Use bond enthalpies in the table below to estimate AH for each of the following reactions.Average bond enthalpy (kJ/mol)Part AC-H: 413N-H: 391O-H: 463F-F: 155C-C: 348N-N: 1630-0: 146C=C: 614N-O: 201O=0: 495Cl-F: 253BrBrBr-C-H+Cl-Cl→ Br- C-Cl+ CI-HBrBrExpress your answer in kilojoules to three significant figures.C-N: 293N-F: 272O-F: 190Cl-Cl: 242C-O: 358N-Cl: 200O-Cl: 203Br-F: 237ΜΕ ΑΣΦ7 0?C=O: 799N-Br: 243O-I: 234Br-Cl: 218C-F: 485H-H: 436Br-Br: 193AH=C-Cl: 328H-F: 567C-Br: 276C-I: 240H-Cl: 431H-Br: 366H-I: 299I-Cl: 208SubmitRequest AnswerI-Br: 175I-I: 151Part BkJConstants | PeriodicHH-C-H+20=00=C=0 + 2 H-O-HHExpress your answer in kilojoules to three significant figures.ΔΗ=ΜΕ ΑΣΦSubmitRequest AnswerProvide FeedbackMacBook Pro20?kJ

Use bond enthalpies in the table below to estimate AH for each of the following reactions. Average bond enthalpy (kJ/mol) Part A Br Br Br-C-H+Cl-Cl→ Br-C-CI+ Cl-H Br Br Express your answer in kilojoules to three significant figures. C-H: 413 N-H: 391 O-H: 463 F-F: 155 C-C: 348 N-N: 163 0-0: 146 C=C: 614 N-O: 201 O=0: 495 Cl-F: 253 C-N: 293 N-F: 272 O-F: 190 Cl-Cl: 242 C-O: 358 N-Cl: 200 O-Cl: 203 Br-F: 237 C=O: 799 N-Br: 243 O-I: 234 Br-Cl: 218 C-F: 485 H-H: 436 Br-Br: 193 AH = C-Cl: 328 H-F: 567 C-Br: 276 H-Cl: 431 C-I: 240 H-Br: 366 H-I: 299 I-I: I-Cl: 208 I-Br: 175 151 ▾ Part B ΜΕ ΑΣΦ Submit Request Answer ? kJ H H-C-H+2 0 0 0=C=0 + 2 H-O-H H Express your answer in kilojoules to three significant figures. ΜΕ ΑΣΦ ΔΗ Submit Request Answer kJ

Use bond enthalpies in the table below to estimate AH for each of the following reactions. Average bond enthalpy (kJ/mol) Part A Br Br Br-C-H+Cl-Cl→ Br-C-CI+ Cl-H Br Br Express your answer in kilojoules to three significant figures. C-H: 413 N-H: 391 O-H: 463 F-F: 155 C-C: 348 N-N: 163 0-0: 146 C=C: 614 N-O: 201 O=0: 495 Cl-F: 253 C-N: 293 N-F: 272 O-F: 190 Cl-Cl: 242 C-O: 358 N-Cl: 200 O-Cl: 203 Br-F: 237 C=O: 799 N-Br: 243 O-I: 234 Br-Cl: 218 C-F: 485 H-H: 436 Br-Br: 193 AH = C-Cl: 328 H-F: 567 C-Br: 276 H-Cl: 431 C-I: 240 H-Br: 366 H-I: 299 I-I: I-Cl: 208 I-Br: 175 151 ▾ Part B ΜΕ ΑΣΦ Submit Request Answer ? kJ H H-C-H+2 0 0 0=C=0 + 2 H-O-H H Express your answer in kilojoules to three significant figures. ΜΕ ΑΣΦ ΔΗ Submit Request Answer kJ

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.93E: Find the enthalpies of the combustion reactions for methane through n-octane. Plot them versus the...

See similar textbooks

Similar questions

Enthalpy changes for the following reactions can be determined experimentally: N2(g) + 3 H2(g) 2 NH3(g) rH = 91.8 kJ/mol-rxn 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) rH = 906.2 kJ/mol-rxn H2(g) + O2(g) H2O(g) rH = 241.8 kl/mol-rxn Use these values to determine the enthalpy change for the formation of NO(g) from the elements (an enthalpy change that cannot be measured directly because the reaction is reactant-favored). N2(g) + O2(g) NO(g) rH = ?
Calculate the enthalpy change when 1.0(1 g of methane is burned in excess oxygen according to the reaction CH,(g) 4- 2O2(g) ->CO2(g) + H-CH/) 1H = -891 kJ/mol
Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.
Compare your answer from Exercise 72 of Chapter 3 to the H value calculated from standard enthalpies of formation in Appendix 4. Explain any discrepancies. .. 72. Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: Use tabulated values of bond engines(Table 3-3) to estimate E for this reaction
If a reaction occurs readily but has an endothermic heat of reaction, what must be the driving force for the reaction?
The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?
9.99 The chemical reaction BBr3(g)+BCl3(g)BBr2Cl(g)+BCl2Br(g) , has an enthalpy change very close to zero. Using Lewis structures of the molecules, all of which have a central boron atom, provide a molecular-level description of why H for this reaction might be very small.
Find the enthalpies of the combustion reactions for methane through n-octane. Plot them versus the number of carbon atoms in the molecule, and determine an equation that gives H for the combustion of a given hydrocarbon. Then use the equation to predict the enthalpy of combustion for n-C12H26 and compare it to experimental values.
The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?
When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?
Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide. CH3OH () + CO(g) CH3CO2H() rH= 134.6 kJ/mol-rxn What is the enthalpy change for producing 1.00 L of acetic acid (d = 1.044 g/mL) by this reaction?
A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.