0
What will happen to the concentration of reactants after an equilibrium reaction shifts to the left?
Wiki User
∙ 10y ago
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.
Wiki User
∙ 16y ago
Add your answer:
Earn +20 pts
What would happen to a system at equilibrium of more of one compound in a reaction were added?
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
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.
Do the forward and reverse reactions stop at equilibrium?
A Reversible reactions is a chemical phenomenon. This happens when in a reaction the reactants transform from the reactants into there products. This is what happens normally in a reaction. However in a reversible reaction the product that has been form goes back into its reactants. Then the newly formed reactants react into there products and the process is repeated. In plain english it means the what you have created returns into its original form. Its much clearer in a equation: A → B represents the transformation of the reactants (A) into the product (B), Once a product is formed its decomposes into its reactants B → A and so on is the process repeated i.e A ←→ B.
Hat will happen when a reactant is added to a system at equilibrium?
The concentrations of reactants and products are modified.
When a reaction is at the equilibrium's will increasing pressure favor the reaction that produces more gas?
Not usually. This could only happen if the gas produced were so far from ideal that its production reduces the pressure of the total mixture of reactants and products, a very unlikely occurrence.
what would happen to a system at equilibrium of more one compound on a reaction were added?
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
What would happen to a system at equilibrium of more of one compound in a reaction were added?
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
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.
A higher concentration of molecules causes a faster chemical reaction This is known as?
This is known as chemical equilibrium. All of the chemicals will want to become stable and this can only happen with equilibrium.
Do the forward and reverse reactions stop at equilibrium?
A Reversible reactions is a chemical phenomenon. This happens when in a reaction the reactants transform from the reactants into there products. This is what happens normally in a reaction. However in a reversible reaction the product that has been form goes back into its reactants. Then the newly formed reactants react into there products and the process is repeated. In plain english it means the what you have created returns into its original form. Its much clearer in a equation: A → B represents the transformation of the reactants (A) into the product (B), Once a product is formed its decomposes into its reactants B → A and so on is the process repeated i.e A ←→ B.
What occurs when the forward and reverse reactions occur at the same rate?
If a forward and reverse reaction happen at the same rate, the result is called a dynamic equilibrium; the overall chemical composition does not change, even though reactions are constantly taking place.
Hat will happen when a reactant is added to a system at equilibrium?
The concentrations of reactants and products are modified.
What would happen if NO were added to N2g O2 g 2NO g at equilibrium?
Adding NO to the system at equilibrium would increase the concentration of the NO product. According to Le Chatelier's principle, the system will counteract this change by producing more of the reactants, N2 and O2.
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 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.
When a reaction is at the equilibrium's will increasing pressure favor the reaction that produces more gas?
Not usually. This could only happen if the gas produced were so far from ideal that its production reduces the pressure of the total mixture of reactants and products, a very unlikely occurrence.
What change will most likely increase the rate of a chemical reaction?
Factors which can increase the rate of a chemical reaction:- temperature- pressure- concentration of reactants- stirring- if solids are involved the dimension of particles is important- the type of reaction- the order of reaction- presence of catalysts- influence of external factorsetc.
