CHM2046-Chemistry Fundamentals II: Free Energy and Thermodynamics

This set of flashcards covers key concepts in thermodynamics and free energy from the chemistry lecture notes, focusing on definitions, equations, and principles involved in the subject.

What is Heat Death in thermodynamics?

A state of no thermodynamic free energy.

What does ΔG represent in a chemical reaction?

Free energy change of the reaction.

What is Hess's Law?

The total ΔG of a reaction can be calculated as the sum of the ΔG values of the individual steps.

How does the sign of ΔG change when a reaction is reversed?

The sign of its ΔG value reverses.

What happens to ΔG if the amount of reactants/products is multiplied by a factor?

The value of ΔG is multiplied by the same factor.

Under what conditions is ΔG equal to ΔGo?

When the reactants and products are in their standard states.

What is the reaction quotient (Q) under nonstandard conditions?

It is the ratio of the concentration of products to reactants at any point in a reaction.

What does ΔG = 0 signify in a reaction?

The system is at equilibrium.

How do standard states for gases vary?

Partial pressure of gas = 1 atm; concentrations = 1 M.

How do you relate ΔGo rxn to K?

ΔGo rxn = -RTln(K), where R is the gas constant and T is the temperature.

What does a ΔGo value greater than 0 indicate about a reaction?

The reaction is nonspontaneous under standard conditions.

What occurs when K < 1 in terms of ΔGo?

ΔGo is positive, indicating the reaction is spontaneous in the reverse direction.

How do you derive K from the standard free energy change?

K = e^(-ΔGo/RT).

What is the equation for temperature dependence of K?

∆Go = ∆Ho - T∆So.