Class 11 Chemistry - KARNATAKA
Thermodynamics
The chapter 'Thermodynamics' in Class 11 Chemistry explores the flow of energy in chemical and physical processes. You will study key terms like system, surroundings, work, heat, internal energy, and enthalpy. It introduces the First Law of Thermodynamics (conservation of energy), Hess's Law, and criteria for spontaneity using Entropy and Gibbs Free Energy. This is a high-scoring and crucial chapter for the Karnataka (KSEEB) board exams as well as competitive exams like NEET and JEE, often featuring numerical problems and conceptual derivations.
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System and Surroundings
The specific part of the universe under thermodynamic study is the system, while the rest of the universe constitutes the surroundings.
First Law of Thermodynamics
Energy can neither be created nor destroyed, though it can be transformed from one form to another, expressed mathematically as delta U = q + w.
Enthalpy (H)
The total heat content of a system at constant pressure, where the change in enthalpy (delta H) equals heat absorbed or evolved.
Entropy (S)
A measure of the degree of randomness or disorder of a system, which increases in spontaneous processes in an isolated system.
Gibbs Free Energy (G)
A thermodynamic property defined as G = H - TS, used to predict the spontaneity of a process at constant temperature and pressure.
Important Formulas
Board Exam Info
In the Karnataka (KSEEB) Class 11 Chemistry annual examination, Thermodynamics typically carries around 6 to 8 marks. Questions usually include a mix of 1-mark definitions, 2-mark conceptual reasons (like spontaneity or entropy), and 3 to 5-mark numerical problems based on Hess's Law, enthalpy of reaction, or Gibbs Free Energy calculations.
Frequently Asked Questions
What is the difference between an intensive and extensive property?
Extensive properties (like mass, volume, enthalpy) depend on the amount of matter present, whereas intensive properties (like temperature, pressure, density) do not depend on the quantity of matter.
Why is delta G negative for a spontaneous reaction?
A negative value of Gibbs Free Energy (delta G < 0) indicates that the process results in a net decrease in free energy, making it thermodynamically favorable and spontaneous under constant temperature and pressure.
How is state function different from path function?
State functions (like internal energy, pressure, temperature) depend only on the initial and final states of the system, not on the path taken. Path functions (like heat and work) depend entirely on the path followed.
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