Question

Derive relationship between \(\Delta H\) and \(\Delta U\) for gaseous reaction. Define: Vulcanization What is peptide bond?

Hint:

For gaseous reactions, the change in volume (\(\Delta n_g\)) directly affects the relationship between enthalpy and internal energy. Vulcanization is crucial for improving material properties in rubber.

Answer 1

Step 1: Relationship between \(\Delta H\) and \(\Delta U\) for Gaseous Reaction.
The relationship between enthalpy change (\(\Delta H\)) and internal energy change (\(\Delta U\)) for a gaseous reaction is: \[ \Delta H = \Delta U + \Delta n_g RT \] Where: - \(\Delta H\) is the change in enthalpy, - \(\Delta U\) is the change in internal energy, - \(\Delta n_g\) is the change in the number of moles of gas, - \(R\) is the gas constant, - \(T\) is the temperature. Step 2: Vulcanization.
Vulcanization is the process of cross-linking polymer chains, typically rubber, by adding sulfur. This process improves the elasticity, strength, and durability of the material, making it suitable for use in tyres and other rubber products. Step 3: Peptide Bond.
A peptide bond is the covalent bond formed between two amino acids when the carboxyl group of one amino acid reacts with the amino group of another, releasing a molecule of water. This bond is a fundamental link in protein structure.