oxygenPhotosynthesis in plants converts carbon dioxide and water into glucose (C,H,O) andaccording to the equation below.6CO₂(g) + 6H₂O() - CH₂O() + 60₂(g)SubstanceCO(g)H₂O(1)C₂H₁₂O(s)O(g)AHi(kJ/mol)-393.5-285.8-1273.30SᵒJ/mol K)213.669.9209.2205.0Calculate the AH, AS, and AG. Is the reaction spontaneous at standard conditions?

Answered: Image /qna-images/answer/d2f12420-1a41-4a99-89d8-4841ab45bf2a.jpg

Photosynthesis in plants converts carbon dioxide and water into glucose (E₂ according to the equation below. 600,(g) + 6H₂O(0) CHO,G) + 60,(g) Substance CO(g) H₂O( C₂H₁₂O₂(s) Olg) AH(kJ/mol) -393.5 -285.8 -1273.3 0 SU/mol-K) 213.6 69.9 209.2 205.0 Calculate the AH, AS, and AG. Is the reaction spontaneous at standard conditions? and oxyge

Photosynthesis in plants converts carbon dioxide and water into glucose (E₂ according to the equation below. 600,(g) + 6H₂O(0) CHO,G) + 60,(g) Substance CO(g) H₂O( C₂H₁₂O₂(s) Olg) AH(kJ/mol) -393.5 -285.8 -1273.3 0 SU/mol-K) 213.6 69.9 209.2 205.0 Calculate the AH, AS, and AG. Is the reaction spontaneous at standard conditions? and oxyge

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.79QE

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Prepare a table identifying several energy transitions that take place during the typical operation of an automobile.
Some automobiles and buses have been equipped to bum propane (C3H8). Compare the amounts of energy that can be obtained per gram of C3H8(g) and per gram of gasoline, assuming that gasoline is pure octane, C8H18(l). (See Example 7-11.) Look up the boiling point of propane. What disadvantages are there to using propane instead of gasoline as a fuel?
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Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
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[4] rxn 2. Given the following information, calculate AH for the reaction. 2C3Hs(g) +1002(g) → 6CO2(g) + 8H₂O(1) | AH¦ (C³H8(g)) = -103.9 kJ/mol; AH; (CO2(g)) = -393.5 kJ/mol, AH; (H₂O(1) = -285.5 kJ/mol
Given the following data: 4C(s) + 3H2(g) + 1/2O2(g) → HCOC(CH2)(CH3)(l) ΔH°=-139.0 kJ CH3CH2OH(l) + 1/2O2(g) → CH3CHO(l) + H2O(l) ΔH°=-204.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ Calculate ΔH° for the reaction:2CH3CHO(l) → HCOC(CH2)(CH3)(l) + H2O(l)
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