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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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
Given the following information: C(s) + 02(g) ---> C02(g) delta H= -393.5 kJ H2(g) + 1/2 02(g)--> H20(I) delta H= -285.8 kJ C2H2(g) + 5/2 02(g)--> 2 C02(g) + H20(I) delta H= -1299.8 kJ find the enthalpy change for: 2 C(s) + H2(g)--> C2H2(g) a.) -454.0 kJ b.) -227.0 kJ c.) 0.0 kJ d.) 227.0 kJ e.) 454.0 kJ
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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
Use the AHºf information provided to calculate AH°rxn for the following: CH4(g) + 2O2(g) → CO₂(g) + 2H₂O(l) AHºf CH4(8) O₂(g) CO₂(g) H₂O(l) (kJ/mol) -74.8 0 -393.5 -285.8 AH°rxn = ?
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Use the AH° information provided to calculate AH°rxn for the following: SO,C2(g) + 2 H20(1) → 2 HCl(g) + H2SO4() AH°rxn = ? AH°¡ (kJ/mol) SO,Cl2(g) -364 H2O(I) -286 HCl(g) -92 H2SO4() -814 Select one: O -62 kJ/mol O 800. kJ/mol 161 kJ/mol O -256 kJ/mol
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Given the AH°¢ and S° values below, what is the boiling point of Br2? So AH°f (kJ/mol) (J/ mol K) Br2(1) -239 127 Br2(g) -201 240 O 273 K 336 K 373 K 1199 K O 2.1 K
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