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F. Is this reaction thermodynamically favorable at 25°C? Justify with a calculation.

F. Is this reaction thermodynamically favorable at 25°C? Justify with a calculation.

Chemistry
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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4.) HX is used as a reagent in the reaction below. NH2 HO, + HX + :NEN: A. What functional-group transformation occurs in this reaction? B. What is the likely identity of HX? Verify your decision with the table of Ka values in the back of your textbook. Consider the following thermodynamic data for the reaction shown above. NH2 он + HX + :NEN: AH°r (kJ/mol) -386 260.1 30.00 -393.5 S° (J/mol K) 166 146.0 191.3 191.5 213.8 C. Does the reaction absorb or release heat? Justify with a calculation. D. Based on the reaction equation given above, does entropy increase or decrease in this reaction? E. Justify your answer to (D) with a calculation. Does your calculation agree with your prediction? F. Is this reaction thermodynamically favorable at 25°C? Justify with a calculation. G. Over what temperature range (in K) is the above reaction thermodynamically favorable? H. Calculate the numerical value of the equilibrium constant at 25 °C for this reaction. Is your K value consistent with your answer to F? Explain.
Transcribed Image Text:4.) HX is used as a reagent in the reaction below. NH2 HO, + HX + :NEN: A. What functional-group transformation occurs in this reaction? B. What is the likely identity of HX? Verify your decision with the table of Ka values in the back of your textbook. Consider the following thermodynamic data for the reaction shown above. NH2 он + HX + :NEN: AH°r (kJ/mol) -386 260.1 30.00 -393.5 S° (J/mol K) 166 146.0 191.3 191.5 213.8 C. Does the reaction absorb or release heat? Justify with a calculation. D. Based on the reaction equation given above, does entropy increase or decrease in this reaction? E. Justify your answer to (D) with a calculation. Does your calculation agree with your prediction? F. Is this reaction thermodynamically favorable at 25°C? Justify with a calculation. G. Over what temperature range (in K) is the above reaction thermodynamically favorable? H. Calculate the numerical value of the equilibrium constant at 25 °C for this reaction. Is your K value consistent with your answer to F? Explain.
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