Thermodynamics Concepts and Applications

Mr. Aiden introduces unit 6 on thermodynamics, focusing on Gibbs free energy, enthalpy, and entropy. Gibbs free energy (Delta G) determines reaction favorability, with negative values indicating favorable reactions. Enthalpy (Delta H) is the heat per mole, with negative values for exothermic reactions and positive for endothermic. Entropy (Delta S) measures particle dispersion, with positive values indicating greater disorder. The video explains the importance of unit consistency in calculations, particularly in the equation Delta G = Delta H - T Delta S.

What is the main focus of the first video in the thermodynamics series?

• Atomic structure and periodic trends

• Gibbs free energy, enthalpy, and entropy

• Chemical kinetics and reaction rates

• Electrochemistry and its applications

What condition must be met for a reaction to be thermodynamically favorable?

• Delta G must be greater than Delta H

• Delta G must be positive

• Delta G must be zero

• Delta G must be negative

How is Gibbs free energy related to the equilibrium constant (Keq)?

• A negative Delta G means Keq is less than one

• A zero Delta G means Keq is less than one

• A negative Delta G means Keq is greater than one

• A positive Delta G means Keq is greater than one

What is the definition of enthalpy?

• The energy required to start a reaction

• The measure of disorder in a system

• The amount of heat per mole of a substance

• The total energy of a system

Which of the following is true for an exothermic reaction?

• Delta H is negative

• Delta H is zero

• Delta H is positive

• Delta H is greater than Delta S

What happens to entropy when a solid changes to a gas?

• Entropy decreases

• Entropy remains constant

• Entropy increases

• Entropy becomes zero

How does the number of moles affect entropy in a reaction?

• More moles in products increase entropy

• More moles in reactants decrease entropy

• Fewer moles in products increase entropy

• Fewer moles in reactants decrease entropy

What is the unit of entropy?

• Kilojoules per mole

• Joules per mole Kelvin

• Joules per mole

• Kilojoules per mole Kelvin

Why is it important to convert entropy units when using the equation Delta G = Delta H - T Delta S?

• To ensure all units are in joules

• To ensure all units are in moles

• To ensure all units are in kilojoules

• To ensure all units are in Kelvin

What is the relationship between Delta G, Delta H, and Delta S in thermodynamics?

• Delta G = T Delta H - Delta S

• Delta G = Delta H + T Delta S

• Delta G = Delta H - T Delta S

• Delta G = Delta S - T Delta H