**Title: Calculating Average Molar Bond Enthalpy****Introduction**In this exercise, you will learn how to calculate the average molar bond enthalpy of the carbon-bromine bond in a CBr₄ molecule using given enthalpy values.**Given Data**- ΔHf [Br(g)] = 111.9 kJ·mol⁻¹- ΔHf [C(g)] = 716.7 kJ·mol⁻¹- ΔHf [CBr₄(g)] = 29.4 kJ·mol⁻¹**Objective**Calculate the average molar bond enthalpy of the carbon-bromine (C–Br) bond in a CBr₄ molecule.**Procedure**1. Use the given data and the formula for calculating bond enthalpy using the enthalpies of formation.2. Apply the relationship involving the enthalpies of formation to solve for ΔH_{C–Br}.**Calculation Area**ΔH_{C–Br} = [Calculation Placeholder]**Conclusion**Complete the calculation to find the average molar bond enthalpy of the C–Br bond. This exercise illustrates the use of thermochemical data in bond enthalpy calculations.**Note:**Ensure accuracy in your calculations and refer to any standard tables if necessary.

The balanced overall reaction will be,C + 4 Br → CBr4 Find the ΔHrxn for this reaction first ΔHrxn = [ nΔHfo (products) - nΔHfo (reactants) ] Average molar bond enthalpy can be found out by dividing theΔHrxn with total number of bonds present in CBr4 In CBr4 we have 4 C-Br bonds ΔHrxn = - 4 x ΔHC-Br (negative because bonds broken are 0)ΔHrxn = [ 1mol x 29.4 kJ/mol ] - [ (1mol x 716.7 kJ/mol) + (4mol x 111.9 kJ/mol) ] ΔHrxn = 29.4 kJ - [716.7kJ + 447.6 kJ] = -1134.9 kJ Substitute this value into the bond enthalpy equation -1134.9 kJ = -4 x ΔHC-Br ΔHC-Br = (1134.9/4) = 283.725 kJ Therefore the average molar bond enthalpy of C-Br bond in CBr4 molecule is 283.725 kJ

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Given that AH; Br(g)] = 111.9 kJ-mol- %3D AH; [C(g)] = 716.7 kJ-mol¬1 AH¡ CBr,(g)] = 29.4 kJ-mol¯1 %3D calculate the average molar bond enthalpy of the carbon-bromine bond in a CBr, molecule. AHC-Br %3D

Given that AH; Br(g)] = 111.9 kJ-mol- %3D AH; [C(g)] = 716.7 kJ-mol¬1 AH¡ CBr,(g)] = 29.4 kJ-mol¯1 %3D calculate the average molar bond enthalpy of the carbon-bromine bond in a CBr, molecule. AHC-Br %3D

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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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
Use the table below to determine ΔH for the following reactionN 2H 4(g) + H 2O(g) ↔ NH 2OH(g) + NH 3(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 C≡C 835 C≡N 887 C≡O 1072 N=N 418 N=O 607 S=O (in SO2) 532 N≡N 942 O2 494 S=O (in SO3) 469
Q. Use the average bond energy approach to calculate the enthalpy for the complete combustion of CH3OH(g).
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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
Consider the following reactions: AH = -393.5 kJ + O2(g) CO 2(9) (graphite) AH = -285.8 k) + V2 O2(g) H2(9) AH = -726.4 k CH,OH + 3/2 0, CO2(9) + 2H,0) (1) Choose... Calculate the enthalpy change for the following reaction: CH;OH) (graphite) + 2 H2(g) + 2 02
Consider the following Lewis structure and table of bond energies. What is the total sum of the bond energies in this molecule? Em H- :O: -C Ö-H H-H 436 H-F 569 H-Cl 432 H-Br 366 H-I 298 Table of Average Bond Energies (kJ/mole) C-H 410 C-C 350 C-N 300 C- O 350 C -F 450 C-Cl 330 C-Br 270 CII 240 N H N N 390 240 N-F 270 NCI 200 N-Br 240 200 N O 460 142 -F 180 200 220 01H 010 O O Cl 011 F-F 157 F-CI 251 F-Br 234 Cl-Cl Cl-Br Br-Br 1-1 1-Br -Cl 1 I-F 243 219 194 153 179 208 280 C=C C=0 C=N C-S 010 N=N N=0 C C C=0 CEN NEN 611 745 615 477 498 418 607 835 1077 891 941
Use bond enthalpies (Table 9.5 page 303) to estimate AH (kJ/mol) for the following gas-phase reaction. H H H. H+ C=C H,O H-C-C-H + | | OH H H. H Ethylene Water Ethanol
Use the bond energies provided to estimate AH°rxn for the reaction below. XeF6 AH°rxn = ? Bond Xe-F F-F XeF2+2F2 Bond Energy (kl/mol) 147 159 O-270 kJ +159 kJ -660 kJ +176 kJ -429 kJ K
28. Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HC1O,(g), and c) CH;OCH;(g)
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