Using values of Δ f H ° and S°, calculate the standard molar free energy of formation, Δ f G °, for each of the following: (a) Ca(OH) 2 (s) (b) Cl(g) (c) Na 2 CO 3 (s) Compare your calculated values of Δ f G° with those listed in Appendix L. Which of these formation reactions are predicted to be product-favored at equilibrium at 25 °C?
Using values of Δ f H ° and S°, calculate the standard molar free energy of formation, Δ f G °, for each of the following: (a) Ca(OH) 2 (s) (b) Cl(g) (c) Na 2 CO 3 (s) Compare your calculated values of Δ f G° with those listed in Appendix L. Which of these formation reactions are predicted to be product-favored at equilibrium at 25 °C?
Using values of ΔfH° and S°, calculate the standard molar free energy of formation, ΔfG°, for each of the following:
(a) Ca(OH)2(s)
(b) Cl(g)
(c) Na2CO3(s)
Compare your calculated values of ΔfG° with those listed in Appendix L. Which of these formation reactions are predicted to be product-favored at equilibrium at 25 °C?
(a)
Expert Solution
Interpretation Introduction
Interpretation:
The the standard molar free energy for formation of Ca(OH)2(s) should be calculated and compared with the values placed in appendix L. It should be identified that whether the reaction is product favored at equilibrium.
Concept introduction:
The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔGo. It is related to entropy and enthalpy by the following expression,
ΔGo=ΔHo-TΔSo
The sign of ΔGo should be positive for a product-favored reaction. Thus, spontaneous reactions are referred to those that have negative free energy formation.
Answer to Problem 34PS
The standard molar energy of formation for Ca(OH)2(s) is −898.486kJ/mol-rxn.
Explanation of Solution
The standard molar energy of formation for Ca(OH)2(s) is calculated below.
Given:
The Appendix L referred for the values of standard entropies and enthalpies.
The value of free energy change is negative. Thus, the reaction is product-favored at equilibrium.
(b)
Expert Solution
Interpretation Introduction
Interpretation:
The the standard molar free energy for formation of Cl(g) should be calculated and compared with the values placed in appendix L. It should be identified that whether the reaction is product favored at equilibrium.
Concept introduction:
The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔGo. It is related to entropy and enthalpy by the following expression,
ΔGo=ΔHo-TΔSo
The sign of ΔGo should be positive for a product-favored reaction. Thus, spontaneous reactions are referred to those that have negative free energy formation.
Answer to Problem 34PS
The standard molar energy of formation for Cl(g) is 105.3kJ/mol-rxn.
Explanation of Solution
The standard molar energy of formation for Cl(g) is calculated below.
Given:
The Appendix L referred for the values of standard entropies and enthalpies.
The value of free energy change is positive. Thus, the reaction is reactant-favored at equilibrium.
(c)
Expert Solution
Interpretation Introduction
Interpretation:
The the standard molar free energy for formation of Na2CO3(s) should be calculated and compared with the values placed in appendix L. It should be identified that whether the reaction is product favored at equilibrium.
Concept introduction:
The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔGo. It is related to entropy and enthalpy by the following expression,
ΔGo=ΔHo-TΔSo
The sign of ΔGo should be positive for a product-favored reaction. Thus, spontaneous reactions are referred to those that have negative free energy formation.
Answer to Problem 34PS
The standard molar energy of formation for Na2CO3(s) is −1047.08kJ/mol-rxn.
Explanation of Solution
The standard molar energy of formation for Na2CO3(s) is calculated below.
Given:
The Appendix L referred for the values of standard entropies and enthalpies.
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY