Use the bond energy to estimate the heat of reaction at 25 °C for the reaction below.CH4 (g) + 2 02 (g) → CO2 (g) + 2 H2O(g)Compare your result with that calculated from enthalpies of formation. Average Bond Energies (kJ/mol)Single BondsMultiple BondsH-H432NH391149C=C614H-F565N-N160208C=C839H-CI427N-F272-Br175O=0495H-Br363N-CI200C=0745HI295N-Br243S H347C=01072N-O201SF327N=0607C-H413O-H467S CI253N=N418C-C3470-0146S Br218N=N941C-N305O-F190266C=N891C-O358O-C203C=N615C-F485234Si Si340C-Cl339Si-H393C-Br276F-F154Si-C360240F-Cl253Si-O452C-S259F-Br237C-CI239ClBr218Br-Br193

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Answered: Use the bond energy to estimate the…

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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Given the listed average bond energies (BE), calculate the enthalpy change for the production of one mole of methanol (CH3OH) by the following reaction. (There are two C=O double bonds in CO2) CO2(g) + 3 H2(g) → CH3OH(g) + H2O(g) B.E.C–O = 300 kJ/mol B.E.C=O = 700 kJ/mol B.E.H–H = 450 kJ/mol B.E.H–O = 500 kJ/mol B.E.H–C = 400 kJ/mol Select one: a. 250 kJ b. 950 kJ c. -250 kJ d. 50 kJ e. -950 kJ
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. C2H4(g) + Br2(g) CH,BRCH,Br(g) To analyze the reaction, first draw Lewis structures for all reactant and product molecules. • Include all valence lone pairs in your answer. • Draw the reaction using separate sketchers for each species. One molecule per sketcher, please. Separate multiple reactants and/or products using the + sign from the drop-down arrow. Separate reactants from products using the If you have to draw H,, draw H-H. • Be sure that your structural equation is balanced. symbol from the drop-down menu.
Using the table of thermodynamic data provided, for the reaction below: CS₂(1) + 302(g) → CO2(g) + 2SO2(g) Compound CO₂(g) CS₂(1) O₂(g) SO₂(g) SO₂(g) AHºf (kJ/mol) -393.5 89.0 0 -296.8 -395.7 S°(J/K mol) 213.8 151.3 205.15 248.2 256.8 Determine/calculate and report the following values in the labelled boxes below: a) The standard enthalpy change (AH°, in kJ/mol) of the reaction. b) The standard entropy change (AS°, in J/K mol) of the reaction. c) The standard free energy change (AG°, in kJ/mol) of the reaction. d) The free energy change (AG, in kJ/mol) of the reaction at 7.50 x 10² K.
Q. Use the average bond energy approach to calculate the enthalpy for the complete combustion of CH3OH(g).
Is the heat of Mg combustion equal to the heat of formation of MgO when both are measured at standard conditions? Provide an explanation to your Yes/No answer.
At 25°C, calculate the AG, N₂+ 3H2 → 2NH3 sys for: f • AG˚ N2(g) = 0 kJ/mol AG H2(g) = 0 kJ/mol f • AG˚ NH3(g) = -16.66 kJ/mol f a) 12.9 kJ b) -33.3 kJ c) -16.7 kJ d) -8.33 kJ e) Unsure AG sys =ΣnpG˚ products - Σn,G° reactants 60
How much energy is required to break the bonds in the molecule of NO, BCl3, and NO2? and How do I find the ΔH of the molecule from the elements in their standard states?
For an unidentified nonmetal element X, the following chemical equation was determined and measured: XC12(g) + 2 Cl 2(g) --> XC16(g) AHrxn = -374.60 kJ Based on this information, what would be the estimated average bond energy, in kJ/mol, of an X-Cl bond?
How much heat (J) is given off when 8.2 mg of Al reacts with the right stoichiometric amount of Fe2O3 in the thermite reaction. Use the enthalpy of combustion and the balanced reaction equation. Make sure to indicate the answer to be either negative or positive. Your answer should be to 2 decimal places. ΔH = -852 kJ
Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2co(g) + 2NO(g)→2C02(g) + N2(g) kJ
The reaction of CH3OH(g) with N2(g) to give HCN(g), NH3(g), and O2(g) requires 164 kJ/mol of CH3OH(g). Write a balanced chemical equation for this reaction. Include the phases of all species in the reaction. How much heat is involved in the reaction of 65.0 g of CH3OH(g) with excess N2(g) to give HCN(g) and NH3(g) in this reaction?
What is the enthalpy of reaction for the following reaction: 2H₂O(g) → 2H₂(g) + O₂(g) Bond H-H O=O H-O Bond energy (kJ/mol) 436 499 460 VE ΑΣΦ ? kJ/mol

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Use the bond energy to estimate the heat of reaction at 25 °C for the reaction below. CH4 (g) + 2 02 (g) → CO2 (g) + 2 H2O(g) Compare your result with that calculated from enthalpies of formation.