Average Bond Dissociation Energies at 298 K Bond Energy, kJ mol1 H-H 432 O=0 495 H-O 467 The tables above contain information for determining thermodynamic properties of the reaction below. 2H,(g) + 02(8) - 2H,O(g) (a) Calculate the AH° for the reaction above, using the table of average bond dissociation energy. (b) Use the table below to calculate the entropy for the formation of water. 2H, + 02 - 2H,O Substance S°(J/mol· K) H2 131.0 H20 69.91 O2 205.0 (c) Calculate the value of AG°298K for the synthesis of water.

Average Bond Dissociation Energies at 298 K Bond Energy, kJ mol1 H-H 432 O=0 495 H-O 467 The tables above contain information for determining thermodynamic properties of the reaction below. 2H,(g) + 02(8) - 2H,O(g) (a) Calculate the AH° for the reaction above, using the table of average bond dissociation energy. (b) Use the table below to calculate the entropy for the formation of water. 2H, + 02 - 2H,O Substance S°(J/mol· K) H2 131.0 H20 69.91 O2 205.0 (c) Calculate the value of AG°298K for the synthesis of water.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 68E: Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following...

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Using a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.
Estimate ΔrH° for forming 2 mol ammonia from molecular nitrogen and molecular hydrogen. Is this reaction exothermic or endothermic?
Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: Use tabulated values of bond energies (Table 3-3) to estimate E for this reaction.
26. From the relevant bond energies given below, find the approximate AH ( in kilojoules) for the industrial synthesis of chloroform (CHC3) in a reaction of methane ( CH4) with chlorine gas (Cl2). Is the reaction exothermic or endothermic? (4 CH4 (g) + 3Cl+ (g) — СHC1(g) +3 HсI (9) Bond Dissociation Energies ( Bond Enthalpies) in kJ/mol at 298K for Selected Bonds Bond Bond Energy (kJ/mol) С —Н 410 kJ/mol Cl-Cl 243kJ/mol C-Cl 330kJ/mol H-C1 432 kJ/mol
A.) What is the heat of reaction, ΔH°? CO2(g) + H2O(l) à H2CO3(aq) –20.2 kJ mol–1 –1379 kJ mol–1 –592 kJ mol–1 B.) What is the average bond energy in CO2? CO2(g) ΔH°f, = –393.5 kJ mol–1 CO(g) ΔH°f, = –110.5 kJ mol–1 C(g) ΔH°f, = +715 kJ mol–1 CO32–(aq) ΔH°f, = –676.3 kJ mol–1 O(g) ΔH°f, = +249.0 kJ mol–1 207 kJ mol–1 1607 kJ mol–1 804 kJ mol–1
Calculate the enthalpy change for the reaction below. Compound Нeat Value -> 3NO(s) ,0,ls) AH +174 k (belONH2 -(aloH (2Fo+ ('N AH -183 k AH =-128 k) 2NO(g) O-137 kJ O-128 kJ -174kJ 270KJ
[References] Calculate AH for the reaction: 2NH3 (g) + O2(g) → N2H4 (1) + H2O(1) given the following data: 2NH3 (g) + 3N2O(g) → 4N2(g) + 3H2O(1) AH =–1010. kJ N2O(9) + ЗH2(9) — N;Ha (1) + Hа0(1) ДН %3D — 317 kJ N2H4 (1) + O2 (9) → N2(g)+2H20(1) ΔΗ--623 k.J На (9) + О2(9) — Н,0(1) AH = -286 kJ ΔΗ- kJ Submit Answer Try Another Version 3 item attempts remaining
22.) Estimate the enthalpy of reaction of the given reaction using the following data: C3H6 (g) + Hz (g) → C3H8 (g) Bond С-Н H-H С-С C=C Bond Energy (kJ/mol) 614 413 432 347 a.) -220 kJ/mol b.) -286 kJ/mol c.) -127 kJ/mol d.) 286 kJ/mol 23.) Calculate the standard enthalpy of combustion of aniline from the following standard enthalpies of formations. C6H5NH2 (1) + 31/4 02 (g) –→ 6 CO2 (g) + ½ N2 (g) + 7/2 H2O (1) H20 (1) CO2 (g) -393.51 C6H5NH2 (1) -285.83 A:H° (kJ/mol) +31.1 c.) -3123 kJ/mol d.) -4107 kJ/mol a.) -3393 kJ/mol b.) -3330 kJ/mol
Calculate the enthalpy of formation, AHF° in kJ, of hydrogen peroxide, H2O2(g), from the relevant bond energy data. Bond Bond energy Bond Bond energy O-H 463 kJ mol-1 H-H 436 kJ mol-1 O=O 498 kJ mol-1 O-O 138 kJ mol-1 -285 +285 +130 -380 -130
3. Calculate the reaction enthalpy of this reaclion Under Stondard conditions. 2C, Hu (G) + 70, lg) ->4C0, 4) + (6 H,O ) 70, (g) –> 4CO,(G) +(6 HqO() kJ
Another reagent that can be used to convert carboxylic acids into acid chlorides is phosphorus trichloride (PCI3), as shown in the scheme below. :0: :0: :ö: PCI2 + -PCI2 H. H :O: + НОРCI2 The mechanism, for the reaction, is shown above but the curved arrows and the formal charges, on the respective atoms, have been omitted. (a) Draw the missing curved arrows for each step (b) Supply any missing formal charges
Given the following enthalpy change values for the reactions below: A + B -->2C; ?rH = 419 kJ mol-1 C + 2D--> E+F; ?rH = 70.1 kJ mol-¹ ½E+G-->H; ?rH = -33.1 kJ mol-¹ Calculate ?rH for the following reaction (in kJ mol-¹) using Hess's Law: A + B + 4D + 4G -->4H + 2F