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How would a change in pressure affect a gaseous system in equilibrium, according to Le Chatelier's principle?
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The answer is "The equilibrium would shift to reduce the pressure change" on Apex
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According to le chatelier principle how would a change in pressure affect a gaseous system in equilibrium?
The answer is "The equilibrium would shift to reduce the pressure change" on Apex
How would Le Chatelier's principle a change in pressure affect a gaseous system in equilibrium?
The equalibrium would shift to reduce the pressure
What does Le Chatelier's principle state?
A reaction at equilibrium will respond to balance a change - apex (Explanation): The answer is NOT "a new equilibrium ratio will form", because although this is true, it will not necessarily always happen and is not what le chatelier's principle is about. His principle focuses on the reaction changing to cancel out or balance the change in equilibrium. Therefore, this is the correct answer.
Why is it important to use high pressure in the Haber process?
The Haber process is basically converting Nitrogen and Hydrogen into ammonia. The equation is N2 + 3H2 -------> 2NH3 but it is an equilibrium. By Le Chetalier's principle if we apply pressure the system will try to counteract that by trying to lower pressure and to do this it needs to form product because there are 4 molecules of reactants and only two of product so the pressure is lower when there are fewer molecules. High Pressure thus favors high yields and hence good productivity and profitability.
How could you increase the production of 2NH3(g) N2(g) plus 3H2(g) 2NH3(g) Increase the volume of the reaction vessel. Increase the pressure of the system. Decrease the pressure of the system. Remove?
Given N2(g) + 3H2(g) <---> 2NH3(g), increasing the pressure will cause more NH3 to form. According to LeChatelier's Principle, an increase in pressure moves the equilibrium in the direction where there are fewer moles (particles), which in this equilibrium, is to the right.
According to le chatelier principle how would a change in pressure affect a gaseous system in equilibrium?
The answer is "The equilibrium would shift to reduce the pressure change" on Apex
according to le chatelier's principle, how would a change in pressure affect a gaseous system in equilibrium?
The answer is "The equilibrium would shift to reduce the pressure change" on Apex
How did the addition of HCl affect the direction of the shift in equilibrium?
This may be innacurate but I am currently doing an AP question soo this is my best guess. I believe because when you wrtie the equation and then set up an ice table(or however you find equillbrium) HCl is in the equation so it must be taken into account. If something were to change like pressure this could determine what direction the reaction goes(forward or backwards) according to le' chateliers principle.
How would Le Chatelier's principle a change in pressure affect a gaseous system in equilibrium?
The equalibrium would shift to reduce the pressure
Pascal's principle states that a fluid in equilibrium enclosed by a vessel exerts pressure?
Equally in all direction.
What does Le Chatelier's principle state?
A reaction at equilibrium will respond to balance a change - apex (Explanation): The answer is NOT "a new equilibrium ratio will form", because although this is true, it will not necessarily always happen and is not what le chatelier's principle is about. His principle focuses on the reaction changing to cancel out or balance the change in equilibrium. Therefore, this is the correct answer.
What is the LeChatlier?
The Chatelier's Principle states that when a dynamic equilibrium is disturbed by changing conditions then the position of equilibrium shifts to counteract the change to reestablish equilibrium. A chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products , equilibrium will shift in opposite directions to offset change.
Why is it important to use high pressure in the Haber process?
The Haber process is basically converting Nitrogen and Hydrogen into ammonia. The equation is N2 + 3H2 -------> 2NH3 but it is an equilibrium. By Le Chetalier's principle if we apply pressure the system will try to counteract that by trying to lower pressure and to do this it needs to form product because there are 4 molecules of reactants and only two of product so the pressure is lower when there are fewer molecules. High Pressure thus favors high yields and hence good productivity and profitability.
How could you increase the production of 2NH3(g) N2(g) plus 3H2(g) 2NH3(g) Increase the volume of the reaction vessel. Increase the pressure of the system. Decrease the pressure of the system. Remove?
Given N2(g) + 3H2(g) <---> 2NH3(g), increasing the pressure will cause more NH3 to form. According to LeChatelier's Principle, an increase in pressure moves the equilibrium in the direction where there are fewer moles (particles), which in this equilibrium, is to the right.
What does Le Ch and Atilde and centtelier's principle state?
Le Chatelier's principle states that a system at equilibrium will respond to stress by shifting to minimize the effect of the stress and re-establish equilibrium. This means that if a system is subjected to a change in concentration, temperature, or pressure, it will adjust its composition to counteract the change.
What happen to the movement of molecules at equillimbrium?
The movement of molecules at equilibrium is determined by Le Chatalier's principle. This basically says that if you change a reaction to favour one side, the equilibrium will try and counteract this change. The three things that can affect an equilibrium is temperature, pressure and concentration.
What is an equilibrium in meteorology?
I am a meteorologist. An equilibrium, as it pertains to meteorology, most likely applies to a pressure equilibrium - or equalization of pressure. "Equilibrium" means balance, or balanced.
