The glucose fermentation reaction is C6H12O6 (aq) → 2 C₂H5OH (aq) + 2 CO₂ (g), finding the summarizedthermodynamic data in the following table:AHO (kJ mol-¹)AGO (kJ mol-¹)C6H12O6 (aq) C₂H5OH (aq)-1261,5-914,5-277,7-174,8CO2 (g)-393,5-394,4What is the free energy AG of this reaction at 25°C and justify if it is a spontaneous process. Indicate theentropy change AS at the same temperature.

In the above question fermentation of glucose reaction is given C6H12O6 (aq). ==> 2C2H5OH…

The glucose fermentation reaction is C6H12O6 (aq) → 2 C₂H5OH (aq) + 2 CO₂ (g), finding the summarized thermodynamic data in the following table: AHO (kJ mol-¹) AGO (kJ mol-¹) C6H12O6 (aq) C₂H5OH (aq)| CO2 (g) -1261,5 -277,7 -393,5 -914,5 -174,8 -394,4 What is the free energy AG of this reaction at 25°C and justify if it is a spontaneous process. Indicate the entropy change AS at the same temperature.

The glucose fermentation reaction is C6H12O6 (aq) → 2 C₂H5OH (aq) + 2 CO₂ (g), finding the summarized thermodynamic data in the following table: AHO (kJ mol-¹) AGO (kJ mol-¹) C6H12O6 (aq) C₂H5OH (aq)| CO2 (g) -1261,5 -277,7 -393,5 -914,5 -174,8 -394,4 What is the free energy AG of this reaction at 25°C and justify if it is a spontaneous process. Indicate the entropy change AS at the same temperature.

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...

See similar textbooks

Similar questions

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.
Gaseous SO2Cl2 reacts with liquid water to form hydrogen chloride gas and liquid sulfuric acid. Using data tabulated in Appendix G of your text, calculate the enthalpy change, in units of kJ/mol, for the formation of 2 mol of liquid sulfuric acid.
Consider the following reaction: 3C(s) + 3H2(g) → C3H6(g); AG°= 60.0 kJ and AS° =-256.7 J/K at 298 K What is the equilibrium constant and AH° at 298 K for this reaction? Express AH° in kJ and use 3 significant figures for both answers. AH° = kJ and Keq x 10
(Q70) Using the tabulated values from the text (located in Appendix G, beginning at p. 1211) calculate (and report in kJ) the standard Gibbs free energy (AG°rxn) for the net reaction that occurs during photosynthesis: 6 H2O (1) + 6 CO2 (g) --> C6H12O6 (s) + 6 O2 (g). The AG°; for glucose (C6H1206) is -1273.3 kJ/mol.
Combustion of glucose (CH,0 is the main source of energy for animal cells: CH,0,) + 60,(g) -- 6CO,(g) + 6H,o) AG,(37 C) =- 2872. kI One of the most important uses to which this energy is put is the assembly of proteins out of amino acid building blocks. The Gibbs free energy of formation of one peptide bond, joining one amino acid to another, is 21 k/mol. Suppose some cells are assembling a certain protein made of 84 amino acids. (Note that the number of peptide bonds in the protein will be one less than the number of amino acids.) Calculate the minimum mass of glucose that must be burned to assemble 400. umol of this protein. Round your answer to 2 significant digits.
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 136.0 °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. AH = -2220, kJ J AS = -5426. K C,H, (g) + 50,(8) → 3C0,g) + 4H,0() AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither ΔΗ 50. ky AS = 6CI, (g) + 2Fe,0.(s)…