**Transcription for Educational Website:**---**Problem Statement:**Calculate the standard free energy change at 25.0 °C for the reaction between 0.620 mol of hydrogen gas and 0.220 mol of nitrogen to form ammonia, as shown in the following chemical equation:\[ 3\text{H}_2(g) + \text{N}_2(g) \rightarrow 2\text{NH}_3(g) \]**Given Answer:**\[ A: -6.77 \]---**Explanation:**In this problem, you are asked to calculate the standard free energy change (\(\Delta G^\circ\)) for the reaction described. This involves using the provided moles of hydrogen and nitrogen and applying thermodynamic principles to find the energy change in producing ammonia at the specified temperature (25.0 °C). The negative sign in the given answer indicates that the reaction is exergonic, meaning it releases energy.

First we need to calculate the moles of ammonia produced in this reaction. Then using the moles of each compound and their standard thermodynamic values we can calculate the standard free energy change for this reaction.

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5. From the information given in the textbook, calculate the standard free energy change at 25.0 °C for the reaction between 0.620 mol hydrogen gas and 0.220 mol nitrogen to form ammonia, shown in the following equation: 3H₂(g) + N₂(g). → 2NH3(8) A: -6.77

5. From the information given in the textbook, calculate the standard free energy change at 25.0 °C for the reaction between 0.620 mol hydrogen gas and 0.220 mol nitrogen to form ammonia, shown in the following equation: 3H₂(g) + N₂(g). → 2NH3(8) A: -6.77

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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**Transcription for Educational Website:**

---

**Problem Statement:**

Calculate the standard free energy change at 25.0 °C for the reaction between 0.620 mol of hydrogen gas and 0.220 mol of nitrogen to form ammonia, as shown in the following chemical equation:

\[ 3\text{H}_2(g) + \text{N}_2(g) \rightarrow 2\text{NH}_3(g) \]

**Given Answer:**

\[ A: -6.77 \]

---

**Explanation:**

In this problem, you are asked to calculate the standard free energy change (\(\Delta G^\circ\)) for the reaction described. This involves using the provided moles of hydrogen and nitrogen and applying thermodynamic principles to find the energy change in producing ammonia at the specified temperature (25.0 °C). The negative sign in the given answer indicates that the reaction is exergonic, meaning it releases energy.

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