Acetone, CH3 COCH3 , is a fragrant liquid that is used as asolvent for lacquers, paint removers, and nail polish remover. Itburns in oxygen to give carbon dioxide and water:CH; COCH, (1) + 402(9) → 300, (9) + 3H,0(1)If the standard free-energy change for this reaction is –1739.0kJ/mol, what is the standard free energy of formation of acetone?Substance AG; (kJ/mol)O2 (9)Co2(9)-394.4H20(1)-237.1Standard free energy =|kJ/mol

Welcome to bartleby ! We have to calculate standard free energy of formation of acetone

Acctone, OCH, Is a fragrant liquid solvent for lacquers, paint removers, and nail polish remover. It burns in oxygen to give carbon dioxide and water: nat is as a CH, COCH, (1) + 40,(9) → 3CO, (9) + 3H3O(1) If the standard free-energy change for this reaction is -1739.0 kJ/mol, what is the standard free energy of formation of acetone? Substance AG? (kJ/mol) 02(9) Co (9) -394.4 H20(1) -237.1 Standard free energy = kJ/mol

Acctone, OCH, Is a fragrant liquid solvent for lacquers, paint removers, and nail polish remover. It burns in oxygen to give carbon dioxide and water: nat is as a CH, COCH, (1) + 40,(9) → 3CO, (9) + 3H3O(1) If the standard free-energy change for this reaction is -1739.0 kJ/mol, what is the standard free energy of formation of acetone? Substance AG? (kJ/mol) 02(9) Co (9) -394.4 H20(1) -237.1 Standard free energy = kJ/mol

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

365 Calculate the standard free energy change for the following reaction: = Drive 2XO(s)+O2(g)→ 2XO2(s) AG 298(XO2) = -219.1 AG 298 (XO) = -150 Use 4 significant figures in your answer. Do not include the unit.
4. The standard free energy (AG°) for a reaction at 298 K is -104 J / mol. What is Keq for this reaction?
33. Use the standard free energy of formation data in Appendix G to determine the free energy change for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions. MnO2 (s) ⟶ Mn(s) + O2 (g) H2 (g) + Br2 (l) ⟶ 2HBr(g) Cu(s) + S(g) ⟶ CuS(s) 2LiOH(s) + CO2 (g) ⟶ Li2CO3 (s) + H2O(g) CH4 (g) + O2 (g) ⟶ C(s, graphite) + 2H2O(g) CS2 (g) + 3Cl2 (g) ⟶ CCl4(g) + S2Cl2 (g)
Acetone, CH3 OCOCH3, is a fragrant liquid that is used as a solvent for lacquers, paint removers, and nail polish remover. It burns in oxygen to give carbon dioxide and water CH: COCH, (1) + 402 (9) → 3CO2(9) + 3H2O(1) If the standard free-energy change for this reaction is –1739.0 kJ/mol, what is the standard free energy of formation of acetone? Substance AG; (kJ/mol) O2 (9) Co (9) НаО() -394.4 -237.1 Standard free energy= kJ/mol
[Review Topics] [References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.21x1012 for the following reaction. CO(g) + Cl2(g)- COC12(g) Based on this value of Keg AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.65 moles of CO(g) at standard conditions at 298K. AG rxn kJ
Calculate standard free energy change using AGf values. Consider the reaction 2NH3(g) + 3N₂O(g)4N₂(g) + 3H₂O(g) Use standard free energies of formation to calculate the standard free energy change for this reaction at 25°C. kJ/mol AG° = rxn
A student determines the value of the equilibrium constant to be 1.29×1064 for the following reaction.2Na(s) + 2H2O(l)2NaOH(aq) + H2(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) ________ than zero.Calculate the free energy change for the reaction of 1.63 moles of Na(s) at standard conditions at 298K. G°rxn = _______ kJ
a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) = -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l) b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?
For the reaction CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) ΔΗ° - 206.1 kJ and AS = - 214.7 J/K The standard free energy change for the reaction of 1.67 moles of CO(g) at 253 K, 1 atm would be This reaction is favored under standard conditions at 253 K. Assume that AH° and AS° are independent of temperature. == kJ.
Calculate AG° at 298 K for the reaction CS, (1) + 30,(g) –→ CO,(g) + 2 SO,(g) based on these reactions. C(s) + 0,(g) Co,(g) AG° = -397.28 kJ/mol S(s) + 0,(g) → so,(g) AG° = -300.19 kJ/mol C(s) +2 S(s) → CS,(1) Cs,(1) AG° = +62.37 kJ/mol AG° = kJ/mol
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(8) + 3H2(g) → 2NH3(g) AG° at 298 K for this reaction is -33.3 kJ/mol. The value of AG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is O -1.8 O -104.5 O-3.86 x 103 O-7.25 x 10 -40.5
Calculate AG° at 298 K for the reaction CS,1) + 3 0,(g) → CO,(g) + 2 SO,(g) CO,(g) + 2 SO, (g) > based on these reactions. C(s) + O,(g) → CO, (g) AG° = -397.28 kJ/mol S(s) + 0,(g) –→ SO, (g) AG° = -300.19 kJ/mol C(s) + 2 S(s) · CS,(1) AG° = +62.37 kJ/mol AG° = kJ/mol