THERMODYNAMICS

FACULTY- ER. GOSTA PANDA

SEMESTAR- 3^RD

SUBLECT- EME

THERMODYNAMICS

• Thermodynamics is a branch of physics that deals with heat, work, and temperature, and their relation to energy, radiation, and physical properties of matter.

MATTER

• In classical physics and general chemistry, matter is any substance that has mass and takes up space by having volume. Three states of matter are observable in everyday life: solid, liquid, gas.

THERMODYNAMIC PROPERTY

• Thermodynamic properties are defined as characteristic features of a system, capable of specifying the system's state.
• The thermodynamic properties are classified into two types such as intensive properties and extensive properties.
• Intensive properties do not depend on the quantity of matter. Examples include density, state of matter, and temperature. Extensive properties do depend on sample size. Examples include volume, mass, and size.

ENERGY

• Energy, in physics, the capacity for doing work. It may exist in potential, kinetic, thermal, electrical, chemical, nuclear, or other various forms. 
• The kinetic energy of an object is the energy that it possesses due to its motion.
• Potential energy is the energy by virtue of an object's position relative to other objects.
• Internal energy is the energy possessed by a system by virtue of its molecular arrangement or due to motion of the molecules.

HEAT

• Heat is the form of energy which flow from high temperature body to low temperature body without transfer of mass. Unit is joule.

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WORK

• In physics, work is the energy transferred to or from an object via the application of force along a displacement.

THERMODYNAMIC SYSTEM

• It is defined as a define area or a space where some thermodynamic process is taking place.
• A thermodynamic system has a fixed boundary and anything outside the boundary called surrounding.
• There are three types such as open system , closed system and isolated system.

• In open system the mass and energy of the working substance crosses the boundary of the system.  
• Closed system is a system of fixed mass whose identity is determined by the space of the matter.
• A closed system doesn’t permit the transfer of mass across its boundary but it permits the transfer of energy (heat and work).
• A system which is completely uninfluenced by the surrounding is called an isolated system.
• It is a system of fixed mass and no heat or work energy cross its boundary.  

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Specific heat

• It is defined as the amount of heat required to raise the temperature of a unit mass of any substance through one degree.
• It is denoted as “c”.
• Its unit taken as kJ/kg.
• Mathematically,

Heat required= m c (T₂ – T₁) kJ

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Sensible Heat

• When a substance is heated and temperature rises as the heat is added, then increase in heat is called sensible heat.
• It is denoted by h_f.
• Exp: - Heat absorbed in heating of water up to the boiling temp.

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Latent heat

• The heat which brings about a change of state with no change in temperature called latent heat.
• It is denoted by h_fg.

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ZEROTH LAW OF THERMODYNAMICS

• The zeroth law of thermodynamics states that if two thermodynamic systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.

FIRST LAW OF THERMODYNAMICS

• The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but can be neither created nor destroyed.
• For a thermodynamic process without transfer of matter, the first law is often formulated
• ΔU=Q-W

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