**Title: Calculating Standard Free-Energy Change for a Chemical Reaction****Question:** What is the standard free-energy change, ΔG°, for the following reaction at 54.4 °C?\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \]**Table of Thermodynamic Data:**| Substance | ΔH°f (kJ/mol) | ΔS° (J/K·mol) ||-----------|----------------|----------------|| N₂(g) | 0 | 191.6 || H₂(g) | 0 | 130.6 || NH₃(g) | -45.9 | 192.7 |**Calculation:**\[ ΔG° = \_\_\_\_\_\_\_\_\_ \text{ kJ} \]**Buttons/Links:**- **Submit**- **Show Tutor Steps**This problem requires calculating the standard free-energy change (ΔG°) at a temperature of 54.4 °C. The thermodynamic data provided in the table include the standard enthalpy of formation (ΔH°f) and the standard entropy (ΔS°) for each substance involved in the reaction.To solve, you will need to apply the equation for calculating ΔG°:\[ ΔG° = ΔH° - TΔS° \]Where T is the temperature in Kelvin. Adjust the temperature from Celsius to Kelvin when performing calculations.

Answered: What is the standard free-energy…

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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Step 1

Step 1) Standard free energy:

The standard free energy or Gibbs free energy is defined as the energy which is associated with the chemical reaction that can be used to do the work.

Free energy of the system is the change in the enthalpy of the system subtracted by the product of the temperature and the change in the entropy.

. $∆ G = ∆ H - T ∆ S ∆ G = free energy ∆ H = change in enthaly T ∆ S = product or temperature and change in entropy$

Standard state free energy of reaction = $∆ G^{°}$

${∆G}^{°} = ∆ H^{°} - T ∆ S^{°}$

At a standard state conditions the compound is formed from its elements in their most thermodynamically states with which its said to be change in free energy.

$∆ G^{°} < 0 = reaction is spontaneous ∆ G^{°} > 0 = reaction is non spontaneous$

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