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All motion ceases
The equilibrium constant (K) indicates the relative amounts of reactants and products at equilibrium in a chemical reaction. Specifically, it shows the ratio of product concentrations to reactant concentrations when the reaction has reached equilibrium. A large equilibrium constant suggests the reaction favors products, while a small equilibrium constant indicates a preference for reactants.
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.
If one of the products of a chemical reaction is removed, the equilibrium of the reaction will shift towards the side to produce more of that product to reach a new equilibrium state. This is known as Le Chatelier's Principle.
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.
All motion ceases
All motion ceases
The equilibrium constant (K) indicates the relative amounts of reactants and products at equilibrium in a chemical reaction. Specifically, it shows the ratio of product concentrations to reactant concentrations when the reaction has reached equilibrium. A large equilibrium constant suggests the reaction favors products, while a small equilibrium constant indicates a preference for reactants.
Reaction rate refers to the speed at which reactants are consumed and products are formed in a chemical reaction, while equilibrium is a state in which the rates of the forward and reverse reactions are equal, leading to no net change in concentrations of reactants and products. The rate of the forward reaction is equal to the rate of the reverse reaction at equilibrium.
No, in a chemical reaction at equilibrium the rates of the forward and reverse reactions are equal, so the amounts of products and reactants remain constant. The reaction has reached a balance point where there is no net change in the concentrations of products and reactants.
If one of the products of a chemical reaction is removed, the equilibrium of the reaction will shift towards the side to produce more of that product to reach a new equilibrium state. This is known as Le Chatelier's Principle.
Dynamic equilibrium has been reached.
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.
Every physical phenomenon is an example of equilibrium; whenever there is conservation ,if you look closer, there is equilibrium. The action reaction principle is one example.
Many chemical reactions, like combustion , go to completion and not to equilibrium. It is normally desirable to give a chemical reaction time to reach equilibrium in order you get the maximum yield of one or more products.
A promoter catalyst can increase the rate of both the forward and reverse reactions in a reversible reaction without affecting the position of the equilibrium. It achieves this by lowering the activation energy, allowing the reaction to reach equilibrium more quickly but not altering the ratio of products to reactants at equilibrium.
Equal. At equilibrium, the rates of the forward and reverse reactions are balanced, meaning that the rate of the forward reaction is equal to the rate of the reverse reaction. This results in no net change in the concentrations of reactants and products over time.