Le Chatelier's Principle states that an equilibrium will shift under conditions of stress in such a way as to remove that stress. Most chemical reactions appear to go to completion and stop there but under the correct conditions all chemical reactions are reversible. When forward and reverse reactions are proceeding at the same rate a state of dynamic equilibrium is established, both reactions will occur. Le Chatêlier’s principle allows us to predict the effects of a stress placed on a system at equilibrium. The stress produces a shift in concentrations that may be seen as changes in the properties of the system.
If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. A + 2B --> C + D , if conc. A is increased, the equilibrium position will shift to the right. According to Le Chatelier, the position of equilibrium will move in such a way as to counteract the change. That means that the position of equilibrium will move so that the pressure is reduced again. Pressure is caused by gas molecules hitting the sides of their container. The more molecules you have in the container, the higher the pressure will be. The system can reduce the pressure by reacting in such a way as to produce fewer molecules.
Le Chatelier's principle creates a shift in a dynamic reaction's equilibrium position to counteract the affect of a disturbance produced by either a change in temperature, pressure, or concentration. Its ulterior motive for doing so is to make qualitative predictions about how a reaction's equilibrium responds to various external conditions. Also, Le Chaltelier's principle prove that when a reaction's external factors are altered the dynamic equilibrium will shift until the new state of balance is attained or reached. (A reaction at dynamic equilibrium is in a "dynamic" state of balance) This principle can informally be compared to the method of an object's self-correction to adapt to new conditions.
Le Chatelier's principle states that if a dymanic equilibrium is disturbed by cahnging the conditions, the postition of equilibrium moves to counteract the change.
Temp: In exothermic reactions, increase in temperature decreases the equilibrium constant, K. While in endothermic reactions, increase the K value.
Pressure: An increase in presure due to a decrease in volume cause the reaction to shift to the side with fewer gas moles. A decrease in pressure due to an increase in volume auses the reaction to shift to the side with more gas moles. There is no effect on a reaction where the number of moles of gas is the same on each side of the equation.
Le Chatelier's Principle states that an equilibrium will shift under conditions of stress in such a way as to remove that stress. Most chemical reactions appear to go to completion and stop there but under the
ReplyDeletecorrect conditions all chemical reactions are reversible. When forward and reverse reactions are proceeding at the same rate a state of dynamic equilibrium is established, both reactions will occur. Le Chatêlier’s principle allows us to predict the effects of a stress placed on a system at equilibrium. The stress produces a shift in concentrations that may be seen as changes in the properties of the system.
If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
ReplyDeleteA + 2B --> C + D , if conc. A is increased, the equilibrium position will shift to the right.
According to Le Chatelier, the position of equilibrium will move in such a way as to counteract the change. That means that the position of equilibrium will move so that the pressure is reduced again. Pressure is caused by gas molecules hitting the sides of their container. The more molecules you have in the container, the higher the pressure will be. The system can reduce the pressure by reacting in such a way as to produce fewer molecules.
Le Chatelier's principle creates a shift in a dynamic reaction's equilibrium position to counteract the affect of a disturbance produced by either a change in temperature, pressure, or concentration. Its ulterior motive for doing so is to make qualitative predictions about how a reaction's equilibrium responds to various external conditions. Also, Le Chaltelier's principle prove that when a reaction's external factors are altered the dynamic equilibrium will shift until the new state of balance is attained or reached. (A reaction at dynamic equilibrium is in a "dynamic" state of balance) This principle can informally be compared to the method of an object's self-correction to adapt to new conditions.
ReplyDeleteLe Chatelier's principle states that if a dymanic equilibrium is disturbed by cahnging the conditions, the postition of equilibrium moves to counteract the change.
ReplyDeleteTemp:
In exothermic reactions, increase in temperature decreases the equilibrium constant, K. While in endothermic reactions, increase the K value.
Pressure:
An increase in presure due to a decrease in volume cause the reaction to shift to the side with fewer gas moles. A decrease in pressure due to an increase in volume auses the reaction to shift to the side with more gas moles. There is no effect on a reaction where the number of moles of gas is the same on each side of the equation.
Your responses are awesome. I am not convinced by the the effect of temperature on the position of equilibrium. Is it possible for you to explain?
ReplyDelete