The reaction would shift to balance the change
The reaction would shift to balance the change
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
The reaction quotient indicates the relative amounts of products and reactants present in a system at a given time compared to what would be present at equilibrium. It helps determine the direction a reaction will shift to reach equilibrium.
No, the equilibrium constant is independent of concentration as long as the ratio of products and reactants remains as is. It can be effected by anything that would influence the ratio of products and reactants, such as changes in temperature or the addition of a catalysis.
The reaction 2O₃(g) ⇌ 3O₂(g) represents the decomposition of ozone (O₃) into oxygen (O₂). If the reaction is at equilibrium and conditions such as temperature or pressure change, the equilibrium position may shift according to Le Chatelier's principle. An increase in temperature would favor the formation of O₂, while decreasing the pressure could also shift the equilibrium to the right, producing more O₂. Conversely, lowering the temperature or increasing the pressure would favor the formation of O₃.
The reaction would shift to balance the change
The reaction would shift to balance the change
The reaction would shift to balance the change
The reaction would shift to balance the change
The reaction would shift to balance the change
The concentration of products would increase. apex
The base dissociation constant (Kb) for a weak base is the equilibrium constant for the reaction of the base with water to produce hydroxide ions. In this case, the expression for Kb would be [OH-][BH]/[B].
If a weak acid dissociation were upset, the equilibrium would shift to try to restore the balance of reactants and products. This could result in changes to the pH of the solution and the concentration of the acid and its conjugate base. Ultimately, the system would try to reach a new equilibrium point.
If more product is added to a weak base dissociation equilibrium, Le Chatelier's principle predicts that the equilibrium will shift to the left towards reactants to relieve the stress caused by the increase in product concentration. This will result in more reactant molecules being formed.
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
If the added substance is a reactant, the equilibrium shifts toward products. If it is a product, it moves towards reactants.
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.