Enthalpy And Entropy

What Is Enthalpy?

Enthalpy is defined as the sum of internal energy of a system and the product of its pressure and volume. It is denoted by the symbol E. It is a state function. Units used to express are calorie, BTU, or joules. Below we have given the equation.

Enthalpy Equation:

E= U + PV where,

E is the enthalpy

U is the internal energy of a system

P is the pressure

V is the volume

What is the Enthalpy change?

An enthalpy change is defined as the difference between the energy gained by the formation of new chemical bonds and the energy used to break bonds in a chemical reaction at constant pressure. In simple terms, it tells about the amount of heat evolved or absorbed during a reaction. It is denoted as ΔH. It is expressed as follows:

ΔH = ΔU +PΔV

Some important terms related to enthalpy:

Enthalpy of reaction – It is defined as the difference between the total enthalpy of the reactants and the total enthalpy of the products in a reaction. It is denoted as ΔHRXN

Enthalpy of formation – Enthalpy of formation is the amount of energy required to produce a compound from its composition of elements. It is denoted as ΔHf

Enthalpy of combustion – It is the change in enthalpy accomplished when one mole of an element is heated in the presence of excess oxygen under standard conditions. It is denoted as ΔHc.

Enthalpy of solution – It is defined as the total amount of heat released or absorbed when two substances are put in a solution. It can be either negative or positive. If is positive it will result in an endothermic reaction. If it is negative it will result in an exothermic reaction. It is denoted as ΔHsolution.

What Is Entropy?

Entropy is defined as the measure of the thermal energy of a system per unit temperature which is not available for doing useful work. It is denoted as S. The SI unit for Entropy is Joules per Kelvin. Entropy change at constant temperature is calculated as given below:

ΔSsystem = qrev / T

ΔS represents the change in entropy,

qrev represents the reverse of the heat, and

T is the temperature in the Kelvin scale.

Properties of entropy:

  • Entropy is greater in malleable solids whereas it is lower in brittle and hard substances.
  • When gas is dissolved in water the entropy decreases whereas it increases when liquid or solid is dissolved in water.
  • With an increase in chemical complexity, the entropy also increases.
  • As mass increases entropy increases.

The relationship between enthalpy and entropy:

The relationship between enthalpy and entropy can be seen to calculate the Gibbs free energy. Josiah Willard Gibbs developed Gibbs energy in the 1870s. He termed it as available energy of a system that can be used to do work. It is defined as the sum of the enthalpy of a system and the product of the entropy and temperature of the system. It is denoted as G.

G = H + TS

Or

G = U + PV – TS

Where,

U is the internal energy in joules

P is the pressure in Pascal

V is the volume in m3

T is the temperature in Kelvin

S is the entropy in joules/Kelvin

H is the enthalpy in joules

The change in Gibbs energy is given as ΔG = ΔH – TΔS

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