Listing of Bonds Associated bond energies (kJ/mol) 1. H - H 2. C-H 3.0 = 0 4. C = O 5. H - O 436 413 498 799 463 A pot of water is heated from 12.0°C to 57.0°C by the combustion of propane in a camp stove. The reactants undergo a bonds is released. When the above bonds are arranged from the most energetic to the least energetic, the order will be + + energy as the energy stored in the chemical

Listing of Bonds Associated bond energies (kJ/mol) 1. H - H 2. C-H 3.0 = 0 4. C = O 5. H - O 436 413 498 799 463 A pot of water is heated from 12.0°C to 57.0°C by the combustion of propane in a camp stove. The reactants undergo a bonds is released. When the above bonds are arranged from the most energetic to the least energetic, the order will be + + energy as the energy stored in the chemical

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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Show What You Know: Hess's Law Use the following chart to complete the calculations for the combustion reactions between ethanol and propane. Compound Total Bond Energy Oxygen, O2 495 kl/mol Carbon Dioxide, CO2 1598 kJ/mol Water, H,0 926 kJ/mol
Q. Use the average bond energy approach to calculate the enthalpy for the complete combustion of CH3OH(g).
Use average bond energies (table in the hint) to compare the stabilities of ethanol, C2H5OH, and dimethyl ether, (CH3)20, which have the same empirical formula, C,H¿O (all the bonds are single bonds). Based on average bond energies, is more stable by i kJ/mol. dimethyl ether eTextbook and Media ethanol
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
! 1 Q :0 F1 Calculate the enthalpy of the reaction below (AHrxn, in kJ) using the bond energies provided. 2 H₂(g) + O₂(g) → 2 H₂O(g). 482 133,809 (a 2 W F2 # 3 E Single Bond M Multiple Bonds I U ZO 80 F3 602 C=O 799 835 C=O 1072 C=N 615 O=O 494 C=N 887 N=N 942 **All values in kJ/mol** oc: 7 11 $ 4 H 432 411 346 386 305 167 459 C=C C=C O CNO a F4 358 201 142 SD F % 5 tv 0 F5 6 Q G F6 NA & 7 F7 G H 33611 RTY U * 8 W F8 ( 9 F9
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
Mm.46.
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
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol
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The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize. a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. C3H8(g)+ O2(g) ---->CO2(g)+ H2O(g) b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite. 3C(s,graphite)+4H2(g)--->C3H8(g) ΔHo = -103.8 kJ/mol C(s,graphite)+O2(g)--->CO2(g) ΔHo= -393.5 kJ/mol H2(g)+1/2 O2(g)--->H2O(g) ΔHo= -285.8 kJ/mol kJ/mol…