One method for making ethanol, C₂H5OH, involves the gas-phase hydration of ethylene, C₂H4: Estimate AH for this reaction from the given average bond dissociation energies. Set your reaction up as follows: C₂H₂ + H₂O-C₂H₂OH Bond D, kJ/mol C=C 615 410 350 C-H C-C C-0 O-H -35 350 460 Your answer is correct. Part 2 of 2 2 16 % X ala 19 What is the amount of energy, in k3, changed upon hydration of 63.1 10 11.9 %

One method for making ethanol, C₂H5OH, involves the gas-phase hydration of ethylene, C₂H4: Estimate AH for this reaction from the given average bond dissociation energies. Set your reaction up as follows: C₂H₂ + H₂O-C₂H₂OH Bond D, kJ/mol C=C 615 410 350 C-H C-C C-0 O-H -35 350 460 Your answer is correct. Part 2 of 2 2 16 % X ala 19 What is the amount of energy, in k3, changed upon hydration of 63.1 10 11.9 %

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter8: Bonding And Molecular Structure

Section8.9: Bond Properties: Order, Length, And Dissociation Enthalpy

Problem 3RC: 3. Use bond dissociation enthalpies to estimate the enthalpy change for the decomposition of...

See similar textbooks

Similar questions

3. Use bond dissociation enthalpies to estimate the enthalpy change for the decomposition of hydrogen peroxide. 2 H2O2(g) → 2 H2O(g) + O2(g) +352 kJ/mol-rxn −206 kJ/mol-rxn +1037 kJ/mol-rxn −2204 kJ/mol-rxn
Given that H2 (g) + F2(g) 2 HF(g) AHgxn = -546.6 kJ 2 H2(g)+02(g) 2 H2O(1) ΔΗ -571.6 kJ rxn calculate the value of AH for +4 HF(g) 02(g) 2F, (g) +2 H2O() kJ ΔΗΗ www.tinacio
Given the following enthalpy change values for the reactions below: A + 2B – C; A,H = 350.1 kJ mol-1 E + F - 2C + D;A,H = 476.2 kJ mol-1 ½ E - G + 2B ; A;H = -229.6 kJ mol-1 Calculate A,H for the following reaction (in kJ mol-1) using Hess's Law: 2A + D - F + 2G
Calculate AH, in kJ, for the following reaction using the bond energies given. H. H3C-C-CH3 (g) H2 (g) H3C-C-CH3 (8) + Bond: С-O Н-Н С-Н О-Н С-С С-Он ВЕ: 745 436 414 464 347 351 (kJ/mol)
Use the tables below to determine the enthalpy of reaction (in kJ) for the following balanced chemical equation: Table T16-5-1. BDES, average single bond dissociation energies (in kJ/mol) I Br CI s P si F ONC H 299 366 431 368 322 323 568 463 391 413 436 220 276 328 259 264 301 453 358 276 348 N 159 243 200 200 335 272 176 193 234 234 203 364 340 368 190 146 F 277 237 193 327 490 582 157 Si 234 310 464 226 226 184 264 319 209 218 253 266 CI 208 218 242 Br 175 193 I 151 Multiple Bonds (BDE in kJ/mol) Bond BDE Bond BDE N=N 418 C=C 620 NEN 941 C=C 815 C=N 615 C=0 745 CEN 891 C=O 1072 N=O 607 O=0 499 Reaction: C2H4 + l2 -> C2H412 P.
Comprandd waith carbon. Carbon double bonds, such as ethylene C₂Hy add hydrogen in a reaction called hydrogenation. Calculate the enthalpy, Change for this reaction, lesing the Combursion data and Hell's low C₂ Hut H2 - C₂H6 (i) 3C2 Hut 90 →600₂ + 6H₂0 DH = 1401kJ (ii) 2 C₂H6+ 7 0₂ → 4 CO₂ + 6H₂₂0DH = 3 sook] (1₁) 24₂ +10₂ > 21120 DH= 572 KJ
Use the AH°f and AH°, rxn SO 2(8) AH'f (kJ/mol) -297 1) -792 kJ/mol 2) -248 kJ/mol 3) -495 kJ/mol 4) -578 kJ/mol 5) -396 kJ/mol information provided to calculate Hºf for SO3(g): 2SO2(8) +02(g) → 25O3(g) AH xn-198 kJ
4.) HX is used as a reagent in the reaction below. NH2 он + HX + :NEN: VW llat 1ufnctiofUrgrou What is the l'1 Sur ucOISIOn With tht taulc UI Ka valucs i the van Consider the following thermodynamic data for the reaction shown above. NH2 он + HX + NEN: + AH°r (kJ/mol) -386 260.1 30.00 -393.5 S° (J/mol K) 166 146.0 191.3 191.5 213.8 D. Based on the reaction equation given above, does entropy increase or decrease in this reaction? E. Justify your answer to (D) with a calculation. Does your calculation agree with your prediction? F. Is this reaction thermodynamically favorable at 25°C? Justify with a calculation. +
Given the following data: C2H2(g) + 5/2 O2(g) --> 2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) + O2(g) --> CO2(g) ΔH= -394kJ H2(g) + 1/2O2(g) --> H2O(l) ΔH= -286kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) --> C2H2(g)
Match each of the following with its correct answer If AH°, of H,O, is -285.8 KJ/mol and AH° of H,0 is -241.8 KJ/mol, then the AH°, of evaporation of H,O in ( KJ/mol) : 2 (L) (g) Chooser Choose.. -44 -413.9 Using the following information below, calculate AHº, for Pbo in kJ/mol. +44 -108.7 -210 -151.6 PbO + CO (s) (g) Pb + CO (s), 2(g), ΔΗΟ = 131.4 kJ/mol- 1) Molecules AHO Choose... CO 6), -110.5 CO 2(g) -393.5 Given the following thermochemical equation: 16CO, + 18 H O 2(g) AH° = -11020 2CH,8) + 25 0,(g) 18(1) kJ/mol If AH°, [CO,l] = -393.5 kJ/mol and AH°. [H,o ] = -285.8kJ/mol, calculate the standard enthalpy of formation of octane ( C H) 2(g) %3D Choose...v in kJ/mol wwwwt
7. Calculate AH for 2NO(g) + O2(g) - Using the following information: 2NO2 (g) N₂O4(g) 2NO(g) + O2(g) 2NO2(g) N2O4(g), AH = +57.9 kJ ΔΗ= -113.1 kJ
Using the table of average bond energies below, the AH for the reaction is kJ. H H | | H-C=C-H(g) + 2HI(g) → I-C-C-I(g) H H Bond C=C C-C H-I C-I C-H AH (kJ/mol) 839 348 299 240 413 63 -63 160 -160 -217 217