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In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °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. ΔΗ = -439, kJ AS = -1179. J K X

In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °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. ΔΗ = -439, kJ AS = -1179. J K X

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.79QE
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In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °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 because the system is at equilibrium. Reaction 1: \[ P_4O_{10(s)} + 6H_2O_{(l)} \rightarrow 4H_3PO_{4(s)} \] - ΔH = -439. kJ - ΔS = -1179. J/K - ΔG = [ ] kJ Which is spontaneous? - [ ] this reaction - [ ] the reverse reaction - [ ] neither Reaction 2: \[ 2NH_{3(g)} \rightarrow N_2H_{4(g)} + H_{2(g)} \] - ΔH = 188. kJ - ΔS = [ ] J/K - ΔG = 16. kJ Which is spontaneous? - [ ] this reaction - [ ] the reverse reaction - [ ] neither Diagram: There is no specific graph or diagram present in the image, just textual boxes to fill in calculations.
Transcribed Image Text:In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °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 because the system is at equilibrium. Reaction 1: \[ P_4O_{10(s)} + 6H_2O_{(l)} \rightarrow 4H_3PO_{4(s)} \] - ΔH = -439. kJ - ΔS = -1179. J/K - ΔG = [ ] kJ Which is spontaneous? - [ ] this reaction - [ ] the reverse reaction - [ ] neither Reaction 2: \[ 2NH_{3(g)} \rightarrow N_2H_{4(g)} + H_{2(g)} \] - ΔH = 188. kJ - ΔS = [ ] J/K - ΔG = 16. kJ Which is spontaneous? - [ ] this reaction - [ ] the reverse reaction - [ ] neither Diagram: There is no specific graph or diagram present in the image, just textual boxes to fill in calculations.
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