Consider the reaction: H2(g) + F2(g)2HF(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.190 moles of H2(g) react at standard conditions. AG° kJ
Consider the reaction: H2(g) + F2(g)2HF(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.190 moles of H2(g) react at standard conditions. AG° kJ
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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![**Chemical Reaction Free Energy Calculation**
**Consider the Reaction:**
\[ \text{H}_2(\text{g}) + \text{F}_2(\text{g}) \rightarrow 2\text{HF}(\text{g})\]
**Problem Statement:**
Using standard thermodynamic data at 298K, calculate the free energy change when 2.190 moles of \(\text{H}_2(\text{g})\) react at standard conditions.
**Equation:**
\[ \Delta G^\circ_{\text{rxn}} = \underline{\hspace{3cm}} \text{kJ} \]
**Instructions:**
To solve this problem, you will need to refer to standard thermodynamic tables for values like the Gibbs free energy of formation (\(\Delta G^\circ_f\)) for each compound at 298K. Calculate the Gibbs free energy change \(\Delta G^\circ_{\text{rxn}}\) for the reaction using the following steps:
1. **Write out the balanced chemical equation for the reaction.**
2. **Find the \(\Delta G^\circ_f\) values for \(\text{H}_2(\text{g})\), \(\text{F}_2(\text{g})\), and \(\text{HF}(\text{g})\).**
3. **Apply the formula to calculate \(\Delta G^\circ_{\text{rxn}}\):**
\[ \Delta G^\circ_{\text{rxn}} = \sum \Delta G^\circ_{f(\text{products})} - \sum \Delta G^\circ_{f(\text{reactants})}\]
4. **After determining \(\Delta G^\circ_{\text{rxn}}\) for 1 mole of \(\text{H}_2(\text{g})\), calculate the total free energy change for 2.190 moles of \(\text{H}_2(\text{g})\).**
\[ \Delta G = \Delta G^\circ_{\text{rxn}} \times 2.190 \text{ moles} \]
**Note:** Fill in the value computed for the free energy change in the provided box.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77bfbc94-404c-40d5-8c71-b661b10ff379%2F743e0544-5965-4b67-972d-90b249adfba2%2Flz5twp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction Free Energy Calculation**
**Consider the Reaction:**
\[ \text{H}_2(\text{g}) + \text{F}_2(\text{g}) \rightarrow 2\text{HF}(\text{g})\]
**Problem Statement:**
Using standard thermodynamic data at 298K, calculate the free energy change when 2.190 moles of \(\text{H}_2(\text{g})\) react at standard conditions.
**Equation:**
\[ \Delta G^\circ_{\text{rxn}} = \underline{\hspace{3cm}} \text{kJ} \]
**Instructions:**
To solve this problem, you will need to refer to standard thermodynamic tables for values like the Gibbs free energy of formation (\(\Delta G^\circ_f\)) for each compound at 298K. Calculate the Gibbs free energy change \(\Delta G^\circ_{\text{rxn}}\) for the reaction using the following steps:
1. **Write out the balanced chemical equation for the reaction.**
2. **Find the \(\Delta G^\circ_f\) values for \(\text{H}_2(\text{g})\), \(\text{F}_2(\text{g})\), and \(\text{HF}(\text{g})\).**
3. **Apply the formula to calculate \(\Delta G^\circ_{\text{rxn}}\):**
\[ \Delta G^\circ_{\text{rxn}} = \sum \Delta G^\circ_{f(\text{products})} - \sum \Delta G^\circ_{f(\text{reactants})}\]
4. **After determining \(\Delta G^\circ_{\text{rxn}}\) for 1 mole of \(\text{H}_2(\text{g})\), calculate the total free energy change for 2.190 moles of \(\text{H}_2(\text{g})\).**
\[ \Delta G = \Delta G^\circ_{\text{rxn}} \times 2.190 \text{ moles} \]
**Note:** Fill in the value computed for the free energy change in the provided box.
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