Certainly! Here is a transcription of the image, designed for an educational website:---### Thermodynamics Problem Set**Note:** To find the value of the equilibrium constant at each temperature, you must first find the value of ΔG° at each temperature:\[ \Delta G^\circ = \Delta H^\circ - T \Delta S^\circ \]For this reaction, the values are $ \Delta H^\circ = +88.3 \, \text{kJ/mol} $ and $ \Delta S^\circ = -151.3 \, \text{J/mol}\cdot\text{K} $.---**13. [0.05/0.1 Points]****Details** | **Previous Answers****2/4 Submissions Used**Consider the reaction $ 2 \text{NO}_2 (g) \rightarrow \text{N}_2\text{O}_4 (g) $.(a) Using $ \Delta G_f \text{N}_2\text{O}_4 (g) = 97.79 \, \text{kJ/mol} $ and $ \Delta G_f \text{NO}_2 (g) = 51.3 \, \text{kJ/mol} $, calculate $ \Delta G^\circ $ at 298 K. \[ 4.81 \, \text{kJ} \] ✔️(b) Calculate $ \Delta G $ at 298 K if the partial pressures of $ \text{NO}_2 $ and $ \text{N}_2\text{O}_4 $ are 0.25 atm and 1.35 atm, respectively. \[ 12.37 \, \text{kJ} \] ❌---**14. [0.1/0.1 Points]****Details** | **Previous Answers****2/4 Submissions Used**Consider the reaction given below.\[ \text{H}_2(g) + \text{F}_2(g) \rightarrow 2 \text{HF}(g) \](a) Using thermodynamic data from the course website, calculate $ \Delta G^\circ $ at 298 K. \[ -546.4 \, \text{kJ} \] ✔️---This problem set is intended to help students understand the application of thermodynamics in chemical reactions

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←C Secure | https://www.webassign.net/web/Student/Assignment-Responses/submit?dep=29518359&tags=autosav Note: To find the value of the equilibrium constant at each temperature you must first find the value of AGO at each temp AGO AHO - TASO For this reaction the values are AHO = +88.3 kJ/mol and AS0= 151.3 J/mol*K 13. [0.05/0.1 Points] DETAILS 14. [0.1/0.1 Points] PREVIOUS ANSWERS Consider the reaction 2 NO2(g) → N₂O4(g) . (a) Using AG N2O4(g) = 97.79 kJ/mol and AGF NO₂(g) = 51.3 kJ/mol, calculate AG° at 298 K. -4.81 ✓ KJ DETAILS Course: 2022 Fall ENGL 200 X (b) Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.25 atm and 1.35 at, respectively. X KJ 12.37 Consider the reaction given below. 2/4 Submissions Used PREVIOUS ANSWERS 2/4 Submissions Used (a) Using thermodynamic data from the course website, calculate AG° at 298 K. -546.4 KJ H₂(g) + F2(g) → 2 HF(g)

←C Secure | https://www.webassign.net/web/Student/Assignment-Responses/submit?dep=29518359&tags=autosav Note: To find the value of the equilibrium constant at each temperature you must first find the value of AGO at each temp AGO AHO - TASO For this reaction the values are AHO = +88.3 kJ/mol and AS0= 151.3 J/mol*K 13. [0.05/0.1 Points] DETAILS 14. [0.1/0.1 Points] PREVIOUS ANSWERS Consider the reaction 2 NO2(g) → N₂O4(g) . (a) Using AG N2O4(g) = 97.79 kJ/mol and AGF NO₂(g) = 51.3 kJ/mol, calculate AG° at 298 K. -4.81 ✓ KJ DETAILS Course: 2022 Fall ENGL 200 X (b) Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.25 atm and 1.35 at, respectively. X KJ 12.37 Consider the reaction given below. 2/4 Submissions Used PREVIOUS ANSWERS 2/4 Submissions Used (a) Using thermodynamic data from the course website, calculate AG° at 298 K. -546.4 KJ H₂(g) + F2(g) → 2 HF(g)

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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Answer the following questions based on the given information about this chemical reaction.
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A] HgS occurs in two crystalline forms called "red" and "black". For the conversion of 8. L- the red form to the black form at 525 °C, 4Gº = -0.157 kJ mol-¹ and AH = 4.184 kJ mol-¹. Assuming the AH is temperature independent, find the temperature at which the two forms can coexist at equilibrium at 1.000 bar. Which is more stable above this temperature?
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N8.
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