Oxygen difluoride reacts with water vapor to produce 318 kJ of heat by the followingequation:OF2 (g) + H;0 (g) → 2 HF (g) + O2 (g)Calculate AH of OF in kJ/mol for the reaction below. Look up the values for AH: below.Table 6.3 Standard Enthalpies of Formation of SomeInorganic Substances at 25°CSubstanceAH¡ (kJ/mol)SubstanceAH¡ (kJ/mol)Ag(s)H,O,(/)- 187.6AgCl(s)- 127.04Hg(/)Al(s)(s)Al;O;(s)- 1669.8HI(g)25.94Br2()HBr(g)C(graphite)Mg(s)MgO(s)M9CO;(s)-36.2-601.8-1112.9C(diamond)1.90N2(g)NH,(g)NO(g)NO,(g)N,0.(9)N,0(g)O(g)0,(g)0;(g)COlg)CO,(g)-110.5-46.3-393.590.4Ca(s)33.85CaO(s)-635.69.66CaCo;(s)Cl,(9)HCIG)Cu(s)-1206.981.56249.4-92.3142.2CuO(s)-155.2S(rhombic)F,(9)HF(g)H(g)H2(g)S(monoclinic)0.30-268.61SO-(g)-296.1218.2so:(g)-395.2H,S(g)-20.15H,O(g)-241.8Zno(s)-347.98H,O(1)-285.8

Answered: Image /qna-images/answer/15ae9dbf-3b61-419c-bd23-36563be07ec6.jpg

en difluoride reacts with water vapor to produce 318 kl of heat by the following tion: g) + H;O (g) → 2 HF (g) + O2 (g) late AH: of OF; in kl/mol for the reaction below. Look up the values for AHe below. e 6.3 Standard Enthalpies of Formation of Some janic Substances at 25°C

en difluoride reacts with water vapor to produce 318 kl of heat by the following tion: g) + H;O (g) → 2 HF (g) + O2 (g) late AH: of OF; in kl/mol for the reaction below. Look up the values for AHe below. e 6.3 Standard Enthalpies of Formation of Some janic Substances at 25°C

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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Calculate enthalpy changes for the following: a. 0.089 g of sulfur (rhombic) burns, forming SO₂(g) ( ▲ƒH˚ for SO₂ (g) = - 296.84 kJ/mol) Enthalpy change b. 0.28 mol of d. = HgO(s) decomposes to Hg(l) and O₂(g) ( c. 2.20 g of Af HⓇ for HgO = -90.83 kJ/mol) Enthalpy change = NH3(g) is formed from N₂(g) and excess H₂(g) ( Af HⓇ for NH3 = -45.90 kJ/mol) Enthalpy change = KJ = kJ kJ [Review Topics] A 1.19 x 10-2 mol of carbon is oxidized to CO2(g) ( AfH for CO2 = -393.509 kJ/mol) Enthalpy change kJ [References]
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the first picture is the question and the second picture is the expected answer (please apply thermochemistry and their formula)
Calculating a Heat of Formation Using Hess’s LawAs discussed in lecture, the simplest and most general method for determining theenergy change during a chemical reaction involves the use of the heat of formation (ΔHf) for thereactants and products. Conceptually, the heat of formation is the heat released or absorbedwhen one mole of the substance is created from its elements at standard temperature andpressure. In some cases, this number can be measured directly (i.e. by reacting the elements at1.0 atm and 25oC and observing the heat given off). In most cases, however, this is notpractical. For instance, the direct calculation of the ΔHf for magnesium oxide would involveburning magnesium metal in a pure oxygen atmosphere; while such a reaction is certainlypossible, it would difficult to measure changes in temperature since the reaction is highlyexothermic and the product is a solid powder. Instead, in this lab you will be calculating the ΔHf for magnesium oxide by determiningthe heat of…
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Use the molar bond enthalpy data in the table to estimate Average molar bond enthalpies. (Hpond) the value of AHn for the equation Bond kJ - mol-1 Bond kJ - mol-1 CCI, (g) + 2F, (g) CF,(g) + 2Cl, (g) O-H 464 C=N 890 The bonding in the molecules is shown. 0-0 142 N-H 390 С-О 351 N-N 159 CICI O=0 502 N=N 418 + C CI C=0 730 N=N 945 F-F С-С 347 F-F 155 C=C 615 Cl-CI 243 C=C 811 Br-Br 192 С-Н 414 Н-Н 435 C-F 439 Н-F 565 C-CI 331 Н-С 431 C-Br 276 Н-Br 368 C-N 293 H-S 364 C=N 615 S-S 225
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