure.
Effect on Equilibrium Constant (K)
Since the equilibrium constant (K) is a ratio of the concentrations of products to reactants at equilibrium, changing the total pressure (without changing the temperature) will not alter K. The concentrations of the species at equilibrium may change to re-establish equilibrium, but the ratio of concentrations (K) will remain the same.
Therefore, in this case, the equilibrium constant (K) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) will remain the same when the total pressure is increased without changing the temperature.
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Community Answer
On increasing the pressure, in which direction will the gas phase reac...
Concept:
Van't Hoff equation -The Van't Hoff equation gives the relationship between the standard Gibbs free energy change and the equilibrium constant.
It is represented by the equation -
-ΔG° = RT logeKp
where, R = gas constant
T = temperature
Kp = equilibrium constant
or
Thus, the equilibrium constant K is temperature-dependent.
Explanation:
The given reaction is -
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Given condition - the total pressure at which the equilibrium is established, is increased without changing the temperature or at a constant temperature.
According to Van't Hoff equation, the equilibrium constant K is temperature-dependent.
If the temperature is constant, the reaction is neither exothermic nor endothermic.
Therefore, K will remain same as temperature is constant.
Conclusion:
Hence, if the total pressure at which the equilibrium is established, is increased without changing the temperature the equilibrium constant K for the reaction
N2 (g) + 3H2 (g) ⇌ 2NH3 (g), remains same.
Hence, the correct answer is option 1.
Van't Hoff equation -The Van't Hoff equation gives the relationship between the standard Gibbs free energy change and the equilibrium constant.
It is represented by the equation -
-ΔG° = RT logeKp
where, R = gas constant
T = temperature
Kp = equilibrium constant
or
Thus, the equilibrium constant K is temperature-dependent.
Explanation:
The given reaction is -
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Given condition - the total pressure at which the equilibrium is established, is increased without changing the temperature or at a constant temperature.
According to Van't Hoff equation, the equilibrium constant K is temperature-dependent.
If the temperature is constant, the reaction is neither exothermic nor endothermic.
Therefore, K will remain same as temperature is constant.
Conclusion:
Hence, if the total pressure at which the equilibrium is established, is increased without changing the temperature the equilibrium constant K for the reaction
N2 (g) + 3H2 (g) ⇌ 2NH3 (g), remains same.
Hence, the correct answer is option 1.
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On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.N2(g) + 3H2(g)2NH3(g)Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?a)K will remain sameb)K will decreasec)K will increased)More than one of the aboveCorrect answer is option 'A'. Can you explain this answer?
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On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.N2(g) + 3H2(g)2NH3(g)Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?a)K will remain sameb)K will decreasec)K will increased)More than one of the aboveCorrect answer is option 'A'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.N2(g) + 3H2(g)2NH3(g)Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?a)K will remain sameb)K will decreasec)K will increased)More than one of the aboveCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.N2(g) + 3H2(g)2NH3(g)Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?a)K will remain sameb)K will decreasec)K will increased)More than one of the aboveCorrect answer is option 'A'. Can you explain this answer?.
Solutions for On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le Chatelier’s principle. Consider the reaction.N2(g) + 3H2(g)2NH3(g)Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?a)K will remain sameb)K will decreasec)K will increased)More than one of the aboveCorrect answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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