A;H°(CO2, g) = -393.5 kJ mol"; A;H°(H2O, 1) = -294.6 kJ mol" S°(CH;OH, I) = 126.8 J mol K'; s°(O2, g) = 205.0 J mol' K'; s°(CO2, g) = 213.6 J mol" K'; AH°(H2O, 1) = 76.0 J mol' K Let's consider the reaction of combustion of methanol at 298 K with a standard molar enthalpy of reaction A,H° = -725.2 kJ mol!: 3 CH,OH) CO2 (9) + 2 H,Om 2 (g) 2 Calculate the standard molar enthalpy of formation of methanol at 298 K.

A;H°(CO2, g) = -393.5 kJ mol"; A;H°(H2O, 1) = -294.6 kJ mol" S°(CH;OH, I) = 126.8 J mol K'; s°(O2, g) = 205.0 J mol' K'; s°(CO2, g) = 213.6 J mol" K'; AH°(H2O, 1) = 76.0 J mol' K Let's consider the reaction of combustion of methanol at 298 K with a standard molar enthalpy of reaction A,H° = -725.2 kJ mol!: 3 CH,OH) CO2 (9) + 2 H,Om 2 (g) 2 Calculate the standard molar enthalpy of formation of methanol at 298 K.

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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1. From the following enthalpies of reaction: • 2HFe) CFA@) F2tet AH = -537 kJ Hate + 2 F2te) 2 H2(8) C. AH = -680 kJ 4. AH = -52.3 kJ 4- 2C, and HF(e) Calculate the AH for the reaction of C,Hate) with F2te) to make CF4te)
Calculate the ΔH for the target reaction below using the three equations listed. Rewrite the three equations so that they add to give the reaction below Target: CS2(l) + 3O2(g) --> CO2(g) + 2SO2(g) ΔH = ? C(s) + O2(g) --> CO2(g) ΔH = -393.5 kJ S(s) + O2(g) --> SO2(g) ΔH = -296.8 kJ C(s) + 2S(s) --> CS2(l) ΔH = 87.9 kJ Enter ΔH for the top equation in Kj. (Your answer should have one digit after the decimal)
Calculate the AH°rxn for the combustion of methane using the given AH°r. CH4 (g) + 202 (g) 2H20 (1) + CO2{g) AH°t, methane(g) = -74.60 kJ/mol AH°f, water(l) = -285.8 kJ/mol AH°t, carbon dioxide(g) = -393.5 kJ/mol 890.5 kJ/mol -890.5 kJ/mol -1.04 x 103 kJ/mol
MISSED THIS? Read Section 19.8 (Pages 871 - 877); Watch IWE 19.6. Liquid methanol burns in oxygen to form gaseous carbon dioxide and gaseous water. Substance H° (kJ/mol) S° (J/(mol. K)) CH3OH (1) -238.6 126.8 O2 (g) 0 CO₂ (g) -393.5 CO2(aq) -413.8 H₂O(g) -241.8 H₂O(1) -187.8 205.2 213.8 117.6 188.8 70.0 stan 1 Periodic Liquid methanol (CH3OH(1)) burns in oxygen (O₂ (g)) to form gaseous carbon dioxide (CO2 (g)) and gaseous water (H₂O(g)), which is represented by the following balanced equation: 2CH3OH(1) +302(g) → 2CO2 (g) + 4H₂O(g) The balanced chemical equation is neeed to calculate the standard enthalpy change for a reaction (AH) the standard entropy change for a reaction (AS) from the standard enthalpies of formation and standard molar entropies, respectively. Part B Calculate AHxn at 25 °C. Express your answer in kilojoules to three significant figures. AH = VE ΑΣΦ C ? kJ
a. 0.045 g of sulfur (rhombic) burns, forming SO2 (g) ( A¡H° for SO2 (g) = - 296.84 kJ/mol) Enthalpy change = kJ %3D b. 0.36 mol of HgO(s) decomposes to Hg(l) and O2 (g) ( A;H° for HgO = -90.83 kJ/mol) %3D Enthalpy change = kJ c. 2.85 g of NH3 (g) is formed from N2 (g) and excess H2 (g) ( AƒH° for NH3 = -45.90 kJ/mol) %3! Enthalpy change = kJ %3D d. 1.06 x 10-2 mol of carbon is oxidized to CO2 (g) ( AƒH° for CO2 = -393.509 kJ/mol) Enthalpy change = kJ
2) Determine the Sign of Ds for each of the following reactions a) CH₂(g) + 20₂(g) → 2H₂0 (1) + CO₂(g) b) 2 C 2 H 6 (g) + 70₂(g) → 6H₂0 (1) +4 (0₂ (9) c) Ca(OH)₂ (s) → (90) + H₂0 (1)
Hydrogenation reactions, which involve the addition of H2 to a molecule, are widely used in industry to transform one compound into another. For example, 2- butene (C4H3) is converted to butane (C4H10) through the addition of H2. H H H H C=C -H(g) + H2(g) H. H H H H C- C -H (g) H Use the bond dissociation enthalpies in the table below to estimate the enthalpy change for this hydrogenation reaction. Bond Dissociation enthalpy, kJ/mol C=C 610 H-H 436 C-Ç 346 C-H 413 Enthalpy change = | kJ
how do you know the state (s,l,g,aq) of a compound?
Which of the following would you expect to have the most negative ∆S? a) I b) II c) III d) IV
Given the table below and the gaseous and solid phases CO₂ at 1 atm and 298K, CO2(g) CO2 (s) -393.5 -427.4 213.8 AH°; (in 1/1) ΔΙ J So in mol - K What is the AH of the CO2 sublimation? ?
Calculate the AS° for the given reaction. + Cazs(PO4)2(0) 2+ Ca (ag) + PO43 (ag) molar ratio of the balanced chemical equation: Caz(PO4)2(0) 2+ Ca (ag) PO,3- Substance (at -53.1 -222.0 S° ( J/mol · K) 241.0 ES" (product) %3D ES (reac tan t) AS°, rxn