The reaction of ethene, C2H4, to form polyethylene is shown below: (See Table 3-2.)2n+Estimate how much energy is released when one mole of ethene forms polyethylene using bond energies.75 kJ/mol38 kJ/mol690 kJ/mol345 kJ/mol69 kJ/mol

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Chemistry

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Enter your answer in the provided box. Use the bond enthalpies given below to estimate the enthalpy of reaction for the combination of carbon monoxide and oxygen to produce carbon dioxide: 2CO(g) + O2(g) → 2CO2(g)
5. For the reaction H2(g) + C2H4(g) C2H6(g) (a) Estimate the enthalpy of reaction, using the bond enthalpy values. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. (AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol, respectively.)
Dd.41.
Using the bond energies provided below, calculate the enthalpy change (AHrxn) for the reaction shown. 2H₂O (g) → 2H2(g) + O2(g) Bond: Avg. bond energy (kJ/mol): -425 kJ/mol -509 kJ/mol 356 kJ/mol 509 kJ/mol 7 kJ/mol 425 kJ/mol H-H O-H 432 467 O-O 146 O=O 495
If the following reaction is given: C2H5F + Cl2 || AHran If the bond energy for C-H is 414 kJ/ mole, the bond energy for C-C is 347 kJ/mole, the bond energy for C-Cl is 377 kJ/ mole, the bond energy for Cl-Cl is 243 kJ/ mole, the bond energy for C-F is 450 kJ/ mole and the done energy for H-Cl is 431 kJ/ mole, determine the bond energy for the H-F bond in kJ/mole. C2H4Cl2 + HF 151kJ mole Give your answer as a positive value as all energies for bond values should be written in terms of a positive value (the energy needed to break the bond = endothermic)
Don't give handwritten answers Which of the following is the formation reaction for N2O (g)? Group of answer choices A.) 1/2 N2(g) + 2 O2(g) → NO2(g) B.) 1/2 N2(g) + O2(g) → NO2(g) C.) N(g) + O2(g) → NO2(g) D.) 2 N2(g) + O2(g) → 2 NO2(g) E.) N(g) + 2 O(g) → NO2(g)
Give ∆H(reaction) in kj/mol
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Enter your answer in the provided box. For the reaction O(g) + O2(g) → O3(g) Δ H o = −107.2 kJ/mol Given that the bond enthalpy in O2(g) is 498.7 kJ/mol, calculate the average bond enthalpy in O3.
PCB, CO, HCO3, H&PO4 2.Calculate the enthalpy change for the reaction H2+ CH20 CH3OH given the following bond enthalpies: C-H=413 kJ/m, C-C = 348 kJ/m, C-0 = 358 kJ/m, C-0=743 kJ/m, H-H=436 kJ/m, O-H=463 kJ/m %3D %3D 11 %3D %3D
Use the bond energies (kJ/mol) given (using variables only) to calculate the total enthalpy (energy) change for the following reaction: H2C=CH2(g) + Cl2(g) = ClH2C-CH2Cl(g) (Each carbon in the product has 2 H and one Cl atom bonded to it) Bond Energies: C-H: A C=C: B Cl-Cl: C C-C: D C-Cl: E
find the enthalpy of formation for CH3(CH2)14COONa use bond breaking and bond forming energy to find the value

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The reaction of ethene, C2H4, to form polyethylene is shown below: (See Table 3-2.) 2n + Estimate how much energy is released when one mole of ethene forms polyethylene using bond energies. 75 kJ/mol 38 kJ/mol 690 kJ/mol 345 kJ/mol 69 kJ/mol