**Gibbs Free Energy Calculation**Calculate ΔG° for the reaction below at a temperature of 25°C, given that ΔH° = -52.9 kJ and ΔS° = -166.4 J/K.\[ 2\text{HI}(g) \rightarrow \text{H}_2(g) + \text{I}_2(g) \]**Options:**a) -3.35 kJb) 3.35 kJc) -49.6 kJd) 49.6 kJ**Explanation:**To calculate the Gibbs free energy change (ΔG°) for a reaction, use the formula:\[ \Delta G^\circ = \Delta H^\circ - T\Delta S^\circ \]- **ΔH°**: Enthalpy change, given in kJ.- **ΔS°**: Entropy change, converted to kJ by dividing J by 1000.- **T**: Temperature in Kelvin, converted from Celsius by adding 273.15.Given:- ΔH° = -52.9 kJ- ΔS° = -166.4 J/K = -0.1664 kJ/K- T = 25°C = 25 + 273.15 = 298.15 KSubstitute these values into the formula to find ΔG°:\[ \Delta G^\circ = -52.9 \, \text{kJ} - (298.15 \, \text{K} \times -0.1664 \, \text{kJ/K}) \]Calculate ΔG° and select the correct option.

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Answered: Calculate AG for the reaction below at…

Calculate AG for the reaction below at a temperature of 25°C, given that AH° = -52.96 kJ and AS° = -166.4 J/K. 2HI(g) →H₂(g) + 1₂(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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