Equilibrium Class 11 Notes Chemistry Pdf Download

[Vespasiano Jilg]

Lookingfor revision notes that are specific to the exam board you are studying? If so, click the links below to view our condensed, easy-to-understand revision notes for each exam board, practice exam question booklets, mindmap visual aids, interactive quizzes, PowerPoint presentations and a library of past papers directly from the exam boards.

A chemical reaction is a process in which one or more substances, the reactants, are converted to one or more different substances, the products. Substances are either chemical elements or compounds. A chemical reaction is complete if the reactants are completely transformed in products at the end of the process. A single arrow is usually used for writing an irreversible reaction.

There are many reactions which are incomplete under given conditions: the products that are formed react with each other to restore the starting reactant. These are called reversible reactions. A double arrow is usually used for writing a reversible reaction, indicating that the reaction happens in the same time in both directions. Reactant A with reactant B creates product C and product D. In the same time C and D generate again A and B.

The reaction rate depends on the concentration of the reactants. At the beginning the quantity of reactant is the highest, thus the rate of product formation is the highest. As the reactant amount decreases, also the rate of reactant transformation decreases and the rate of product formation increases. After a certain time, the concentrations of reactants and products become constant and this state is called equilibrium.

It is important to notice that the reactions never stop in equilibrium phase but both direct and inverse reactions are happening at the same time and at the same rate. As a result, the concentrations of the substances do not change.

If we add some colorless N2O4 to an evacuated glass container at room temperature, over time, we observe the gas changing to a yellowish orange color and gradually getting darker until the color remain constant.

If at the equilibrium all the chemical species are in the same phase, we call it homogeneous equilibrium. For solutions, they are all dissolved, and for gaseous equilibria, they are all gases. However, we can also talk about equilibria in which not all of the species are in the same phase. These equilibria are referred to as heterogeneous equilibria. An example of a heterogeneous equilibrium would be when an ionic compound partially dissolves in water or the decomposition of calcium carbonate, CaCO3.

Any time we put something in the square brackets, this means that we need its concentration. Because CaCO3 is a solid in this process, it doesn't really have a clearly defined concentration. As a result, we just leave it out of this expression. Likewise, whenever you have a pure solid or a pure liquid (but not a solution) in an equilibrium expression, you leave it out of the expression for Kc.

This equilibrium is only established if the calcium carbonate is heated in a closed system, preventing the carbon dioxide from escaping. It is important to remember that solids and pure liquids are not included in the expression of the equilibrium constants so in this case, the only thing in this equilibrium which isn't a solid is the carbon dioxide. That is all that is left in the equilibrium constant expression.

The equilibrium state depends on temperature, pressure, or concentrations. This means that the change of one or more than one of these parameters stimulates a response that partially offsets the change while a new equilibrium condition is established. This is the Le Chtelier's principle. In 1884 the French chemist and engineer Henry-Louis Le Chtelier proposed one of the central concepts of chemical equilibria, which describes what happens to a system when something briefly removes it from a state of equilibrium.

Chemical equilibrium in which all the reactants and products involved in a chemical reaction are not in the same physical state rather exists in different physical states. A reactant may be in solid form while the product is in aqueous solution form.

Atoms and molecules, states of matter, chemistry of the elements. Prerequisite: Chemistry 30, or equivalent. Note: Restricted to Engineering students only. Other students who take this course will receive *3.0.

Atoms and molecules, states of matter, chemistry of the elements. Prerequisite: Chemistry 30, or equivalent. Note: Restricted to Engineering students only. Other students who take this course will receive 3 units.

Rates of reactions, thermodynamics and equilibrium, electrochemistry, modern applications of chemistry. Prerequisite: CHEM 103. Note: Restricted to Engineering students only. Other students who take this course will receive *3.0.

Rates of reactions, thermodynamics and equilibrium, electrochemistry, modern applications of chemistry. Prerequisite: CHEM 103 or 101. Note: Restricted to Engineering students only. Other students who take this course will receive 3 units.

