What Is Enthalpy?
Enthalpy is defined as the sum of the 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 enthalpy are calorie, BTU, or joules. It is not possible to measure the total enthalpy of the system directly due to which, change in enthalpy is generally measured during experiments.
Table of Contents
- Enthalpy Equation
- What is the Enthalpy change?
- Some important terms related to enthalpy:
- What is Entropy?
- Recommended Videos
- Properties of Entropy
- The relationship between enthalpy and entropy:
E= U + PV where,
E is the enthalpy
U is the internal energy of a system
P is the pressure
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 is evolved or absorbed during a reaction. It is denoted as ΔH. It is expressed as follows:
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 ΔHreaction
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 the 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. For endothermic reactions, enthalpy of solution is positive and for exothermic reactions, it is negative. 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,
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, entropy also increases.
- As mass increases entropy increases.
The relationship between enthalpy and entropy:
The relationship between enthalpy and entropy can be seen during the calculation of the Gibbs free energy. Josiah Willard Gibb’s developed Gibbs energy in the 1870s. He termed it as the 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
G = U + PV – TS
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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