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Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: 2NH3(g) → N₂H₂(g) + H₂ (g) Round your answer to zero decimal places.

Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: 2NH3(g) → N₂H₂(g) + H₂ (g) Round your answer to zero decimal places.

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
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NH3(g) -45.9 -16.4 192.8

 The middle values are Delta G or Free energy. Thanks

N2H4(g) 95.4 159.4 238.5
H2(g) 0 0

130.7
**Thermodynamics and Reaction Free Energy Calculation** Using the thermodynamic information in the ALEKS *Data* tab, calculate the standard reaction free energy of the following chemical reaction: \[ 2\text{NH}_3 \, (g) \rightarrow \text{N}_2\text{H}_4 \, (g) + \text{H}_2 \, (g) \] Round your answer to zero decimal places.
Transcribed Image Text:**Thermodynamics and Reaction Free Energy Calculation** Using the thermodynamic information in the ALEKS *Data* tab, calculate the standard reaction free energy of the following chemical reaction: \[ 2\text{NH}_3 \, (g) \rightarrow \text{N}_2\text{H}_4 \, (g) + \text{H}_2 \, (g) \] Round your answer to zero decimal places.
### Thermodynamic Properties of Aluminum Compounds This table presents the standard thermodynamic properties of various aluminum compounds, including their standard enthalpy of formation (ΔHf°), standard Gibbs free energy of formation (ΔGf°), and standard entropy (S°). | Substance | ΔHf° (kJ/mol) | ΔGf° (kJ/mol) | S° (J/mol·K) | |------------|---------------|---------------|--------------| | Al(s) | 0 | 0 | 28.3 | | Al³⁺(aq) | -531.0 | -485.0 | -321.7 | | AlCl₃(s) | -704.2 | -628.8 | 109.3 | **Key Observations:** - **Al(s)**: Elemental aluminum in its solid form has a standard enthalpy and Gibbs free energy of formation of zero, which serves as a reference point. - **Al³⁺(aq)**: The aluminum ion in aqueous solution has a negative ΔHf° and ΔGf°, indicating that the formation of this ion is exothermic and thermodynamically favored. The entropy is notably negative, reflecting a decrease in disorder associated with the formation of Al³⁺ from Al. - **AlCl₃(s)**: Aluminum chloride exhibits a significantly negative ΔHf° and ΔGf°, suggesting its formation is highly exothermic and spontaneously favorable. The entropy is positive, indicating an increase in disorder when compared to the solid aluminum. These properties are crucial for understanding the energy changes and stability associated with reactions involving aluminum compounds.
Transcribed Image Text:### Thermodynamic Properties of Aluminum Compounds This table presents the standard thermodynamic properties of various aluminum compounds, including their standard enthalpy of formation (ΔHf°), standard Gibbs free energy of formation (ΔGf°), and standard entropy (S°). | Substance | ΔHf° (kJ/mol) | ΔGf° (kJ/mol) | S° (J/mol·K) | |------------|---------------|---------------|--------------| | Al(s) | 0 | 0 | 28.3 | | Al³⁺(aq) | -531.0 | -485.0 | -321.7 | | AlCl₃(s) | -704.2 | -628.8 | 109.3 | **Key Observations:** - **Al(s)**: Elemental aluminum in its solid form has a standard enthalpy and Gibbs free energy of formation of zero, which serves as a reference point. - **Al³⁺(aq)**: The aluminum ion in aqueous solution has a negative ΔHf° and ΔGf°, indicating that the formation of this ion is exothermic and thermodynamically favored. The entropy is notably negative, reflecting a decrease in disorder associated with the formation of Al³⁺ from Al. - **AlCl₃(s)**: Aluminum chloride exhibits a significantly negative ΔHf° and ΔGf°, suggesting its formation is highly exothermic and spontaneously favorable. The entropy is positive, indicating an increase in disorder when compared to the solid aluminum. These properties are crucial for understanding the energy changes and stability associated with reactions involving aluminum compounds.
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