Using the values you got from the textbook for enthalpy and entropy, calculate AGO (kJ mol-¹) at 298K for the reaction: C₂H5OH (1) + O2(g) --> CO2(g) + H₂O (1) Make sure to balance this reaction.

Using the values you got from the textbook for enthalpy and entropy, calculate AGO (kJ mol-¹) at 298K for the reaction: C₂H5OH (1) + O2(g) --> CO2(g) + H₂O (1) Make sure to balance this reaction.

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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Can u help me work this problem. I didn’t write notes in how I got the correct answer (2nd option).
0/5 Nerbs 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 85.0 °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. do AH = -2220. kJ J AS = -6189 K C,H, (g) + 50, (g) 3Co, (g) + 4H,0(1) AG = KJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = -50. kJ 0- AS =…
(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.
Determine the enthalpy change for the reaction: S03 (g) + H20(g) → H2SO4 (1) Given: i. H2SO4 (1) → H2SG) + 2 02 (9); ΔΗ 1236.4 kJ %3D ii. SO3 + H20(1) H2S(9) + 2 02 (9); ΔΗ1086.7 ky (g) iii. H20(1) → H20(g); AH° = 40.7 kJ
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2) Consider the situation: 2CH,O, + 30) 4H,0 + e) AH --1453.0 kJ 2 CO, ΔΗ, 2(8) Showing your work, how much heat would this represent for the combustion of 12.74 mol of liquid methanol (CH4O0)? Answer to 1 decimal place. [K3] the follouing processes: (2 marks each) [C4]
Q5 (i) Draw an energy cycle and use the Standard Enthalpies of combustion values in the table below to calculate the 10(g)* enthalpy of formation of butane, C4H₁09). Explain how the value obtained here might be different from the value obtained using calorimetry. (Show working as this question will be assessed using grade descriptors 1, 3 & 7) Substance Enthalpy of Combustion/kJ mol-¹ -394 -286 -2876 C(s) H2(g) CH10(9)
Use the given standard enthalpies of formation to calculate AH° for the following reaction (SHOW CALCULATIONS) 2 Fe304(s) + C02(g) → 3 Fe2O3(s) + CO(g) Species AH°†, kJ/mol Fe2O3 (s) -824.2 FezO4 (s) -1118.4 CO (g) CO2 (8) -110.5 -393.5
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.