1. What is the mass law constant? The law of action of mass states that a chemical reaction frequency is proportional to the active masses of materials reacting at constant temperature. Kc is the equilibrium reaction constant while Kp is the equilibrium constant found by applying partial pressure. The law of mass action states that the rate of a chemical reaction is proportional to the product of the concentrations of the reactants. To derive this law, we must first understand the collision theory of the chemical reaction. This theory states that a chemical reaction occurs when two atoms collide and form a new molecule. The reaction rate is determined by the frequency of these collisions. The law of mass action states that the reaction rate is proportional to the product of the concentrations of the reactants. This means that the more atoms collide, the faster the reaction. Reaction rate (alpha [{text{A}}][{text{B}}])(=text{K} [{text{A}}][{text{B}}]) The concentration quotient (QC) of a chemical reaction at a given temperature is defined as the ratio of the product to the concentrations of the products and those of the reactants. However, when the system reacts, the Qc value fluctuates, but the equilibrium concentrations determine the equilibrium constant Kc. Reactions without volume change: Reactions in which the volume remains unchanged are independent of pressure changes.
Le Chatelier`s principle states that for reactions that are in dynamic equilibrium, changes in concentration, pressure, or temperature shift the equilibrium position to counteract the change and establish a new state of equilibrium. In reversible reactions, when solids and liquids participate in the reaction, their concentrations are assumed as a unit. For this type of reaction, (rm{K}_rm{p}) is defined as ({{text{K}}_{text{p}}} = {{text{P}}_{{text{C}}{{text{O}}_2}}}left({{text{CaO}},{text{CaC}}{{text{O}}_3}} right.) are solids, (left. {{{text{P}}_{{text{CaO}}}} = {{text{P}}_{{text{CaC}}{{text{O}}_3}}} = 1.} right)) Consider hypothetically the following reversible reaction: Applying the formula of the law of mass action, the expression of the equilibrium constant for this reaction is: Law of mass action: In chemistry textbooks, we often read about multiple reactions, but have you ever wondered how one molecule transforms into another and how the reaction is carried out? Molecules are always moving. They are constantly exposed to collisions. And that`s when a molecule with enough energy collides with another molecule and turns into another. Therefore, the law of mass action dictates that the equilibrium constant at a given constant temperature is equal to the product of the concentration of the products increased to the respective stoichiometric coefficients divided by the product of the high reagent concentrations at the corresponding stoichiometric coefficient. We have understood the concept of the law of mass action and the importance of reversible and irreversible reactions. The derivation of the equilibrium constant and its use and application in different reactions. Forward reaction ( {text{aA}} + {text{bB}} to ,……..) ({vartheta _{text{f}}}alpha {[{text{A}}]^{text{a}}}{[{text{B}}]^{text{b}}}) ({vartheta _{text{f}}} = {{text{K}}_{text{f}}}{[{text{A}}{[{{{text{A}}{[{{text{A}}{}}{[{text{A}}}{{text{A}}{{text{A}}{{text{A}}}{{text{a}}} }}]^{text{a}}}{[{text{B}}]^{text{b}}}) The law of mass action can be applied both to the direct reaction ({text{aA}} + {text{bB}} to left({{text{products}}} right)) and vice versa Reaction ({text{cC}} + {text{dD}} to left({{text{reactants}}} right)). As shown below: In the same way, the reverse reaction rate will be: Reactions with volume increase: For reactions accompanied by an increase in volume, a pressure reduction increases the reaction rate. According to the law of mass action, the constant value obtained by the relation of equilibrium concentrations of reactants and products is called the equilibrium constant.
For the direct reaction, this is given by temperature: In endothermic reactions, an increase in temperature shifts the equilibrium to the right. Conversely, in exothermic reactions, an increase in temperature shifts the balance to the left. In a gas system, the law of mass action states that the pressure of the gas is proportional to the product of the number of gas particles and their average kinetic energy.