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What is ∆G° for the reaction CaO(s) + CO₂(g) → CaCO₃(s)

What is ∆G° for the reaction CaO(s) + CO₂(g) → CaCO₃(s)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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What is ∆G° for the reaction CaO(s) + CO₂(g) → CaCO₃(s)?

### Standard Gibbs Free Energy of Formation The table below presents the standard Gibbs free energy of formation (\( \Delta G_f^\circ \)) for various substances, expressed in kilojoules per mole (kJ/mol): | Substance | \( \Delta G_f^\circ \) (kJ/mol) | |-----------|--------------------------------| | CaO (s) | -604 | | CO\(_2\) (g) | -394.4 | | CaCO\(_3\) (s) | -112.8 | **Explanation:** - **CaO (s):** Calcium oxide in solid form has a \( \Delta G_f^\circ \) of -604 kJ/mol. - **CO\(_2\) (g):** Carbon dioxide in gaseous form has a \( \Delta G_f^\circ \) of -394.4 kJ/mol. - **CaCO\(_3\) (s):** Calcium carbonate in solid form has a \( \Delta G_f^\circ \) of -112.8 kJ/mol. This data is useful for understanding the thermodynamic stability and reactivity of these substances under standard conditions.
Transcribed Image Text:### Standard Gibbs Free Energy of Formation The table below presents the standard Gibbs free energy of formation (\( \Delta G_f^\circ \)) for various substances, expressed in kilojoules per mole (kJ/mol): | Substance | \( \Delta G_f^\circ \) (kJ/mol) | |-----------|--------------------------------| | CaO (s) | -604 | | CO\(_2\) (g) | -394.4 | | CaCO\(_3\) (s) | -112.8 | **Explanation:** - **CaO (s):** Calcium oxide in solid form has a \( \Delta G_f^\circ \) of -604 kJ/mol. - **CO\(_2\) (g):** Carbon dioxide in gaseous form has a \( \Delta G_f^\circ \) of -394.4 kJ/mol. - **CaCO\(_3\) (s):** Calcium carbonate in solid form has a \( \Delta G_f^\circ \) of -112.8 kJ/mol. This data is useful for understanding the thermodynamic stability and reactivity of these substances under standard conditions.
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