Free Energy of Dissolution

The video tutorial explores the dissolution of ionic solids, focusing on sodium chloride in water. It explains the process of ions becoming solvated and the role of ion-dipole interactions. The Gibbs free energy equation is introduced, highlighting the importance of enthalpy and entropy in determining spontaneity. The tutorial provides a quantitative analysis of lattice and hydration energies, showing that sodium chloride dissolution is slightly endothermic but entropically driven. The impact of temperature on solubility is discussed, emphasizing the need to consider both enthalpy and entropy in chemical processes.

What is the primary interaction that occurs when sodium chloride dissolves in water?

• Van der Waals forces

• Ion-dipole interactions

• Covalent bonding

• Hydrogen bonding

Which equation is used to determine the spontaneity of a process?

• Boyle's Law

• Gibbs Free Energy Equation

• Avogadro's Law

• Newton's Second Law

What is the lattice energy of sodium chloride?

• 774 kilojoules per mole

• 778 kilojoules per mole

• 4 kilojoules per mole

• 0 kilojoules per mole

Why is the dissolution of sodium chloride considered entropically driven?

• It releases heat

• It involves a dispersal of matter

• It forms a solid precipitate

• It absorbs heat

How does temperature affect the solubility of most ionic solids?

• Solubility increases with temperature

• Solubility remains constant

• Temperature has no effect

• Solubility decreases with temperature