Chemistry

# First Law of Thermodynamics Examples Formula and Derivation

## Statement of First Law of Thermodynamics

The first law of thermodynamics is also known as the ‘Law of Conservation of Energy.

“ Energy can neither be created nor destroyed, but only be changed from one form to another form”.

Or

“ The total energy of a system and its surroundings remain constant”.

## Mathematical Form and derivation

Consider a system whose initial system is ‘E1’ let a  quantity of heat ‘q’ absorbed by the system from the surroundings and does some work ‘W’ on the surroundings while the internal energy change to

‘E2’.

Then, a change in internal energy is given by

ΔE = E1 – E2

According to the first law of Thermodynamics

ΔE = q – W

The value of ΔE is negative when the system loses energy and positive when the system gains energy. ### Pressure-Volume Work

Consider a gas enclosed in a cylinder, fitted with a frictionless and weightless piston. Let the area of the piston is ‘A’ external pressure acting on the piston ‘P’, the force exerted by the gas on the piston ‘F’.

Now, if the system expands, and the piston moves against the surroundings traveling a distance ‘ΔI’. Then,

Work  = Force x Displacement

W = F x ΔI  ———– 1

Since,

P  = F/A

Therefore,

F = P x A ———— 2

Put the value of ‘f’ into equation # 1, and we get

W = P x A x ΔI  ———— 3

Since,

A x ΔL  = ΔV

So, in equation # 3 we can write as

W = P x ΔV

Or

W = P ΔV

According to the first law of thermodynamics

ΔE =  q – w  ———– 4

Put the value of ‘W’ in equation # 4 we get

ΔE = q – P ΔV

Or

q = ΔE + p Δ V

## Application of First Law of Thermodynamics

1. ### Process At Constant Volume

According to the first law of thermodynamics

ΔE  =   q – P Δ V

ΔE   =   q v – P Δ V ————– 1

Where, qv = heat absorbed at constant volume when the volume of the system does not change

Δ V   = 0

Under this condition, no work is done

P Δ V = p x 0 = 0

Hence, equation # 1 becomes

Δ E = q v ————- 2

This equation shows that at constant volume, the heat evolved is equal to the change in the internal energy, and no work is done.

1. ### Process At Constant Pressure

When heat is given to the system at constant pressure the internal energy of the system increases, as a result of which the system performs work on the surroundings:

Thus,

QP = ΔE + PΔV ———- 1

where QP is the heat absorbed at the constant pressure

we know that

ΔE  =  E1  – E2

ΔV  = V1  – V2

Then equation # 1 can be written as:

=     (E2 – E1)   +  P(V2 – V1)

QP =     (E2 + PV2)   –   (E1 + PV1) ———- 2

the enthalpy ‘H’ is mathematically defined as:

H =  E + PV

At initial state

H1  =  E1 + PV1

At final state

H2  = E2 + PV2

Substituting the value in equation # 2 we get

QP = H2 – H1 = Δ H

QP  = ΔH  ———– 3

Equation #1 can be written as:

ΔH = Δe + PΔV ———- 4

Equation #3 shows that heat absorbed or evolved from a system at constant pressure is equal to the change in enthalpy of the system.

Thus, a change in enthalpy is the heat absorbed or evolved by a system at constant pressure.