Principles, methods, and experimental applications emphasizing solution phase equilibria, titrimetry, volumetric laboratory skills, evaluation of experimental data, and applications of electrochemistry to analytical measurements. Includes examples of organic and inorganic analyses. Prerequisite: CHEM 102.

A continuation of CHEM 211 emphasizing the principles, methods, and experimental applications of separation techniques, atomic and molecular optical spectrometry, mass spectrometry, and evaluation of experimental data. Includes examples of organic and inorganic analyses and use of the analytical literature. Prerequisite: CHEM 211. Students who have previously taken CHEM 313 may not take CHEM 213 for credit.

The chemistry of main-group elements including a survey of the structure, bonding, and reactivity of their compounds. Transition-metal chemistry will be introduced. The course will include applications in industrial, biochemical, environmental, and materials science. Prerequisites: CHEM 102 or 105 and CHEM 261.

The correlation of structure and chemical bonding in carbon compounds with the physical properties and chemical reactivity of organic molecules. Discussion will be based on functional groups with emphasis on hydrocarbons and derivatives that contain halogens, oxygen, sulfur, and the hydroxy group. Introduction to stereochemistry, three dimensional structure, reaction mechanisms, especially addition to double bonds, nucleophilic substitution and elimination reactions. Prerequisite CHEM 101 or 103. Note: Students who have obtained credit for CHEM 264 cannot take CHEM 261 for credit. Engineering students who take this course will receive *4.5.

The correlation of structure and chemical bonding in carbon compounds with the physical properties and chemical reactivity of organic molecules. Discussion will be based on functional groups with emphasis on hydrocarbons and derivatives that contain halogens, oxygen, sulfur, and the hydroxy group. Introduction to stereochemistry, three dimensional structure, reaction mechanisms, especially addition to double bonds, nucleophilic substitution and elimination reactions. Prerequisite CHEM 101 or 103. Note: Students who have obtained credit for CHEM 264 cannot take CHEM 261 for credit. Engineering students who take this course will receive 4.5 units.

Continuation of the structural and chemical properties of the basic functional groups of organic compounds including alkynes, aromatic compounds, aldehydes, ketones, carboxylic acids and their derivatives and amines. Illustration of these functional groups in natural products such as carbohydrates, amino acids and proteins, nucleic acids and lipids. Discussion of the application of spectroscopic methods for the structure determination in simple organic molecules. Prerequisites: CHEM 261 or CHEM 264 and 266 or SCI 100. Students who have obtained credit for CHEM 265 cannot take CHEM 263 for credit.

A remote delivery offering that emphasizes the correlation of structure and chemical bonding in carbon compounds with the physical properties and chemical reactivity of organic molecules. Discussion will be based on functional groups with emphasis on hydrocarbons and derivatives that contain halogens, oxygen, sulfur, and the hydroxy group. Introduction to stereochemistry, three-dimensional structure, reaction mechanisms, especially addition to double bonds, nucleophilic substitution and elimination reactions. Seminars will emphasize virtual laboratory techniques and online workshops for IR spectroscopy and stereochemistry. Prerequisite CHEM 101 or 103. Note: Students who have obtained credit for CHEM 261 cannot take CHEM 264 for credit.

A remote delivery offering that is a continuation of the structural and chemical properties of the basic functional groups of organic compounds including alkynes, aromatic compounds, aldehydes, ketones, carboxylic acids and their derivatives and amines. Illustration of these functional groups in natural products such as carbohydrates, amino acids and proteins, nucleic acids and lipids. Discussion of the application of spectroscopic methods for the structure determination in simple organic molecules. Seminars will emphasize the virtual application of laboratory techniques in standard organic reactions, as well as online workshops for NMR and structure determination. Prerequisites: CHEM 261 or 264. Note: Students who have obtained credit for CHEM 263 cannot take CHEM 265 for credit.

3a8082e126