Enthalpy

It is the thermal energy involved in different types of chemical reactions, in which simple substances have, by convention, enthalpy equal to zero. The enthalpy change can be calculated by subtracting the enthalpy value of the products from the enthalpy value of the reactants , i.e.:

∆ H = Hp – Hr

∆H → Enthalpy change

Hp → Enthalpy of products

Hr → Enthalpy of reactants

The result of the enthalpy change calculation will determine whether we are dealing with a reaction that releases or absorbs heat, as can be seen in the following graphs:

Types

enthalpy of formation

It is the change in thermal energy involved in the formation of one mole of any substance , whether formed based on simple substances or in the ground state, as in the following example:

1/2H ₂ + O ₂ = H ₂ O

→ Note that the reagents are both simple substances, that is, they have an enthalpy equal to 0, and that the enthalpy value of water (H 2 _O ) is predetermined in the laboratory, therefore being a given given, therefore, the calculation of the enthalpy change is as follows:

∆H = Hp – Hr

∆H = (-68.4) – (1/2.0 + 0)
∆H = -68.4 → Exothermic reaction

→ Note that we have a result less than 0, which means that, in this reaction of formation of one mole of H ₂ O, we will release energy.

enthalpy of combustion

It is the measured change in heat required for the combustion of 1 mole of any substance. Every combustion reaction will have an enthalpy change value less than zero, as it is a reaction that releases heat.

• Example

Reaction and enthalpy change value for the ethanol combustion reaction:

C ₂ H ₆ O(l) + 3.O ₂ (g) → 2 CO ₂ (g) + 3 H ₂ O(l) ΔH = -326 Kcal/mol

The following are enthalpy of combustion values ​​for some common substances:

• Gaseous ethanol (C ₂ H ₆ )= -372.8 Kcal/mol
• Liquid benzene (C ₆ H ₆ ) = -781.0 Kcal/mol
• Solid sucrose (C ₁₂ H ₂₂ O ₁₁ ) = -1348.9 Kcal/mol

binding enthalpy

It is the energy required to break one mole of a chemical bond . The energy variation in this case always results in a value greater than 0, that is, the breaking of bonds requires heat absorption.

• Example

CH ₄ (g)+C(g)+4H(g) ΔH = +1,651.6 kJ/mol

C – H → C(g) + H(g) ΔH = +412.9 KJ/mol

Cl – Cl → Cl(g) + Cl (g) ΔH = +242.0 KJ/mol

Of neutralization

It is the energy change in neutralization reactions , such as acid-base neutralization:

Acid + base = salt + water → exothermic

As in other cases of enthalpy, for the neutralization values, the calculations for 1 mol must be considered. In this case, the final value of the enthalpy change will be, for the neutralization reaction, 1 mol of H ⁺ to 1 mol of OH ^–

Of dissolution

It is the variation in thermal energy involved in the dissolution of a mole of a given solute in an “x” amount of water or any other solvent, provided that there is complete solubilization and it becomes a homogeneous mixture .

• Example

NaCl(s) + aq → Na+(aq) + Cl-(aq) ∆H = -0.9 Kcalmol

In the reaction, we can chemically see the dissolution of sodium hydroxide , popularly known as caustic soda, in an aqueous medium. Note that the reaction has an enthalpy change of less than zero, which means that heat is released. This reaction is commonly carried out in the manufacture of homemade soap, a process that, when not carried out with due care, can result in accidents with burns of up to 3rd degree.

Difference and Comparison

1. It represents the total energy of a system, while entropy measures the degree of disorder or randomness of the system.
2. A positive change in enthalpy implies heat absorption, while a negative change means heat release; increasing entropy indicates increased disorder, while decreasing entropy suggests order.
3. It and entropy influence the spontaneity of reactions, with more negative enthalpy changes and more positive entropy changes making reactions more spontaneous.

Enthalpy vs Entropy

The difference between enthalpy and entropy is that enthalpy is a measure of the total energy of a system, which is the sum of internal energy and the product of pressure and volume. On the other hand, entropy is the amount of thermal energy in a system that is not available for its conversion into work. 

Comparison table