Chemical Equilibrium: Definition, Laws, Formulas, Example Problems
Chemical Equilibrium: Definition, Laws, Formulas, Example Problems – In this discussion, we will explain chemical equilibrium, formula laws and complete and easy examples of chemical equilibrium. For more details, please see the review below carefully.
Chemical Equilibrium: Definition, Laws, Formulas, Example Problems
Let's discuss the meaning of chemical equilibrium first carefully.
Definition of Chemical Equilibrium
Chemical equilibrium is an alternating reaction in which the reaction rates of the reactants and products are the same and the concentrations of both are constant. Chemical equilibrium occurs only in alternating reactions in which the rate of formation of the reactants is equal to the rate of formation of the products.
Chemical equilibrium has dynamics, so it is often called dynamic equilibrium. Dynamic equilibrium is an alternating reaction in which the conditions of concentration are constant but the reaction is actually continuing. Dynamic equilibrium does not occur macroscopically but occurs microscopically (substance particles).
Chemical equilibrium occurs only in alternating reactions in which the rate of formation of the reactants is equal to the rate of formation of the products. The reaction will occur continuously microscopically so it can be called a dynamic equilibrium.
Characteristics of a State of Equilibrium
The characteristics of a state of equilibrium are as follows:
- Occurs in a closed container, with constant temperature and pressure
- The rate of reaction to the reactants is equal to the rate of reaction to the products
- The reaction proceeds continuously (dynamically) in two opposite directions
- Occurrence is very microscopic at the particle level of matter
- The concentrations of products and reactants are fixed
Shifts in Chemical Equilibrium
There are several factors that influence chemical equilibrium, including concentration, temperature, and pressure or volume.
Effect of Substance Concentration on Chemical Equilibrium
If the concentration of one of the substances is increased, then the equilibrium reaction will shift towards (away from) the substance with which the concentration is added. If the concentration of one of the substances is reduced, the equilibrium reaction will shift in the direction of the substance being reduced in concentration.
Example: In the following reaction equation
N2(g) + 3H2(g) <==> 2NH3(g) H = -92 kJ.
If the concentration of N2 is added, the equilibrium reaction will shift to the right, because if the concentration of the substance is added, the reaction equilibrium will shift from the direction of the added concentration.
If the N2 concentration is reduced, the equilibrium reaction will shift to the left, because if the concentration of the substance is reduced, the equilibrium reaction will shift from the direction of reduced concentration.
Effect of Pressure and Volume on Chemical Equilibrium
If the pressure in the system is increased or the volume is reduced, the reaction equilibrium will shift towards a smaller number of molecules.
If the pressure on the system is reduced or the volume is increased, the equilibrium reaction will shift towards a smaller number of molecules.
"pressure and volume are inversely related"
Example: In the following reaction equation
N2(g)+ 3H2(g) <==> 2NH3(g) H = -92 kJ
Number of moles of reactants = 1 + 3 = 4
The number of moles of product = 2
If the pressure in the system is increased, the equilibrium reaction will shift to the right, because if If the pressure is increased, the reaction equilibrium will shift in the direction of the least number of molecules ie 2.
If the volume in the system is reduced then the equilibrium reaction will shift to the right, because if If the volume of the system is reduced then the reaction equilibrium will shift in the direction of smaller molecules ie 2.
If the pressure in the system is reduced then the equilibrium reaction will shift to the left, because if the pressure is increased. So the equilibrium reaction will shift towards the larger number of molecules i.e. 4.
If the pressure in the system is increased, the equilibrium reaction will shift to the left, because if the volume of the system is increased. So the equilibrium reaction will shift in the direction of a larger number of molecules, namely 4.
Effect of Temperature on Chemical Equilibrium
If the temperature of the system is raised, the equilibrium reaction will move towards the substance that releases heat or is endothermic.
If the temperature of the system is reduced, the equilibrium reaction will move in the direction of the substance that releases heat or is exothermic.
Example: In the reaction equation
[A] + [B] <==> [C] H = -X
[C] is an exothermic reaction (releases heat and [A] + [B] is an endothermic reaction (requires heat)
If the temperature is increased then the equilibrium reaction will move to the left because if the temperature system is increased then the equilibrium reaction will shift in the direction of the reaction that requires heat or endothermic
If the temperature is lowered, the equilibrium reaction will move to the right because if the temperature system is increased then the equilibrium reaction will shift towards the reaction direction that requires heat or endothermic
If the temperature is lowered, the equilibrium reaction will move to the right because if If the temperature of the system is increased, the reaction equilibrium will shift in the direction that releases heat exothermic
Laws of Chemical Equilibrium
The law of chemical equilibrium or the equilibrium constant is the ratio of the product concentrations to the coefficient rank of each reactate concentration to the respective coefficient rank. The equilibrium constant can be symbolized by K or Kc.
General Formula of Chemical Equilibrium
The chemical equilibrium equation or formula is as follows:
Heterogeneous Equilibrium
The forms of the substances involved in the reactions at this heterogeneous equilibrium are different, hence those taken in determining the equilibrium constant is the concentration of the substance whose equilibrium constant is affected is the solution and gas.
Homogeneous Equilibrium
In this homogeneous equilibrium, the forms of the substances involved in the reaction are the same, so all the concentrations of substances are used to determine the equilibrium constant. But it must be remembered that only gases and solutions affect the equilibrium constant.
Example of a Chemical Equilibrium Problem
Given an equilibrium reaction
2A + B <==> A2B
Initially in a 2 liter vessel there are 2 mol A and 2 mol B, if in equilibrium 0.5 mol A, what is the equilibrium constant?
Answer:
Based on the statement above, the number of moles can be determined as follows:
So:
The volume in the problem has an effect because it will cancel each other out.
Partial Equilibrium Constant
The partial equilibrium constant is the ratio of the product of the partial pressures of the products at the respective coefficient level to the partial pressures of the reactants at the respective coefficient level. The partial equilibrium constant can be symbolized by Kp.
Information
P = partial pressure
Information:
pX = partial pressure to be found
nX = moles of the substance whose partial pressure will be found
En = total moles of the system
Ep = total partial pressure of the system
Problems example:
As much as 6 mol of NH3 is heated to become N2 and H2. When equilibrium is reached, 2 mol of NH3 remains, if the total pressure of the gas mixture is 10 atm, determine the value of Kp!.
Answer:
From the questions above, we can get the following data:
Total moles in the system:
Find the partial pressure on each substance with the equation:
So we get pBH3 = 2 atm, pN2 = 2 atm, and pH2 = 6atm
Equilibrium Partial Pressure Relationship with Equilibrium Constant
This relationship can be expressed in the following equation:
Information:
R = Gas constant
T = Temperature
p, q, m and n = coefficients of the reacting substances
Degree of dissociation
The degree of dissociation is a value used to determine how much of a substance dissociates. The equation for the degree of dissociation is:
The meaning of the equilibrium constant
The equilibrium constant can be used for several functions, including:
- Gives clues about the position of equilibrium
- Estimate the direction of the reaction
Thus has been explained about Chemical Equilibrium: Definition, Laws, Formulas, Example Problems, hopefully can add to your insight and knowledge. Thank you for visiting and don't forget to read other articles.
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