Pollowing und ex plain why. a.) Electrolysis of water to give gaseaus hudrogen and Oxygen b) Dissoluing of a s mall amount of Sodium nitrate in water (the solution becomes colk

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Title: Thermodynamic Sign Predictions for Various Chemical Processes

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**Objective:**

Evaluate the expected signs for changes in Gibbs free energy (ΔG°), enthalpy (ΔH°), and entropy (ΔS°) for each of the following processes, with explanations for each prediction.

---

**Processes:**

1. **Electrolysis of water to give gaseous hydrogen and oxygen:**

   - Predict the thermodynamic signs for ΔG°, ΔH°, and ΔS°.
   - Provide an explanation based on the nature of electrolysis as an endothermic, non-spontaneous process, resulting in increased disorder due to gas formation.

2. **Dissolving a small amount of sodium nitrate in water (the solution becomes cold):**

   - Predict the signs for ΔG°, ΔH°, and ΔS°.
   - Explain how the endothermic nature of the process (indicated by the cooling effect) and the increase in disorder affect these thermodynamic values.

3. **Combustion of wood:**

   - Determine the expected signs for ΔG°, ΔH°, and ΔS°.
   - Discuss how the exothermic release of energy and increased disorder from gaseous product formation influence these values.

---

This exercise helps in understanding the relationship between chemical processes and their thermodynamic properties, which is crucial for predicting the spontaneity and behavior of reactions.
Transcribed Image Text:Title: Thermodynamic Sign Predictions for Various Chemical Processes --- **Objective:** Evaluate the expected signs for changes in Gibbs free energy (ΔG°), enthalpy (ΔH°), and entropy (ΔS°) for each of the following processes, with explanations for each prediction. --- **Processes:** 1. **Electrolysis of water to give gaseous hydrogen and oxygen:** - Predict the thermodynamic signs for ΔG°, ΔH°, and ΔS°. - Provide an explanation based on the nature of electrolysis as an endothermic, non-spontaneous process, resulting in increased disorder due to gas formation. 2. **Dissolving a small amount of sodium nitrate in water (the solution becomes cold):** - Predict the signs for ΔG°, ΔH°, and ΔS°. - Explain how the endothermic nature of the process (indicated by the cooling effect) and the increase in disorder affect these thermodynamic values. 3. **Combustion of wood:** - Determine the expected signs for ΔG°, ΔH°, and ΔS°. - Discuss how the exothermic release of energy and increased disorder from gaseous product formation influence these values. --- This exercise helps in understanding the relationship between chemical processes and their thermodynamic properties, which is crucial for predicting the spontaneity and behavior of reactions.
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