THERMODYNAMICS

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is the study of heat and its transformation into work.

Thermodynamics

first observed the relationship between heat energy and work.

Count Rumford

was credited for proving that a given amount of MECHANICAL energy produced the SAME AMOUNT of HEAT.

James Prescott Joule

A series of experiments led him to the measurement of the number of JOULES which is EQUIVALENT to ONE CALORIE of HEAT. This quantity of work is called the

mechanical equivalent of heat.

THERMODYNAMIC PROCESS or a change of state can be described as any CHANGE in the values of the following quantities: (4)

PVTQ PRESSURE, VOLUME, TEMPERATURE and QUANTITY of a SUBSTANCE.

describe the features of a system that are ALWAYS THE SAME whenever that system is in a given state.

State variables

A — is a particular situation wherein a system has SPECIFIED VALUES of (PVTQ) - pressure, volume, temperature and quantity of a substance.

state

If the process can be reversed, it is called a —.

reversible process

A — is a succession of CHANGES that ends with the RETURN of the system TO its INITIAL state.

cycle

The first thermodynamic process is the CONSTANT VOLUME process known as —.

isovolumetric or isochoric process

In general under a —-, NO WORK is produced. The HEAT absorbed is used to INCREASE the INTERNAL ENERGY

constant volume process

The second thermodynamic process is the CONSTANT TEMPERATURE process called —.

isothermal process

A system undergoing an isothermal process ABSORBS HEAT, but the — remains constant.

temperature

In isothermal process, the heat received by any system is converted to —.

work

The third thermodynamic process is when HEAT CONTENT of the system or CERTAIN QUANTITY of MATTER remains CONSTANT. This process is called —-

adiabatic process.

An — involves NO TRANSFER OF HEAR between the system and its surroundings.

adiabatic process

The wall of a system, which DOES NOT ALLOW the FLOW OF HEAT through it, is called —; while the wall which ALLOW THE FLOW OF HEAT is called as —.

adiabatic wall, diathermic wall

Adiabatic process happens when there is a RAPID DECREASE in — that the system has LIMITED TIME to ABSORB HEAT from the surroundings.

pressure

The — in an adiabatic process will cause the TEMPERATURE of the system to DECREASE.

work done

ADIABATIC The DECREASE in the INTERNAL ENERGY is equal to the energy — in order to perform work.

needed

The last thermodynamic process is the CONSTANT PRESSURE process known as the —

isobaric process.

During the process the TEMPERATURE of the system INCREASE, thus the INTERNAL ENERGY of the system also INCREASES.

Isobaric process

ISOBARIC The HEAT ABSORBED is EQUIVALENT to the — and some to increase the internal energy of the system.

work done

In its natural condition, — always FLOWS from objects of HIGHER temperature going TO objects of LOWER temperature.

heat

During this process, the object with higher temperature loses heat, while the object with lower temperature gains heat. The amount of heat lost is always equal to the amount of —

heat gained.

The amount of heat lost is always equal to the amount of heat gained. If this energy conservation is applied to thermal system or systems involving changes in temperature, then it is called the —.

first law of thermodynamics

This can be stated as: The HEAT ADDED to a system equals to an INCREASE in the INTERNAL ENERGY of a system plus the WORK done by the system.

first law of thermodynamics

FIRST LAW OF THERMODYNAMICS From this law, when heat is added to a system, the system does one (or both) of the following things: (1) the heat may be used to increase the — of the system and (2) the heat may be used to perform —

internal energy , external work.

The mathematical form of the first law

ΔQ = ΔU + W

first law is the HEAT TRANSFERRED to or from the system is the CHANGE in the INTERNAL ENERGY and is the EXTERNAL WORK done by the system.

Q U W

is the amount of work required to produce a unit quantity of heat.

Mechanical equivalent of heat

The symbol used for mechanical equivalent . •of heat is —, in honor of James Prescott Joule.

•The symbol used for mechanical equivalent . •of heat is J, in honor of James Prescott Joule. Its constant value was to be: J = J =

J = 4.18 joules/calorie J = 4.18 x 107 ergs/calorie

• – no heat is added or removed from the system. U = -W work done on the system increases the internal energy of the system

Adiabatic

• – the temperature of the system remains the same. ΔQ = W Internal energy remains constant.

Isothermal

•– the volume of the system does not change. There is no work produced. ΔQ = ΔW heat added to the system is used to increase the internal energy

Isometric/Isovolumetric/Isochoric

• – the pressure in the system does not change ΔQ = ΔU + PΔV heat added to the system is used to increase the internal energy and do work

Isobaric

A — is any device that converts heat into mechanical work.

heat engine

The — is the ideal heat engine that represents an engine with the HIGHEST POSSIBLE EFFICIENCY.

Carnot engine

In — proposed an ideal heat engine that is free from friction and heat losses. It is a heat engine that uses only isothermal and adiabatic processes. It consists of a cylinder filled with an ideal gas and has a movable piston at one end.

1840 Sadi Carnot

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