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First law of thermodynamics equation and applications

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First law of thermodynamics definition

When heat is added to a system there is an increase in the internal energy due to the rise in temperature,an increase in pressure or change in the state.If at the same time,a substance is allowed to do work on its environment by expansion,the heat Q required will be the heat necessary to change the internal energy of the substance from Uin the first state to Uin the second state plus the work W done on the environment.

First law of thermodynamics equation

Q = (U2 –U1) + W

Or

Q = ΔU + W

Thus the change in internal energy ΔU =U2 -U1 is defined as Q -W.Since it is the same for all processes concerning the state,the first law of thermodynamics,thus can be stated as:

“In any thermodynamic process,when heat Q is added to a system,this energy appears as an increase in the internal energy ΔU stored in the system plus the work W done by the system on its surroundings.”

A bicycle pump provides a good example.When we pump on the handle rapidly,it becomes hot due to mechanical work done on the gas,rising thereby its internal energy.

Human metabolism also provides an example of energy conservation.Human beings and other animals do work.When they walk,run,or move heavy objects,work requires energy.Energy is also needed for growth to make new cells and to replace old cells that have died.Energy transforming processes that occur within an organism or named as metabolism.We can apply the first law of thermodynamics:

ΔU =Q – W

to an organism of the human body.Work (W) done will result in the decrease in internal energy of the body.Consequently the body temperature or in other words internal energy is maintained by the food we eat.

What is an example of first law of thermodynamics ?

A bicycle pump provides a good example. when we pump on the handle rapidly, it becomes hot due to mechanical work done on the gas, raising their by its internal energy. one such simple arrangement is shown in figure.

It consist of a bicycle pump with a blocked outlet allows the air temperature to be monitored. when piston is rapidly pushed, thermometer shows a temperature rise due to increase of internal energy of the air. the push force does work on the air, thereby, increasing its internal energy, which is shown, by the increase in temperature in the air.

First law of thermodynamics and law of conservation of energy

Human metabolism also provides an example of energy conservation. human beings and other animals do work when they walk, run, or move heavy objects. work requires energy. energy is also needed for growth to make new cells and to replace old cells that have died. energy transforming processes that occur with in an organisms are named as metabolism. we can apply the first law of thermodynamics as :

 ΔU = Q-W

to an organism of the human body. work W done will result in the decrease in internal energy of the body. consequently the body temperature or in other words internal energy is maintained by the food we eat.

Change in internal energy

“A function of thermodynamics coordinates whose final value minus initial value is equal to the value of Q +W in the process is called change in internal energy.”

The change in internal energy between equilibrium states i and f is given by:

ΔEint =Eint,f – Eint,i

ΔEint=Q +W

The value of internal energy Eint,i depends only on the coordinate of the state ‘i’.Similarly,Eint,f  depends only on the state of the system and not at all on the path followed.

Sign convention

  • When heat is supplied to the system,it increases the internal energy,so Q is taken as positive(Q > 0)
  • Work done on the system also increases the internal energy ,so it is also taken as positive.(W > 0),In this case first law of thermodynamics is written as:

ΔEint=Q +W

  • When heat is rejected by the system,it decreases the internal energy,so it is taken as negative.(Q <0)
  • Work done by the system decreases the internal energy ,so it is taken as negative (W <0)

In this case first law of thermodynamics is written as:

ΔEint=Q – W

Limitations of first law of thermodynamics

The first law of thermodynamics is a general result that is thought to apply to every process in nature which proceeds between equilibrium states.It tells us that energy must be conserved in every process but it does not tell us whether any process that conserves energy can actually occur.

Applications of first law of thermodynamics

  • Adiabatic process

“A process in which no heat can enter or leave the system is called adiabatic process.”In an adiabatic process ,there is no transfer of heat across the boundary of the system,so Q=0.According to first law of thermodynamics:

ΔEint=Q +W

Since

Q = 0    ,SO

ΔEint = W

The work done on the system increases the internal energy.

  • Isothermal process

“A process in which temperature of the system remains constant is called Isothermal process.”

Since temperature remains constant in isothermal process so the internal energy of the gas must also remain constant so:

ΔEint=Q +W

0 = Q + W

⇒ Q =-W

Constant volume process

“The process in which volume of the system remains constant is known as volume process.”

If volume of a gas remains constant,the work done will be zero,thus W=0

So,according to first law of thermodynamics:

ΔEint =Q +W

Since W=0,SO

⇒ Q = ΔEint

In this case all the heat that enters the gas is stored in it as internal energy.

Cyclic process

“It is a series of processes after which system returns to its initial state.”It is a three step process.It is a cyclic process,because it starts and ends at the same point.

Free expansion

“A process in which a gas goes from one side of the container to the other half initially evacuated is called free expansion.”

Watch video about first law of thermodynamics:

 

Zeroth law of thermodynamic equation:

“According to this law,when two bodies have equality of temperature with third body,then in turn they have equality of temperature with each other.”

Watch video about zeroth law:

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