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Chapter 10: Problem 18

Explain how a comprehensive table of standard Gibbs energies of formation can be used to determine the spontaneity of any chemical reaction.

Short Answer

Expert verified
Using standard Gibbs energies of formation from a table, one can calculate the Gibbs energy change for a reaction. This is done by subtracting the sum of the Gibbs energies of formation of the reactants from that of the products, taking into account their stoichiometric coefficients. If the final Gibbs energy change is negative, the reaction is spontaneous. Otherwise, it is non-spontaneous or at equilibrium.

Step by step solution

01

Understanding Gibbs Energy

The Gibbs free energy (\( \Delta G \)) is a thermodynamic potential that measures the maximum of reversible work that may be performed by a system at a constant temperature and pressure. When ΔG is negative, the process occurs spontaneously, and when it is positive, the process is non-spontaneous.
02

Meaning of Standard Gibbs energies of formation

The Standard Gibbs energy of formation (\( \Delta G_f^° \)) refers to the change of Gibbs energy when one mole of a substance in its standard state is formed from its pure elements under the same conditions. A table of standard Gibbs energies of formation contains these values for various substances under standard conditions.
03

Calculating reaction Gibbs energy

To determine the \( \Delta G \) for a chemical reaction, use the formula \( \Delta G = \Sigma n \Delta G_f^°(products) - \Sigma m \Delta G_f^°(reactants) \) , where n and m represent the stoichiometric coefficients of the products and reactants respectively. This formula calculates the Gibbs energy change by taking account of the difference between the sum of the Gibbs energies of formation of the products and the sum of the Gibbs energies of formation of the reactants.
04

Determining the spontaneity of the reaction

If the calculated \( \Delta G \) for the reaction is negative, the reaction is spontaneous. If it is positive, the reaction is non-spontaneous. If it is zero, the reaction is at equilibrium, meaning it can proceed in both directions.

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