### Calculating ΔG from ΔH and ΔSA chemical engineer is studying the two reactions shown in the table below.In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 18.0 °C and constant total pressure. Then, she measures the reaction enthalpy ΔH and reaction entropy ΔS of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of her measurements are shown in the table.Complete the table. That is, calculate ΔG for the first reaction and ΔS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous and the system is at equilibrium.### Table:1. **First Reaction:** - Reaction: \(6 \text{C}_3 (g) + 2 \text{Te}_3 (g) \rightarrow 4 \text{C}_8 (g) + 3 \text{O}_2 (g)\) - ΔH = 50. kJ - ΔS = 172 J/K - ΔG = [input field] **Which is spontaneous?** - ○ the forward reaction - ○ the reverse reaction - ○ neither2. **Second Reaction:** - Reaction: \(2 \text{CO}_2 (g) + 4 \text{H}_2 (g) \rightarrow 2 \text{CH}_4 (g) + 3 \text{O}_2 (g)\) - ΔH = [input field] kJ - ΔS = [input field] J/K - ΔG = 1353 kJ **Which is spontaneous?** - ○ the forward reaction - ○ the reverse reaction - ○ neither### Instructions:- Calculate ΔG and ΔS using the provided data.- Determine the spontaneity of each reaction under the given conditions.### Explanation and Check:- Use the Gibbs free energy equation: \(ΔG = ΔH - TΔS\), where T is the temperature in Kelvin.This educational content allows students to apply thermodynamic concepts to real-world reactions, enhancing their understanding

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A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 18.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 6C, (e) + 2Fe,0, (s) 4FeC1, () + 30, (e) 200, (e) + 4H₂O(e)- 2CH, OH (e) + 30, (e) All 50 kJ AS 172 AG=J AH Which is spontaneous? O this reaction O the reverse reaction O neither } AS= -0 K 1353. kJ AG = 4, KJ Which is spontaneous? O this reaction O the reverse reaction Oneither 05 d X Lara G dh 4

A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 18.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 6C, (e) + 2Fe,0, (s) 4FeC1, () + 30, (e) 200, (e) + 4H₂O(e)- 2CH, OH (e) + 30, (e) All 50 kJ AS 172 AG=J AH Which is spontaneous? O this reaction O the reverse reaction O neither } AS= -0 K 1353. kJ AG = 4, KJ Which is spontaneous? O this reaction O the reverse reaction Oneither 05 d X Lara G dh 4

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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