The equilibrium constant for a chemical reaction relates to the amount of reactant and product at the state when they are in equilibrium. The same can be represented by using a given normal equation. In an equation, if represent the molar concentration of the element P, and similarly represent the molar concentration of element R, Q, and S respectively. Then, while representing, the coefficient gets converted into the exponents of the concentration for the given expression. The equilibrium constant is a numerical value for any given reaction at a particular temperature, and each reaction has its own characteristic equilibrium constant. The concentration mentioned in the equation for the reaction and product are related to each other and thus they can’t be random values, rather they are dependent on one another. The denominator contains the concentrations of the reactants while the numerator consists of the concentration of the products. Now let’s take another example in which p represents the coefficient of the reactant P which gives out the product, wherein, q represents the coefficient of Q. This equation consists of only one reactant and one product with the coefficient p and q. So, the equilibrium constant expression for the same would be, the ratio of Q with power q to that of P with power p. Now for example, if you take the concentration of reactant to be 6 and the concentration of product to be 5, while the value of coefficient and, then on putting the values we get the equilibrium constant equals to 5/6=0.83. There are certain heterogeneous equilibrium reactions in which the reactants and products of the equation are found to be in different phases. These phases may include liquid, solid, or gas. So in such a case, we have a different rule, that is the concentrations of reactant and product in the solid and liquid form would not be considered for heterogeneous equilibrium. Only the concentrations of gas-phase would be included in the equilibrium constant expressions.
Dependence on Pressure, Temperature and Catalyst
The value of is tends to decrease with the increase in temperature. In the case of an exothermic reaction, increasing the temperature would lead to the decrease in the equilibrium constant value whereas in the case of an endothermic reaction increasing the temperature would lead to the increase in the constant equilibrium value. According to le chatelier’s principle, if one changes the temperature of a reaction, then the reaction proceeds in such a way that it aims at undoing the changes made. Such that if we decrease the temperature, the reaction will move forward to increase the temperature and vice versa. Again according to le chatelier’s principle, if we change the pressure, there would be a change in the equilibrium such that if we increase the pressure, then the reaction will proceed forward to decrease the pressure. This can be done by favoring the reactions that produce fewer molecules. If the same number of molecules are present on either side of the equation, then pressure change would cause no effect on the equilibrium. When a catalyst is added to a reaction, the equilibrium constant will not be affected. Catalyst plays a role in speeding up the reaction so both the forward and backward reaction would carry the equal speed, do it would cause no effect to the equilibrium of the reaction.
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