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class11 chapter 6 notes-Thermodyanamics

Chemistry Class 11 chapter 6notes-Thermodynamics note-

Chemistry Class 11 chapter 6notes-Thermodynamics note

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Chapter 6
Thermodynamics
Some Important Points and Terms of the Chapter Thermodynamics::

  1. System and the Surroundings: A system in thermodynamics refers to that
    part of universe in which observations are made and remaining universe
    constitutes the surroundings.
  2. The surroundings include everything other
    than the system. System and the surroundings together constitute the
    universe. The wall that separates the system from the surroundings is called
    boundary.
Chemistry Class 11 chapter 6notes-Thermodynamics note

Chemistry Class 11 chapter 6notes-Thermodynamics

  1. Types of the System😶:
  • Open System: In an open system, there is exchange of energy and
    matter between system and surroundings.
  • Closed System :In a closed system, there is no exchange of matter,
    but exchange of energy is possible between system and the
    surroundings.
  • Isolated system :In an isolated system, there is no exchange of
    energy or matter between the system and the surroundings
  1. State of a System: The state of a system means the condition of the system
    which is described in terms of certain observable properties such as
    temp(T), pressure(p), volume (v), etc. of the systems. These properties of a
    system are called state variables.

😎Chemistry Class 11 chapter 6notes-Thermodyanamis😎

  1. State Functions: A physical quantity of the system which depends on the state of the system but it does not depend upon
    the path by which this state has been attained.
  2. Path Function : A physical quantity of the system which depends on the path of the system and it is independent of the state of the system.
  1. Internal Energy: a quantity which represents the total energy of the
    system. It may be chemical, electrical and mechanical or any other type of
    energy you may think of, the sum of all these is the energy of the system. In
    thermodynamics, we call it the internal energy, U of the system.

Isothermal Process: When a process is carried out in such a manner that
the temp remains constant throughout this process, it is called an isothermal

6.Adiabatic Process: Process is carried out in such a manner that no heat can
flow from the system to the surrounding or vice versa.

  1. Isochoric Process: Process during which the volume of the system is kept
    constant.

Chemistry Class 11 chapter 6notes

  1. Isobaric Process: Process during which the pressure of the system is kept
    constant..
  1. The positive sign expresses that Work (Wad) is positive when work is done
    on the system. Similarly, if the work is done by the system, wad will be
    negative.
  1. The q is positive, when heat is transferred from the surroundings to the
    system and q is negative when heat is transferred from system to the
    surroundings.
  2. First law of Thermodynamics: Statement: Energy can neither be created
    nor destroyed, however it may be converted from one form to another.

Chemistry Class 11 chapter 6notes-pdf

The total energy of the universe remains constant although it may undergo
transformation from one to another.
Mathematical expression U = q + w

  1. A process or change is said to be reversible, if a change is brought out in
    such a way that the process could, at any moment, be reversed by an
    infinitesimal change. A reversible process proceeds infinitely slowly by a
    series of equilibrium states such that system and the surroundings are
    always in near equilibrium with each other. Processes other than reversible
    processes are known as irreversible processes.

Chemistry Class 11 chapter 6notes-handwritten

  1. Extensive property: An extensive property is a property whose value
    depends on the quantity or size of matter present in the system. For
    example, mass, volume, internal energy, enthalpy, heat capacity, etc. are
    extensive properties.
  2. Intensive property: Those properties which do not depend on the quantity
    or size of matter present are known as intensive properties. For example
    temperature, density, pressure etc. are intensive properties.

  1. Specific heat capacity is the quantity of heat required to raise the
    temperature of one unit mass of a substance by one degree celsius (or one
    kelvin). For finding out the heat, q, required to raise the temperatures of a
    sample, we multiply the specific heat of the substance, c, by the mass m,
    and temperatures change, AT as

  1. Relationship between Cp and Cv for an ideal gas: Cp-Cv=R

  1. Bomb calorimeter: For chemical reactions, heat absorbed at constant
    volume, is measured in a bomb calorimeter. Here, a steel vessel (the bomb)