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Ch.18 - Free Energy and Thermodynamics
Chapter 18, Problem 64

Using standard free energies of formation, calculate ΔG° at 25 °C for each reaction in Problem 62. How do the values of ΔG° calculated this way compare to those calculated from ΔH° and ΔS°? Which of the two methods can determine how ΔG° changes with temperature?

Verified step by step guidance
1
Identify the chemical reactions from Problem 62 for which you need to calculate ΔG.
Use the standard free energies of formation ΔGf for each reactant and product to calculate ΔG for the reaction using the formula: ΔG=ΔGf(products)ΔGf(reactants).
Compare the ΔG values obtained from the standard free energies of formation with those calculated using the equation ΔG=ΔHTΔS, where ΔH is the standard enthalpy change and ΔS is the standard entropy change.
Discuss how the two methods compare in terms of accuracy and applicability, especially considering that the ΔG=ΔHTΔS method can be used to determine how ΔG changes with temperature.
Conclude which method is more suitable for predicting the temperature dependence of ΔG and why.
Related Practice
Textbook Question

For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C? c. N2(g) + O2(g) → 2 NO(g)

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Textbook Question

For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C? d. 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

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Textbook Question

Use standard free energies of formation to calculate ΔG° at 25 °C for each reaction in Problem 61. How do the values of ΔG° calculated this way compare to those calculated from ΔH° and ΔS°? Which of the two methods could be used to determine how ΔG° changes with temperature?

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Open Question
Is the question formulated correctly? If not, please correct it. Here is the question: 'Consider the reaction: 2 NO( g) + O2( g) → 2 NO2( g). Estimate ΔG° for this reaction at each temperature and predict whether or not the reaction is spontaneous, assuming that ΔH° and ΔS° do not change significantly within the given temperature range. a. 298 K b. 855 K.'
Textbook Question

Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) Estimate ΔG° for this reaction at each temperature and predict whether or not the reaction is spontaneous. (Assume that ΔH° and ΔS° do not change too much within the given temperature range.) b. 715 K

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Open Question
Consider the reaction: CaCO3(s) → CaO(s) + CO2(g). Estimate ΔG° for this reaction at each temperature and predict whether or not the reaction is spontaneous. (Assume that ΔH° and ΔS° do not change too much within the given temperature range.) a. 298 K b. 1055 K c. 1455 K.