The amino acid glycine dimerizes to form the dipeptide glycylglycine according to the reaction 2 Glycine(s)→Glycylglycine(s) + H2O(1) Calculate A,H, A,S, A,Ssurr and A,Stotal at T = 298.15 K. Use R = 8.315 J K- mol1. Useful thermodynamic data are given below. Do not use scientific notation. Pay attention to the units and magnitude of the answers given Note: All the enthalpies of formation have negative signs. Table 1 Glycine(s) Glycylglycine(s) H2O(1) A¢H° (kJ mol 4) 537 -746 -286 Sm (J K1 mol1) 104 190 70

The amino acid glycine dimerizes to form the dipeptide glycylglycine according to the reaction 2 Glycine(s)→Glycylglycine(s) + H2O(1) Calculate A,H, A,S, A,Ssurr and A,Stotal at T = 298.15 K. Use R = 8.315 J K- mol1. Useful thermodynamic data are given below. Do not use scientific notation. Pay attention to the units and magnitude of the answers given Note: All the enthalpies of formation have negative signs. Table 1 Glycine(s) Glycylglycine(s) H2O(1) A¢H° (kJ mol 4) 537 -746 -286 Sm (J K1 mol1) 104 190 70

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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For the reaction Cr(C6H6)2 (s) --> Cr(s) + 2 C6H6 (g), the reaction internal energy change at 1 atm and 538 K is DUrxno(T = 538K) = 8.0 kJ/mol. (a) Estimate the molar enthalpy of reaction at 1 atm and 538 K for the above reaction. (b) If the standard molar enthalpy of formation for C6H6 at 1 atm and 538 K is about DHfo (C6H6 (g)) = 84 kJ/mol, estimate the standard enthalpy of formation of Cr(C6H6)2 (s) at 1 atm and 538 K.
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 26.0 °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. N₂(g) + 3H₂(g) → 2NH₂(g) P₁(s) + 20HF (g) 4PF, (g) + 10H₂(g) ΔΗ = -92. kJ AS = AG = | KJ -294. ΔΗ Which is spontaneous? this reaction the reverse reaction neither AS = = - 1005. kJ…
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