**Enthalpy Change Calculation for Benzene Reaction****Objective:**Calculate the change in enthalpy, ΔH, for the combustion of benzene (C₆H₆) using bond enthalpies.**Reaction:**C₆H₆ (l) + \( \frac{15}{2} \) O₂ (g) → 6 CO₂ (g) + 3 H₂O (g)**Bond Enthalpies:**- C-H: 413 kJ/mol- C-C: 348 kJ/mol- C=C: 614 kJ/mol- O=O: 498 kJ/mol- C=O: 805 kJ/mol- O-H: 464 kJ/mol- C-O: 360 kJ/molBenzene (C₆H₆) is a ringed structure depicted in the diagram shown, consisting of alternating single and double bonds between carbon atoms and single bonds between carbon and hydrogen atoms.**Diagram Explanation:**The diagram illustrates the Lewis Dot Structure of benzene, which is a hexagonal ring with each carbon atom bonded to one hydrogen atom. The carbon atoms are connected alternately by single and double bonds.**Extra Credit Question:**Considering the Lewis Dot Structure of Benzene, why might the calculated enthalpy value not be accurate?*Answer Guide:*Benzene has resonance structures, meaning its electrons are delocalized across the ring. This delocalization affects the bond energies, as the actual C-C bonds are intermediate in character between single and double bonds. This can lead to discrepancies between the calculated enthalpy change using average bond enthalpies and the actual enthalpy change.

The combustion reaction of benzene is expressed as, C6H6l+152O2g→6CO2g+3H2OgThe enthalpy change of the given reaction is calculated by the formula, ∆H=12∆HC=O+6∆HO-H-3∆HC-C+3∆HC=C+6∆HC-H+152∆HO=O......(1) Where, ∆HC=O is the bond enthalpy of C=O. ∆HO-H is the bond enthalpy of O-H. ∆HC-C is the bond enthalpy of C-C. ∆HC=C is the bond enthalpy of C=C. ∆HC-H is the bond enthalpy of C-H. ∆HO=O is the bond enthalpy of O=O.Substitute the bond enthalpy of C=O, O-H, C-C, C=C, C-H and O=O in equation (1). ∆H=12×805 kJ/mol+6×464 kJ/mol-3×348 kJ/mol+3×614 kJ/mol+6×413 kJ/mol+152×498 kJ/mol=9660 kJ/mol+2784 kJ/mol-1044 kJ/mol+1842 kJ/mol+2478 kJ/mol+3735 kJ/mol=12444 kJ/mol-9099 kJ/mol=3345 kJ/mol Therefore, 3345 kJ/mol of energy is required for the combustion of 1 mol of benzene.Answer: The enthalpy change of the reaction is 3345 kJ/mol.

Science

Chemistry

6. Calculate the change in enthalpy, AH, for the following reaction using bond enthalpies for 1 mole of benzene: C,H, (1) +02 (g) → 6 CO2 (g) + 3 H2O (g) Bond Type Average bond enthalpy (kJ/mol) C-H 413 C-C 348 C=C 614 O=0 498 C=0 805 O-H 464 C-O 360 C6H6 is benzene: a ringed structure as shown. Extra Credit: Considering the Lewis Dot Structure of Benzene, why might this value not be accurate?

6. Calculate the change in enthalpy, AH, for the following reaction using bond enthalpies for 1 mole of benzene: C,H, (1) +02 (g) → 6 CO2 (g) + 3 H2O (g) Bond Type Average bond enthalpy (kJ/mol) C-H 413 C-C 348 C=C 614 O=0 498 C=0 805 O-H 464 C-O 360 C6H6 is benzene: a ringed structure as shown. Extra Credit: Considering the Lewis Dot Structure of Benzene, why might this value not be accurate?

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...

