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Draw a curve that describes the energy of a system with H and Cl atoms at varying distances. Then, find the minimum energy of this curve two ways.
(a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?)
(b) Use the enthalpy of reaction and the bond energies for
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- Compare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?arrow_forwardUsing the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forwardExplain the decomposition of nitroglycerin in terms of relative bond enthalpies.arrow_forward
- 3. Calculate AH°rxn for the following reactions in two ways. First, estimate the enthalpy change for the reaction using bond enthalpies (using the table provided in your notes). Then, calculate it using the enthalpies of formation provided on the back sheet. Compare your two answers. AHrxn = > bonds breaking – > bonds formed AHfeaction = Enp4H? (products) – En,4H{ (reactants) a. CO(g) + H2O(g) - H2(g) + CO2(g) Answer b. 4 NH3(g) + 5 02(g) → 4 NO(g) + 6 H2O(g) Answerarrow_forwardUsing average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: 2co(g) + 2NO(g)→2C02(g) + N2(g) kJarrow_forwardHydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.arrow_forward
- Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: CH4(g) + Cl₂(g)→→→→CH3CI(g) + HCI(g) kJarrow_forwardAcetylene gas (HC≡CH) burns in an oxygen (O2) rich torch to produce carbon dioxide and water vapor. The enthalpy of reaction for the combustion of acetylene is 1259 kJ/mol. Please use this information to solve Parts A,B,C,D. A) Calculate the C≡C bond energy.C-H: 413 kJ/mol O-O: 498 kJ/mol C-O: 799 kJ/mol O-H: 467 kJ/mol B) When 500.0 g of acetylene burns, how many kilojoules of heat are given off? C) How many grams of CO2 form? D) How many liters of O2 at 298 K and 18.0 atm are consumed? PV=nRT & R=0.0821 (L*atm)/(mol*K)arrow_forwardOctane (C8H18) is combusted with oxygen to give carbon dioxide and water vapor. Calculate the enthalpy of reaction using the bond energies given. Is the combustion of octane an endothermic or exothermic reaction? The reaction below is not balanced. pleaseanswer neatly so i can see how to do it Bond: C=O O=O C–H O–H C–C Bond energy (kJ/mol): 799 498 414 464 347arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
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