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What happens to the yield of ammonia when the concentration of reactant is increased?
Increasing the concentration of reactants typically increases the yield of ammonia. According to Le Chatelier's principle, the equilibrium will shift to the right to counteract the increase in reactant concentration, favoring the production of more ammonia.
What happens when reactant is added to a system at equilibrium?
The equilibrium of the system will be upset.
What is the effect of adding more water to the following equilibrium reaction?
Equilibrium is pushed to the reactant side
What causes the equilibrium to shift to the left?
The equilibrium shifts to the left when there is an increase in the concentration of reactants or a decrease in the concentration of products. This can also happen when the temperature is decreased in an exothermic reaction.
What does Le Châtelier's principle say about upsetting a system at equilibrium?
When a change is imposed on a system at equilibrium, the "position" of the equilibrium shifts in a direction that reduces the effects of that change. For example, if a reactant or product is added, the system shifts AWAY FROM that added component to use the excess up. If heat is added, the system shifts AWAY FROM that added energy energy to use the excess up. If the pressure on a system is increased, the system shifts toward the side with fewer gas molecules.
What would happen when a reactant is added to a system at equilibrium?
When a reactant is added to a system at equilibrium, the concentration of that reactant increases, causing the system to shift in the direction that consumes the added reactant according to Le Chatelier's principle. This shift will favor the forward reaction, leading to the production of more products until a new equilibrium is established. As a result, the concentrations of products will increase while the concentrations of the original reactants will adjust back to equilibrium levels.
What happens to the yield of ammonia when the concentration of reactant is increased?
Increasing the concentration of reactants typically increases the yield of ammonia. According to Le Chatelier's principle, the equilibrium will shift to the right to counteract the increase in reactant concentration, favoring the production of more ammonia.
Why did the addition of potassium thiocyanate cause the equilibrium to shift the way it did which ion causedthis shift?
The addition of potassium thiocyanate (KSCN) introduces thiocyanate ions (SCN⁻) into the equilibrium system. According to Le Chatelier's principle, the equilibrium will shift to counteract the increase in SCN⁻ concentration, often favoring the formation of products if SCN⁻ is a reactant in the equilibrium. This shift occurs because the system seeks to re-establish equilibrium by reducing the concentration of the added ion.
What happens if you add a reactant to a reversible reaction?
If you add a reactant to a reversible reaction, the equilibrium will shift to favor the formation of products in order to counteract the change, according to Le Chatelier's principle. This shift can increase the rate of the forward reaction, leading to the production of more products until a new equilibrium is established. The extent of this shift depends on the concentration of the added reactant and the specific conditions of the reaction.
How does an equilibrium reaction respond to the addiof extra reactant?
The concentration or activity of the product(s) will increase, and if there is at least one other reactant than the added one that is required for the completion of the reaction, the concentration of such an unadded reactant will decrease. (If there were no available unadded reactant, the reaction would not technically have been in equilibrium at the start, even though it may have reached a steady state that can persist for a long time in the absence of changed conditions.)
What happens when reactant is added to a system at equilibrium?
The equilibrium of the system will be upset.
What does Le Chatelier?
Le Chatelier's principle states that if a system at equilibrium is disturbed by changing the concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. For example, if a reactant is added, the equilibrium will shift to favor the formation of products. This principle is fundamental in understanding how chemical reactions respond to changes in their environment.
What will be the consequences of adding or removing a reactant or aproduct from a reaction that is at dynamic equilibrium?
if reaction is at equ. then adding product will cause reaction to proceed forward and product will increase and removing product will do the same while removing reactant will cause reactn 2 proced bakward and reactant will increase and adding product wl do the same it is in accordnc wth LeChateliars principle
When equilibrium shifts to the reactants in response to stress how is the equilibrium position changed?
When the concentration increases, the equilibrium shifts away from the substance. Equilibrium is based on the molarity of the reactants. Increasing concentration increases the amount of that reactant in the solution.
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.
Which set of changes would be best to shift the equilibrium to the right in this system?
To shift the equilibrium to the right in a chemical system, you can increase the concentration of the reactants, decrease the concentration of the products, or increase the temperature if the reaction is endothermic. Additionally, removing a product or adding a catalyst may also help facilitate the forward reaction without changing the overall equilibrium position. Changes that favor the formation of products will effectively drive the equilibrium to the right.
What is the effect of adding more water to the following equilibrium reaction?
Equilibrium is pushed to the reactant side
