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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![### Calculating Standard Gibbs Free Energy Change (ΔG°)
To find the standard Gibbs free energy change (ΔG°) for the following reaction using the standard enthalpy of formation (ΔH°_f) and standard entropy (S°) values:
\[ \text{H}_2(g) + \text{I}_2(s) \rightarrow 2 \text{HI}(g) \]
Given Data:
- The given value to consider in your calculations or result is 206 kJ.
#### Explanation:
To calculate the Gibbs free energy change, you use the formula:
\[ \Delta G = \Delta H - T\Delta S \]
Where:
- \( \Delta G \) is the Gibbs free energy change.
- \( \Delta H \) is the enthalpy change.
- \( T \) is the temperature in Kelvin.
- \( \Delta S \) is the entropy change.
In this exercise, you would need the standard enthalpy of formation (ΔH°_f) and the standard entropy (S°) values for each substance involved in the reaction (H₂, I₂, and HI). Usually, these values can be found in standard thermodynamic tables.
Make sure to convert units where necessary and apply the correct temperature for standard conditions, typically 298 K.
---
This section introduces students to calculating Gibbs free energy change and provides the setup using given conditions. Ensure to fill in standard enthalpy and entropy values from known sources to complete the calculation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe0ae19d5-3750-41df-884f-8ca3aa31e002%2F52817acf-0290-4391-a3b7-6457926b6ceb%2Fyjijcxq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculating Standard Gibbs Free Energy Change (ΔG°)
To find the standard Gibbs free energy change (ΔG°) for the following reaction using the standard enthalpy of formation (ΔH°_f) and standard entropy (S°) values:
\[ \text{H}_2(g) + \text{I}_2(s) \rightarrow 2 \text{HI}(g) \]
Given Data:
- The given value to consider in your calculations or result is 206 kJ.
#### Explanation:
To calculate the Gibbs free energy change, you use the formula:
\[ \Delta G = \Delta H - T\Delta S \]
Where:
- \( \Delta G \) is the Gibbs free energy change.
- \( \Delta H \) is the enthalpy change.
- \( T \) is the temperature in Kelvin.
- \( \Delta S \) is the entropy change.
In this exercise, you would need the standard enthalpy of formation (ΔH°_f) and the standard entropy (S°) values for each substance involved in the reaction (H₂, I₂, and HI). Usually, these values can be found in standard thermodynamic tables.
Make sure to convert units where necessary and apply the correct temperature for standard conditions, typically 298 K.
---
This section introduces students to calculating Gibbs free energy change and provides the setup using given conditions. Ensure to fill in standard enthalpy and entropy values from known sources to complete the calculation.
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