In each case, the engineer fills a reaction vessel with a mixture of reactants and products at a constant temperature of 118.0 °C and a constant total pressure. They measure the reaction enthalpy (ΔH) and reaction entropy (ΔS) for the first reaction, and the reaction enthalpy (ΔH) and reaction free energy (ΔG) for the second reaction. The results of these measurements are shown in the table below.The task is to complete the table, calculating ΔG for the first reaction and ΔS for the second, rounding answers to zero decimal places. Then, decide whether, under the given conditions, the reaction or the reverse reaction is spontaneous, or if neither direction is spontaneous due to equilibrium.**Reaction 1:**\[ 3\text{CO}_2(g) + 4\text{H}_2\text{O}(l) \rightarrow \text{C}_3\text{H}_8(g) + 5\text{O}_2(g) \]- ΔH = 2220.0 kJ- ΔS = 5584.0 J/K- ΔG = [ ] kJ**Spontaneity:**- [ ] This reaction- [ ] The reverse reaction- [ ] Neither**Reaction 2:**\[ \text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 6\text{C}(s) + 6\text{H}_2(g) + 3\text{O}_2(g) \]- ΔH = 1237.0 kJ- ΔS = [ ] J/K- ΔG = -35.0 kJ**Spontaneity:**- [ ] This reaction- [ ] The reverse reaction- [ ] NeitherThe table requires completing the missing ΔG for Reaction 1 and ΔS for Reaction 2, followed by determining the spontaneity of each reaction under the given conditions.The diagrams adjacent to the table appear to show interactions or adjustable parameters in a typical thermodynamic task setup, possibly representing conceptual links between values.

Answered: Image /qna-images/answer/00001439-dae2-44e7-b693-5d7c35df7d33.jpg

In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 118.0 °C and constant total pressure. Then, he 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 his 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. 3CO₂ (g) + 4H₂O(l) C₂Hg (g) + 50₂ (8) C6H₁2O6 (s) 6C(s) + 6H₂(g) + 30₂ (g) AH 2220. kJ AS 5584. AG = Which is spontaneous? Othis reaction O the reverse reaction Oneither ΔΗ = 1237. kJ AS = J K J K AG = -35. kJ Which is spontaneous? Othis reaction the reverse reaction. neither X Do 3

In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 118.0 °C and constant total pressure. Then, he 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 his 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. 3CO₂ (g) + 4H₂O(l) C₂Hg (g) + 50₂ (8) C6H₁2O6 (s) 6C(s) + 6H₂(g) + 30₂ (g) AH 2220. kJ AS 5584. AG = Which is spontaneous? Othis reaction O the reverse reaction Oneither ΔΗ = 1237. kJ AS = J K J K AG = -35. kJ Which is spontaneous? Othis reaction the reverse reaction. neither X Do 3

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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