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Is it true that an example of a stress on an equilibrium is the increase of pressure in a closed system when the pressure of a reactant gas is increased from 1.0 ATM to 2.0 ATM?
Wiki User
∙ 12y ago
false
Wiki User
∙ 12y ago
Yes, increasing the pressure of a reactant gas in a closed system at equilibrium will shift the equilibrium towards the side with fewer moles of gas molecules to counteract the increase in pressure. This is in accordance with Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract any external stress applied to it in order to reestablish equilibrium.
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What will be the consequences of adding or removing a reactant or aproduct from a reaction that is at dynamic equilibrium?
Adding a reactant will shift the equilibrium towards the products to counteract the change. Removing a reactant will shift the equilibrium towards the reactants. Adding a product will shift the equilibrium towards the reactants to counteract the change, while removing a product will shift the equilibrium towards the products.
How does an equilibrium reaction respond to the addiof extra reactant?
Adding extra reactant to an equilibrium reaction will shift the equilibrium towards the products side, in order to consume the added reactant and establish a new equilibrium. This occurs to maintain the equilibrium constant and keep the reaction mixture stable.
Explain chemical equilibrium shifts to favor products?
Chemical equilibrium shifts to favor products when the concentration of products is decreased or the concentration of reactants is increased. This can be achieved by removing some of the product or adding more reactant to the system. Le Chatelier's principle states that a system at equilibrium will respond to changes in concentration, pressure, or temperature by shifting in a direction that helps restore equilibrium.
Why are high temperature and pressure needed for the harbor process?
High temperature and pressure are needed for the Haber process because they help improve the reaction rate and equilibrium yield of ammonia. The increased temperature allows for more collisions between reactant molecules, while high pressure helps to favor the formation of ammonia by reducing the volume of the gas mixture.
When equilibrium shifts to the reactants in response to stress how is the equilibrium position changed?
When equilibrium shifts to the reactants in response to stress, the equilibrium position shifts in the direction that helps counteract the stress applied. This can involve an increase in reactants or a decrease in products to restore equilibrium.
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 does changing the concentration of reactant shift the equilibrium?
Changing the concentration of a reactant shifts the equilibrium because Le Chatelier's principle states that a system at equilibrium will respond to any external change in order to minimize the effect of that change. If you increase the concentration of a reactant, the system will shift towards the product side to reduce that increase, and vice versa.
How does an equilibrium reaction respond to the addiof extra reactant?
Adding extra reactant to an equilibrium reaction will shift the equilibrium towards the products side, in order to consume the added reactant and establish a new equilibrium. This occurs to maintain the equilibrium constant and keep the reaction mixture stable.
What happens when reactant is added to a system at equilibrium?
The equilibrium of the system will be upset.
What does Le Châtelier's principle say about upsetting a system at equilibrium?
Le Châtelier's principle states that when a system at equilibrium is upset by an external stress, the system will shift to counteract the change and restore equilibrium. For example, if you increase the concentration of a reactant, the system will shift to produce more product to restore equilibrium.
What will happen when a reactant is added to a system at equilibrium?
The equilibrium of the system will be upset.
Explain chemical equilibrium shifts to favor products?
Chemical equilibrium shifts to favor products when the concentration of products is decreased or the concentration of reactants is increased. This can be achieved by removing some of the product or adding more reactant to the system. Le Chatelier's principle states that a system at equilibrium will respond to changes in concentration, pressure, or temperature by shifting in a direction that helps restore equilibrium.
How does pressure speed up a chemical reaction?
Increasing pressure can speed up a chemical reaction by bringing reactant particles into closer contact more frequently, leading to more successful collisions. This increased pressure can also alter the equilibrium of the reaction, favoring the formation of products. Additionally, higher pressure can increase the energy of the collisions between reactant particles, making them more likely to overcome the activation energy barrier for the reaction to occur.
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?
Increasing the volume of the reaction vessel would shift the equilibrium towards the side with more moles of gas (the reactants), so more NH3 would be produced. Increasing the pressure of the system would favor the side with fewer moles of gas (the products), so it would decrease NH3 production. Removing NH3 as it is produced would also shift the equilibrium towards the reactant side, increasing NH3 production.
If a reactant rather than a product would be colored could an equilibrium constant be calculated for a specific reaction stoichiometry?
Yes, you can calculate an equilibrium constant for a reaction involving a colored reactant. As long as the reaction is at equilibrium, the equilibrium constant can be determined using the concentrations of reactants and products. The color of a reactant does not prevent the calculation of an equilibrium constant.
Why are high temperature and pressure needed for the harbor process?
High temperature and pressure are needed for the Haber process because they help improve the reaction rate and equilibrium yield of ammonia. The increased temperature allows for more collisions between reactant molecules, while high pressure helps to favor the formation of ammonia by reducing the volume of the gas mixture.
What would happen to the amount of products if you increase the amount of one of the reactants?
Increasing the amount of one reactant typically increases the amount of products produced until the reactant is used up. Once the reactant is exhausted, the reaction will reach equilibrium and the amount of products will no longer increase.
