10.[s] The amino acid glycine dimerizes to form the dipeptide glycylglycine (say that three times fast!) according to the reaction: 2Glycine(s) → Glycylglycine(s) + H₂O(1) Calculate 4S, 4S and 4Suniverse at 298 K. Is the reaction spontaneous at this temperature? Useful thermodynamic data in the Table below: AH,(kJ mol-¹) 45° (JK mol) Glycine -537.2 103.5 Glycylglycine -746.0 190.0 Water -285.8 70.0

10.[s] The amino acid glycine dimerizes to form the dipeptide glycylglycine (say that three times fast!) according to the reaction: 2Glycine(s) → Glycylglycine(s) + H₂O(1) Calculate 4S, 4S and 4Suniverse at 298 K. Is the reaction spontaneous at this temperature? Useful thermodynamic data in the Table below: AH,(kJ mol-¹) 45° (JK mol) Glycine -537.2 103.5 Glycylglycine -746.0 190.0 Water -285.8 70.0

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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Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: C,H; (g) + 50, (g) - 3CO, g) + 4H,0 (1) Round your answer to zero decimal places. J x10 K
Find AG for the following reaction at 298.15 K, using AH and S significant figures. MnO₂ (s) + 2CO(g) - Mn(s) + 2CO₂ (g) Note: Reference the Thermodynamic properties of pure substances table for additional information. Note: Reference the SI prefixes table for additional information. kJ 0.8 values. Be sure your answer has the correct number of t X
A eq req E Consider the reaction: 2SO₂(g) + O2(g) → 2SO3(g) Using standard thermodynamic data at 298 K, calculate the free energy change when 1.57 moles of SO₂(g) react at standard conditions. AG = Substance AG (kJ/mol) SO3(g) SO₂(g) 0₂ (9) Submit Answer $ R % k] 5 Show Hint Use the References to access important values if needed for this question. T -371.1 -300.2 0.0 Retry Entire Group B Cengage Learning Cengage Technical Support ^ 6 9 more group attempts remaining H & 7 N J * 8 M 1 K ( 1 O P Previous Next> D ㅈ R 7 Save and Exit
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1. 2NO(g) + O2(g) → 2NO;(g) DH° = -112 kJ/mol Absolute Entropy at 298 K (J/(K mol)) NO(g) 211 O2(g) 205 NO2(9) 240 a. Explain the sign of the entropy change based on the chemical equation. b. Is the reaction thermodynamically favorable at 298K? Justify your answer based on the calculation of the value and sign of DG°. c. Is the value of the equilibrium constant, K, for the reaction greater than 1, or less than 1? Justify your answer.