Equilibrium helps us to control the reaction conditions to favor formation of desired products. It is also useful in calculation of composition of final reaction mixture.
Table of Contents
What are the important topics on chemical equilibrium?
Ans: The most important topics in chemical equilibrium for JEE Advanced are Law of Chemical Equilibrium and Equilibrium Constants, Application of Equilibrium Constant, Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G), Equilibrium in Physical Processes, and Equilibrium in …
How is chemical equilibrium used in everyday life?
It is used as a refrigerant, for purification of water supplies, and in the manufacture of plastics, explosives, textiles, pesticides, dyes and other chemicals. Ammonia is produced by Haber’s process. It makes use of the Le Chatelier’s principle to increase the yield of ammonia. How?
What are the characteristics of chemical equilibrium?
The main characteristics of chemical equilibrium are as follows: At chemical equilibrium, the rate of forward and reverse reactions are equal. All the reactants and products are present at equilibrium. The position of equilibrium is not affected by a catalyst.
What are the three conditions of equilibrium in chemistry?
There are several factors that affect equilibrium conditions like temperature, pressure, and concentration of the system that affect equilibrium.
What are the types of equilibrium in chemistry?
- Homogeneous Equilibrium.
- Heterogeneous Equilibrium.
What is the meaning of chemical equilibrium in chemistry?
chemical equilibrium, condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs. A reversible chemical reaction is one in which the products, as soon as they are formed, react to produce the original reactants.
What are the factors that affect chemical equilibrium?
The temperature, pressure, and concentration of the system are all factors that affect equilibrium. When one of these factors changes, the equilibrium of the system is disrupted, and the system readjusts itself until it returns to equilibrium.
What is an example of chemical equilibrium?
Examples of chemical equilibrium If you take some hydrogen iodide in the closed vessel at the same temperature, a faction of hydrogen iodide is converted into hydrogen molecule and iodine molecule. Hence the rest of the hydrogen iodide remains unchanged.
What is chemical equilibrium application?
The main application of Chemical Equilibria in industrial process is to maximise the desired product concentration by minimising the leftover reactants.
What are the important characteristics of equilibrium constant?
Characteristics of Equilibrium Constant: It has a definite value for every chemical reaction at a particular temperature. It is independent of the initial concentrations of the reacting species. It changes with the change in the temperature. It depends on the nature of the reaction.
What are the 4 types of equilibrium?
- Stable Equilibrium.
- Unstable Equilibrium.
- Metastable Equilibrium.
What factor does equilibrium constant depend on?
Equilibrium constant depends on temperature and is independent of the actual quantities of reactants and products, the presence of a catalyst and the presence of inert material. It is also independent of concentrations, pressures and volumes of reactants and products.
What are the applications of Le Chatelier’s principle?
The le Chatelier’s principle can be applied to understand the effect of change in pressure on the systems at equilibrium as follows. 1) When the partial pressure of any of the gaseous reactants or of the products is increased, the position of equilibrium is shifted so as to decrease its partial pressure.
What is the unit of equilibrium constant?
Units of Equilibrium Constant Equilibrium constant being the ratio of the concentrations raise to the stoichiometric coefficients. Therefore, the unit of the equilibrium constant = [Mole L-1]△n. where, ∆n = sum of stoichiometric coefficients of products – sum of stoichiometric coefficients of reactants.
What are the 2 types of equilibrium?
Type of Equilibrium. Equilibrium is classified as dynamic equilibrium or static equilibrium.
What is equilibrium explain with example?
Equilibrium is defined as a state of balance or a stable situation where opposing forces cancel each other out and where no changes are occurring. An example of equilibrium is in economics when supply and demand are equal. An example of equilibrium is when you are calm and steady.
How do you calculate equilibrium in chemistry?
- [H2S] = 0.824 − 2x = 0.824 − 2(7.20 × 10−3) = 0.824 – 0.0144 = 0.810 atm.
- [H2] = 2x = 2(7.2 × 10−3) = 0.014 atm.
- [S2] = [x] = 0.0072 atm.
How does temperature affect the equilibrium?
if the temperature is increased, the position of equilibrium moves in the direction of the endothermic reaction. if the temperature is reduced, the position of equilibrium moves in the direction of the exothermic reaction.
How does pressure affect equilibrium?
When there is an increase in pressure, the equilibrium will shift towards the side of the reaction with fewer moles of gas. When there is a decrease in pressure, the equilibrium will shift towards the side of the reaction with more moles of gas.
What is the importance of Le Chatelier’s principle in industries?
Le Chatelier’s principle allows us to change the conditions of an equilibrium in order to shift its position. It is important in industry because it helps to increase yield and maximise profit.
What is Le Chatelier’s principle in chemistry?
Le Châtelier’s principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium.
What is K in equilibrium?
In a reaction at equilibrium, the equilibrium concentrations of all reactants and products can be measured. The equilibrium constant (K) is a mathematical relationship that shows how the concentrations of the products vary with the concentration of the reactants.
What is KC formula?
Formula for Kc: The formula for Kc is Kc=[C]c[D]d[A]a[B]b K c = [ C ] c [ D ] d [ A ] a [ B ] b , where [C] and [D] are the molar concentrations of the products at equilibrium, and [A] and [B] are the molar concentrations of the reactants at equilibrium.
What is Kp and KC in chemistry?
Kp And Kc are the equilibrium constant of an ideal gaseous mixture. Kp is equilibrium constant used when equilibrium concentrations are expressed in atmospheric pressure and Kc is equilibrium constant used when equilibrium concentrations are expressed in molarity.