Chemical Equilibrium Formula
When a chemical reaction happens, the reactants first start colliding together and responsible to make products. When the reaction is in progress, the quantity of product will start increasing at particular situations, and it may turn back to reactants as well. As soon as the rate of forwarding reaction becomes very much equal to the backward reaction, the situation is named as the chemical equilibrium. During a reaction, when it achieves the stage of equilibrium, this is possible to calculate the law of mass action. So, the chemical equilibrium formula in Chemistry for a set of reactants can be given as –
Where,
- Kc = The equilibrium constant using the molar concentrations of reactants and products.
- Xx and Yy = Are the product concentrations raised to the power of their coefficients
- Aa and Bb = Are the reactant concentrations raised to the power of their coefficients
- = Signifies the reaction is at equilibrium
During a reaction, when the concentration of the reactants and products is not changing over the time for a long time span, the situation is chemical equilibrium. They are further divided into multiple categories like homogeneous equilibrium, Heterogeneous equilibrium etc. In the case of homogeneous equilibrium, all reactants are available in the same phase, and this is not possible to separate them. At the same time, for heterogeneous equilibrium, reactants and products are not available in the homogenous phase, and you could separate them as per the convenience.
You must be wondering what could be the criteria for the Chemical Equilibrium –
- The reaction should happen in the closed vessel only.
- The pressure, temperature, and the concentration of the reactants should remain constant.
- The reaction should always be reversible.
Keep in mind that during the chemical equilibrium stage, both reactants and products are in the same sage but the rate of constants is different.