See similar textbooks

Similar questions

stion 7 of 41 > Use the molar bond enthalpy data in the table to estimate the value of AHan for the equation Average molar bond enthalpies. (Hpond) Bond kJ. mol- Bond kJ . mol- CCI,(g) + 2 F,(g) → CF,(g) + 2C,(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 +に+章 F-F C-CI O=0 502 N=N 418 CH C=0 730 N=N 945 F-F C-CI С-С 347 F-F 155 C=C 615 Cl–CI 243 C=C 811 Br-Br 192 С-Н 414 H-H 435 С-F 439 Н-F 565 C-CI 331 H-Cl 431 С-Br 276 Н-Br 368 С-N 293 H-S 364 C=N 615 S-S 225 AHn = kJ Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry| Publisher: University Science Books S A «tv MacBook Air 80 DII DD F3 F8 F10 F11 F12 F4 F5 F6 F7 F9
PCB, CO, HCO3, H&PO4 2.Calculate the enthalpy change for the reaction H2+ CH20 CH3OH given the following bond enthalpies: C-H=413 kJ/m, C-C = 348 kJ/m, C-0 = 358 kJ/m, C-0=743 kJ/m, H-H=436 kJ/m, O-H=463 kJ/m %3D %3D 11 %3D %3D
Use the bond dissociation energies provided to calculate the detla H (in kilojoules) for the combustion of ethylene gas according to the balanced equation provided: C2H4 (g) + 3 O2 (g) equals 2 CO2 (g) + 2 H2O (g)
True or False: This reaction is endothermic because more energy is needed to break up the reactants versus the amount given off by the products. Use the reaction and bond information to answer the question. H-H +0=C = 0 - H-C = O | O-H H2 + CO, → CH,O. Reactant bond energies: H-H is 432 kJ/mol, C=O is 799 kJ/mol Product bond energies: C-H is 413 kJ/mol, C=O is 745 kJ/mol, C-O is 358 kJ/mol, O-H is 467 kJ/mol ○ True ○ False 1
Use the bond energies provided to estimate AH°rxn for the reaction below. CH4(1) + 2 02(g) → CO2(g)+ 2 H2O(g) Bond Energy (kJ/mol). AH°r Ixn = ? Bond С-Н 410 C-O 360 C=O 800 O=0 500 O-H 470
Calculate the heat of the following reaction from the given bond energies. Give the answer to 3 significant figures. 2CH3CH3+7O2⟶4CO2+6H2O2CH3CH3+7O2⟶4CO2+6H2O Bond Energies C-H: 349 C-C: 270 O=O: 592 C=O: 695 O-H: 313
Using bond enthalpies in the table, estimate AH for the following gas-phase reactions. Average Bond Enthalpies (kJ/mol) Single Bonds C-H C-C C-N C-O C-F C-Cl C-Br C-I C-S 413 |N-H 348 |N-N 293 N-O 358 |N-F 485 |N-Cl 328 N-Br 243 276 240 259 CH–C1 242 193 Br-Br Multiple Bonds C=C C=C C=N C=N 614 839 615 391 O-H 0-0 163 201 O-F 272 O-Cl 200 O-I 201 463 146 190 203 234 339 H-H S-H 436 S-F 567 S-Cl 327 253 H-F H-Cl 431 S-Br 218 H-Br 366 S-S 266 H-I 299 |N=N 418 0=0 |N=N 941 |N=O 607 495 Part C Estimate AH for the reaction. Express your answer using one significant figure. AH = Submit —| ΑΣΦ Provide Feedback H H-N-N-H+CI-CI-2 H-N-CI -H+C₁_a_ Previous Answers Request Answer HH X Incorrect; Try Again; 3 attempts remaining ? kJ
2
3.Calculate the overall energy change in the combustion of ethane, C2H. Is it exothermic reaction or an endothermic reaction? (An example is shown in another document, which is also posted) Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391
Using the table of bond enthalpies in your textbook, predict ArH for the following reaction. Express your answer in kJ/mol. HCECH + 2 H2 → H3C-CH3
Use the data below to calculate the bond energy for a C-F bond in kJ/mol. Bond Energy (kJ/mol) С-Н 413 H-F 567 С-С 347 H-CI .431 F-F 159 H-Br 364 Cl-CI 243 H-I 297. Br-Br 193 I-I 151 The reaction shown below has AH = -3372 kJ as written C2H6lg) + 7 F2(g) → 2 CF4(g) + 6 HFig) In C2H6 each C makes 3 bonds with H and 1 bond with C 485 kJ/mol O 489 kJ/mol O -503 kJ/mol O none of the answers are correct
Propane and chlorine react in the presence of UV light to give 2-chloropropane other things: Assuming that the reaction is carried out at a temperature where everything is gaseous, estimate the enthalpy change of reaction from the following bond enthalpies. Bond enthalpy (kJ mol-1) C-H +413 CI-CI +243 C-Cl +346 H-CI +432 C-C +348