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Ch.19 - Free Energy & Thermodynamics
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Not the one you use?Change textbook
All textbooksTro 5th EditionCh.19 - Free Energy & ThermodynamicsProblem 86
Chapter 19, Problem 86

Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possible reactions is shown here. Calculate ΔG° and Kp for this reaction at 25 °C and comment on the spontaneity of the reaction. 3 NO2(g) + H2O(l)→ 2 HNO3(aq) + NO(g)

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Step 1: To calculate the standard Gibbs free energy change (ΔG°), we need to know the standard Gibbs free energies of formation (ΔGf°) for all substances involved in the reaction. These values can be found in a standard thermodynamic table. The formula to calculate ΔG° is: ΔG° = Σ (ΔGf° products) - Σ (ΔGf° reactants).
Step 2: Once you have the ΔG°, you can calculate the equilibrium constant (Kp) using the formula: ΔG° = -RT ln(Kp), where R is the gas constant (8.314 J/(mol·K)) and T is the temperature in Kelvin (25°C = 298.15 K). Rearrange the formula to solve for Kp: Kp = e^(-ΔG°/(RT)).
Step 3: If ΔG° is negative, the reaction is spontaneous in the forward direction. If ΔG° is positive, the reaction is non-spontaneous in the forward direction and spontaneous in the reverse direction. If ΔG° is zero, the reaction is at equilibrium.
Step 4: If Kp is greater than 1, the reaction will proceed to the right, favoring the products. If Kp is less than 1, the reaction will proceed to the left, favoring the reactants. If Kp equals 1, the reaction is at equilibrium.
Step 5: Based on the calculated values of ΔG° and Kp, comment on the spontaneity of the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Gibbs Free Energy (ΔG°)

Gibbs Free Energy (ΔG°) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic process at constant temperature and pressure. A negative ΔG° indicates that a reaction is spontaneous, while a positive ΔG° suggests non-spontaneity. The value of ΔG° can be calculated using standard enthalpy and entropy changes, providing insight into the favorability of a reaction.
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Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a dimensionless value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction, raised to the power of their stoichiometric coefficients. For gaseous reactions, Kp is calculated using partial pressures. The relationship between ΔG° and Kp is given by the equation ΔG° = -RT ln(Kp), linking thermodynamics with chemical equilibrium.
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Spontaneity of Reactions

The spontaneity of a reaction refers to its ability to proceed without external intervention. It is determined by the sign of ΔG°; if ΔG° is negative, the reaction is spontaneous under standard conditions. Factors such as temperature, pressure, and concentration can influence spontaneity, and understanding these factors is crucial for predicting the behavior of chemical reactions in various environments.
Related Practice
Textbook Question

Consider this reaction occurring at 298 K: N2O(g) + NO2(g) ⇌ 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔG°rxn.

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Textbook Question

Determine the sign of ΔSsys for each process. a. water boiling

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Textbook Question

Consider the reaction: 2 NO(g) + O2(g) ⇌ 2 NO2(g) The following data show the equilibrium constant for this reaction measured at several different temperatures. Use the data to find ΔH°rxn and ΔS°rxn for the reaction.

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Textbook Question

Determine the sign of ΔSsys for each process. b. water freezing

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