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Why does changing the concentration of reactant shift the equilibrium?
Wiki User
∙ 11y ago
Wiki User
∙ 12y ago
Wiki User
∙ 11y agoChanging the concentration of an ingredient will shift the equilibrium to the side that would reduce that change in concentration. The chemical system will attempt to partially oppose the change affected to the original state of equilibrium. In turn, the rate of reaction, extent and yield of products will be altered corresponding to the impact on the system.
Wiki User
∙ 11y agoIf there are gases involved, the equilibrium shifts. An increase in pressure will shift the equilibrium to the side with fewer molecules of gas.
Wiki User
∙ 7y agoBy temperature change.
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What would happen to a weak acid dissociation if more reactants were added?
Concentration of products would increase in order to attain equilibrium in the system again.For example:H2CO3 --> H+ + HCO3-K= ([H+][žHCO3-])/([H2CO3])K is constant for this process, so if you increase the concentration of reactants (H2CO3), in order for K to stay the same, concentration of products (H+, HCO3-) would also have to increase.It's part of Le Chatelier's principle: "If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established."So, in your case, adding more reactant would cause equilibrium to shift to the right (toward products), and therefore, their concentration would increase so that new equilibrium could be established.
How will increasing the temperature affect the equilibrium?
It depends if the reaction is exothermic or endothermic. For example: If the reaction requires energy (endothermic), then energy (i.e. 100kJ) will be a reactant on the left-hand side. Then, use Le Chatelier's Principle from there. If you increase the temperature of the system in equilibrium, it will shift towards the product/right-hand side. If you decrease the temperature of the system, it will shift towards the reactants/left-hand side.
How will decreasing the reactant concentration affect the reaction?
It depends on the order of the reaction. If it is zero order, decreasing the reactant concentration will have NO effect on the rate. If it is 1st or 2nd order (or more), then decreasing the concentration will DECREASE the reaction rate.
What does Le Châteliers principle state?
Le Chatelier's principle essentially states that if a stress is imposed on a system at equilibrium, the equilibrium will shift to minimize the stress. These stresses include: -Change in temperature -Change in pressure/volume (for gases) -Change in concentration A simple example of this: N2(g) + 3 H2(g) ⇌ 2 NH3(g) ΔH = −92kJ/mol -If you add N2(g) or 3 H2(g) the equilibrium will shift to the right (to the products), and more NH3(g) will be created so as to minimize the stress. - If you add NH3(g), the equilibrium will shift to the left (to the reactants), and more N2(g) and H2(g) will be created. -If you increase the temperature, the equilibrium will shift to the left (to the reactants). The reason for this is that the above reaction is exothermic, and releases heat. Consequently, the heat is on the side of the products, and thus if you add heat, the equilibrium will shift to the reactants and more N2(g) and H2(g) will be created. - If you increased the pressure, which is the same as decreasing the volume, the reaction will shift to the side with fewer moles, which, in this case, is the products. Thus, more NH3(g) will be created. -Conversely, if you decrease the pressure (increase the volume), the reaction will shift to the side with a greater number of moles, which, in this case, is the reactants. Thus, more N2(g) and H2(g) will be created. *It is important to note that changing pressure and volume only effects the equilibrium in gaseous reactions!
What does Le Chtelier's principle say about upsetting a system at equilibrium?
Le Chatelier principle says, if a restriction is applied to a system in equilibrium, the system adjusts to a new equilibrium that tends to counteract the restriction. When equilibrium is under stress it will shift to relieve that stress. or all concentrations would change.
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.
What will happen to a weak acid dissociation equilibrium if more reactants were added?
Concentration of products would increase in order to attain equilibrium in the system again.For example:H2CO3 --> H+ + HCO3-K= ([H+][žHCO3-])/([H2CO3])K is constant for this process, so if you increase the concentration of reactants (H2CO3), in order for K to stay the same, concentration of products (H+, HCO3-) would also have to increase.It's part of Le Chatelier's principle: "If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established."So, in your case, adding more reactant would cause equilibrium to shift to the right (toward products), and therefore, their concentration would increase so that new equilibrium could be established.
What is mean of dynamic equilibirum in chemistry?
An equilibrium is a "balance", if something is in equilibrium then it is in balance. To add "static" is an unnecessary tautology except in the case of a mechanical equilibrium with zero linear momentum.
What would happen to a weak acid dissociation if more reactants were added?
Concentration of products would increase in order to attain equilibrium in the system again.For example:H2CO3 --> H+ + HCO3-K= ([H+][žHCO3-])/([H2CO3])K is constant for this process, so if you increase the concentration of reactants (H2CO3), in order for K to stay the same, concentration of products (H+, HCO3-) would also have to increase.It's part of Le Chatelier's principle: "If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established."So, in your case, adding more reactant would cause equilibrium to shift to the right (toward products), and therefore, their concentration would increase so that new equilibrium could be established.
What will happen to the concentration of reactants after an equilibrium reaction shifts to the left?
Increasing the concentration of reactants will shift the equilibrium towards the products. The equilibrium will always shift to reduce the change you caused. If you add more products, it shifts toward reactants. This is known as the Le Chatelier Principle.See the Web Links to the left of this answer for more about this.
How are the terms stress and shift used when discussing systems at equilibrium?
In equilibrium, stress means the manner in which equilibrium is altered, and shift represents which direction the equilibrium will move to compensate for the stress.
How does removing ammonia from the process affect equilibrium?
it depends if the ammonia OS on the reactants or the products side. The equilibrium will shift toward whatever side the ammonia has been removed from (or away from whatever has been added), to balance the concentration of ammonia.
How will increasing the temperature affect the equilibrium?
It depends if the reaction is exothermic or endothermic. For example: If the reaction requires energy (endothermic), then energy (i.e. 100kJ) will be a reactant on the left-hand side. Then, use Le Chatelier's Principle from there. If you increase the temperature of the system in equilibrium, it will shift towards the product/right-hand side. If you decrease the temperature of the system, it will shift towards the reactants/left-hand side.
How will decreasing the reactant concentration affect the reaction?
It depends on the order of the reaction. If it is zero order, decreasing the reactant concentration will have NO effect on the rate. If it is 1st or 2nd order (or more), then decreasing the concentration will DECREASE the reaction rate.
What happens to the equilibrium price and equilibrium quantity in a market if the demand curve shifts to the right?
If the demand shift to the right, the equilibrium price and quantity will shift from the initial equilibrium price and quantity to the next, i mean the equilibrium price and quantity will increase as compare to the first.
What does Le chateliers principal say about upsetting system at equilibrium?
A system of whose equilibrium has been upset will shift to restore equilibrium.
