Class 12 Thermodynamics Full Note

               Class 12 Thermodynamics Full Note

                                    Physics

Thermodynamics Course content
4.1 Define thermodynamics.
4.2 Explain the energy change in chemical reactions.
4.3 Define the terms internal energy and state function.
4.4 State and explain the first law of thermodynamics.
4.5 State and explain enthalpy and enthalpy changes in various processes (enthalpy of solution, enthalpy of formation enthalpy of combustion, and enthalpy of reaction).
4.6 Explain endothermic and exothermic processes with the help of an energy profile diagram.
4.7 State laws of thermo-chemistry and solve numerical problems related to Hess law.
4.8 Define the term entropy and spontaneity.
4.9 State and explain the second law of thermodynamics.
4.10 Define standard Gibbs free energy change of reaction by means of the equation ΔG=ΔH-TΔS.
4.11 Calculate ΔG for a reaction using the equation ΔG=ΔH-TΔS.
4.12 State whether a reaction of a process will be spontaneous by using the sign of ΔG.
4.13 Explain the relationship between ΔG and equilibrium constant. Unit 4: Thermodynamics class 12 chemistry notes Nepal Note of thermodynamics chapter of class 12 Note is Presented below: Introduction of Thermodynamics Thermodynamics is the branch of science that deals with the study of energy and its transformations. It is a fundamental subject in chemistry that explains the behavior of matter and energy in chemical processes. Thermodynamics is based on a set of principles and laws that describe the relationship between energy, heat, and work. The principles of thermodynamics are based on the concepts of energy and entropy, which are the two fundamental properties of a system. Energy is defined as the ability to do work, while entropy is a measure of the disorder or randomness of a system. The laws of thermodynamics are as follows: The First Law of Thermodynamics: This law states that energy cannot be created or destroyed, but it can be converted from one form to another. In other words, the total energy of a system and its surroundings is always conserved. The Second Law of Thermodynamics: This law states that the entropy of an isolated system can never decrease over time. In other words, the natural tendency of a system is to move towards a state of maximum entropy or disorder. The Third Law of Thermodynamics: This law states that it is impossible to reach absolute zero temperature. This is because as a system approaches absolute zero, the entropy of the system approaches a minimum value. Thermodynamics is used in many areas of chemistry, including chemical reactions, phase transitions, and heat transfer. It is an essential tool for understanding the behavior of matter and energy in the natural world.

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phase in thermodynamics

1.Homogenous system

2.heterogenous system

1.Homogeneous System: A homogeneous system is one in which all parts of the system are in the same phase. The properties of the system are uniform throughout, and there are no visible boundaries between different portions of the system. Examples of homogeneous systems include:

A container of pure water: All the water in the container is in the liquid phase, and the properties of the water are uniform throughout the container.

A sealed container of air: All the air in the container is in the gas phase, and the properties of the air are uniform throughout the container.

2.Heterogeneous System: A heterogeneous system is one in which the system is composed of two or more phases. The properties of the system are not uniform throughout, and there are visible boundaries between the different phases of the system. Examples of heterogeneous systems include:

A mixture of oil and water: The oil and water are in different phases, and there is a visible boundary between the two liquids.

Ice and water in a glass: The ice is in the solid phase, and the water is in the liquid phase. There is a visible boundary between the ice and water phases.

Understanding the phases and phase transitions in both homogeneous and heterogeneous systems is important in many areas of science and engineering, as it helps us understand the behavior of different materials and substances under different conditions.

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