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The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).
Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:
- a)temperature is increased
- b)temperature is lowered
- c)pressure is increased
- d)pressure is lowered
Correct answer is option 'A'. Can you explain this answer?
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The variables Pressure, Volume, Concentration and Temperature may cha...
Increase in temperature will favour the forward reaction which is endothermic.
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The variables Pressure, Volume, Concentration and Temperature may cha...
The equilibrium Solid → Liquid → Gas will shift in the forward direction when the temperature is increased.
Explanation:
Le Chatelier's principle states that when a system at equilibrium is subjected to a change in conditions, the equilibrium will shift in a direction that minimizes the effect of that change.
In the given equilibrium Solid → Liquid → Gas, the reaction proceeds in the forward direction from solid to liquid to gas. This means that as the temperature increases, the equilibrium will shift in the forward direction, favoring the formation of more gas.
Here's a detailed explanation of why the forward shift occurs when the temperature is increased:
1. Increase in temperature:
- When the temperature is increased, the average kinetic energy of the particles in the system also increases.
- In the solid state, the particles are closely packed and have low kinetic energy, resulting in a fixed shape and volume.
- As the temperature increases, the particles gain energy and start moving more vigorously, leading to the melting of the solid and formation of a liquid.
- Further increase in temperature leads to increased kinetic energy, causing the liquid particles to move even faster, resulting in the evaporation of the liquid and formation of a gas.
- Therefore, increasing the temperature favors the forward reaction, promoting the formation of more gas.
2. Decrease in temperature:
- On the other hand, when the temperature is lowered, the average kinetic energy of the particles decreases.
- In the gas state, the particles have high kinetic energy and are widely separated, resulting in a random arrangement and no fixed shape or volume.
- As the temperature decreases, the gas particles lose energy and slow down, leading to the condensation of the gas and formation of a liquid.
- Further decrease in temperature causes the liquid particles to lose energy and slow down even more, resulting in the solidification of the liquid.
- Therefore, decreasing the temperature favors the reverse reaction, promoting the formation of more solid.
In conclusion, the equilibrium Solid → Liquid → Gas will shift in the forward direction when the temperature is increased because it favors the formation of more gas.
Explanation:
Le Chatelier's principle states that when a system at equilibrium is subjected to a change in conditions, the equilibrium will shift in a direction that minimizes the effect of that change.
In the given equilibrium Solid → Liquid → Gas, the reaction proceeds in the forward direction from solid to liquid to gas. This means that as the temperature increases, the equilibrium will shift in the forward direction, favoring the formation of more gas.
Here's a detailed explanation of why the forward shift occurs when the temperature is increased:
1. Increase in temperature:
- When the temperature is increased, the average kinetic energy of the particles in the system also increases.
- In the solid state, the particles are closely packed and have low kinetic energy, resulting in a fixed shape and volume.
- As the temperature increases, the particles gain energy and start moving more vigorously, leading to the melting of the solid and formation of a liquid.
- Further increase in temperature leads to increased kinetic energy, causing the liquid particles to move even faster, resulting in the evaporation of the liquid and formation of a gas.
- Therefore, increasing the temperature favors the forward reaction, promoting the formation of more gas.
2. Decrease in temperature:
- On the other hand, when the temperature is lowered, the average kinetic energy of the particles decreases.
- In the gas state, the particles have high kinetic energy and are widely separated, resulting in a random arrangement and no fixed shape or volume.
- As the temperature decreases, the gas particles lose energy and slow down, leading to the condensation of the gas and formation of a liquid.
- Further decrease in temperature causes the liquid particles to lose energy and slow down even more, resulting in the solidification of the liquid.
- Therefore, decreasing the temperature favors the reverse reaction, promoting the formation of more solid.
In conclusion, the equilibrium Solid → Liquid → Gas will shift in the forward direction when the temperature is increased because it favors the formation of more gas.
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The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer?
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The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer?.
The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer?.
Solutions for The variables Pressure, Volume, Concentration and Temperature may change the State of Equilibrium. The change is governed by the Le-Chatelier’s principle. The decomposition of NH3(g) can be made spontaneous by increasing the temperature and lowering pressure. In the reaction, removal of any product from the reaction mixture makes the reversible reaction irreversible and therefore, reaction proceeds to completion. Answer the given questions (i) to (iv).Q. The equilibrium Solid → Liquid → Gas will shift in forward direction when:a)temperature is increasedb)temperature is loweredc)pressure is increasedd)pressure is loweredCorrect answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11.
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