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Thermodynamics-1 One Shot Lecture for 11th Class with Ashu sir | Science and Fun 11th 12th

Science and Fun Motivation・77 minutes read

Understanding thermodynamics is crucial for various applications like maintaining the temperature of tea in a thermos flask, with key concepts including isolated systems and energy exchange. The text delves into the different types of systems, such as open, closed, and isolated, and processes like adiabatic and isothermal, emphasizing their importance in studying energy changes and properties.

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Thermodynamics involves studying energy changes in systems like isothermal, isochoric, isobaric, and adiabatic processes, crucial for understanding energy transfer and maintaining system properties.
Internal energy, dependent on factors like substance nature, temperature, and pressure, changes due to heat and work transfer, with formulas and conventions governing these alterations, essential for comprehending system energy dynamics and transformations.

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What is thermodynamics?
The study of energy and its transformations.

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Summary

00:00

"Thermodynamics: Basics, Systems, Practical Applications"

The text discusses the scenario of being in a snowy area without clothes and the choice between sitting on a wooden or iron bench.
It introduces the topic of thermodynamics and how it relates to traveling on gas, boiling water, and cooling food in the fridge.
The text mentions the study of thermodynamics in chemistry and physics, emphasizing its importance and relevance.
It outlines the plan for lectures on thermodynamics, focusing on basics, principles, formulations, and numerical problems.
The text explains the concept of a thermodynamic system, distinguishing between the system and its surroundings.
It details the types of systems - open, closed, and isolated - and provides examples to illustrate their characteristics.
The text delves into the open system, where both energy and mass can be exchanged, contrasting it with the closed system that only allows energy transfer.
It further explains the isolated system, where neither mass nor energy can be lost, using the example of a thermos flask to illustrate the concept.
The text emphasizes the practical application of isolated systems in maintaining the temperature of tea in a thermos flask over time.
It concludes by highlighting the importance of understanding thermodynamics and its practical implications in various scenarios.

14:37

Thermodynamic Processes and System Properties Explained

Isolated systems prevent energy exchange with the surroundings, like a thermos flask keeping hot coffee isolated.
Properties in chemistry are classified as macroscopic, including extension and intensive properties.
Volume is an extension property dependent on substance quantity, while intensive properties like temperature and pressure are substance-independent.
Isothermal processes maintain constant temperature despite energy changes, as seen in state changes like ice melting.
Isochoric processes, or isovolumetric, keep volume constant regardless of temperature changes.
In an isobaric process, pressure remains constant while other factors may change.
Adiabatic processes involve no heat exchange between the system and surroundings, like a thermos flask maintaining temperature.
Thermodynamics introduces processes like adiabatic, isothermal, isochoric, and isobaric to study energy changes.
Understanding these processes aids in studying thermodynamic systems and their properties.
Theoretical concepts like isolated systems and energy exchange are crucial in comprehending thermodynamic processes.

31:33

Understanding Pressure, Energy, and Processes in Thermodynamics

Bar represents pressure, and isobar signifies a constant pressure process.
To maintain constant pressure, hitting a gas in an unclosed container is necessary.
Keeping pressure constant in an open container involves heating a gas.
Reversible processes allow for the reversal of steps, like converting water back to ice.
Irreversible processes, like chemical reactions, cannot be easily reversed.
Cyclic processes differ from reversible processes in that they do not always return to the starting point.
Internal energy, denoted as delta U, represents the change in energy within a system.
Internal energy depends on factors like the chemical nature of substances, temperature, and pressure.
Calculating internal energy is impossible, but changes in internal energy can be determined.
Observing changes in internal energy, like through energy input or output, allows for understanding the system's energy alterations.

49:07

Energy Transfer: Heat, Work, and Internal Energy

Energy transfer occurs in two ways: through heat and work forms.
Heat is a form of energy that travels due to temperature differences between two bodies.
Hit is defined as energy that flows due to temperature disparities, leading to energy transfer.
Internal energy can increase or decrease based on heat transfer between the system and surroundings.
Work can also change internal energy, either by the system working or work being done on the system.
The change in internal energy can be attributed to either work or heat transfer.
Work done by the system decreases internal energy, while work done on the system increases it.
Heat evolving or being supplied affects the internal energy change, with specific formulas and sign conventions to consider.
Understanding volume work, such as compressing gas in a container, can demonstrate the conversion of energy forms.
Further discussions on free energy, heat capacity, and specific heat will be covered in subsequent lectures.

01:10:25

"Formula 4: Calculating Work in Thermodynamics"

Formula 4 is a small workhorse used for displacement calculations.
Work is based on pressure and volume, especially in thermodynamics and chemistry.
Converting work into pressure and volume form simplifies numerical solutions.
The formula aids in calculating work done, particularly in gas-related scenarios.
The process focuses on pressure and volume changes, without specifying a particular process.
External pressure application results in volume changes, always leading to decreased final volume.
The formula for isothermal work done involves the ideal gas equation PV = NRT.
Isothermal processes maintain constant temperature, aiding in work done calculations.
The formula for isothermal work done can be expressed in terms of pressure changes.
The connection to Boyle's Law and Charles's Law further enhances understanding of isothermal work calculations.

01:29:11

Understanding Enthalpy and Standard Conditions

Enthalpy refers to the energy of a substance, specifically the energy emitted or absorbed by one mole of the substance.
Enthalpy is essentially the energy of one mole of a substance, with its unit being calories or joules.
Standard conditions are crucial for enthalpy calculations, ensuring comparability between reactions.
Enthalpy changes during phase transformations involve the energy required or released when a substance changes state.
Standard enthalpy of formation is vital, requiring the use of standard elements and reactants to determine the enthalpy of a substance's formation.
Balancing reactions for standard enthalpy of formation involves using basic elements and ensuring only one value is considered.
The Hess Law states that the net enthalpy change in a process depends solely on the initial and final states of the reaction, regardless of the path taken.

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