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the standard molar enthalpy of ClF3 is -400kj/mol. the bond enthalpies of cl2 and f2 are...
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the Cl–F bond is 254 kJ/mol.) (a) Cl2(g) + 3 F2(g) → 2 ClF3(g) (b) H2C=CH2(g) + H2(g) → H3CCH3(g) (c) 2 CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g) ITITIT Average Bond Enthalpies AH bond (kJ/mol) bond AHond (kJ/mol) bond AH bond (kJ/mol) bond bond AH bond (kJ/mol) С-Н...
Question 6 1 pts Find the average enthalpy of the PF bond in PFs(g) from the following standard molar enthalpies of formation (in kJ/mol): PF5(g) (-1595), P(g) (315), F(g) (79). 461 kJ/mol 177 kJ/mol 491 kJ/mol 398 kJ/mol 394 kJ/mol
Part A. Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (λ=465 nm). Part B. Given the bond energies (in kJ/mol) of the following bonds: F–F (155), F–Cl (193), and Cl–Cl (243), estimate the molar enthalpy of formation of ClF(g), that is find ∆H for the following reaction ½Cl2(g) + ½F2(g) → ClF(g)
the bond enthalpy of cl2 is 242.7 kj/mol . calculate delta Hf for Cl (g). 3. The bond enthalpy of Cl2(g) is 242.7 kJ/mol. Calculate AHⓇ for Cl (g).
Given the bond energies (in kJ/mol) of the following bonds: F–F (155), F–Cl (193), and Cl–Cl (243), estimate the molar enthalpy of formation of ClF(g), that is find ∆H for the following reaction ½Cl2(g) + ½F2(g) → ClF(g) A. 209 kJ/mol B. -50. kJ/mol C. –8 kJ/mol D. –209 kJ/mol E. 8 kJ/mol
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the CI-F bond is 254 kJ/mol.) (a) C12(g) + 3 F2(9) ► 2 CIF3(9) -817 kJ (b) H_C=CHCH2(g) + H2(9) ► H,CCH, CH3(9) 476x kJ (c) CHz(C=O)CH3(g) + 402(9) ► 300,(9) + 3 H20(9) 127 X kJ Supporting Materials Periodic Table 1 Supplemental Data Constants and Factors Additional Materials eBook
Use the molar bond enthalpy data in the table to estimate the Average molar bond enthalpies. (Hd value of AHn for the equation kJ mol Bond Воnd kJ mol CH)+HBrig)C,H,Brig) O-H 464 CEN 890 O-O The bonding in the molecules is shown. 142 N-H 390 C-O 351 N-N 159 H Br O-O 502 N-N 418 H-Br NEN C-O 730 945 C-C 347 F-F 155 Enter numeric value С-С 615 CI-CI 243 AH = C C Br-Br I kJ 811 192...
e standen med en ganger The standard molar enthalpy of formation of CIF3 is -405 kJ. 1/2 Ch(g) + 3/2 F2(g) → CIF 3(g) The bond energies of Ch and F2 are 243 kJ and 159 kJ/mol, respectively. Calculate the energy of a CHF bond. a) 188 kJ/mol b) 255 kJ/mol c) 375 kJ/mol d) 563 kJ/mol e) 807 kJ/mol 1923 . cepentinely couporabimo
TC05E04 Use the enthalpies of formation given in the table below to calculate the standard molar enthalpy change for this reaction at 298K: 2CuS(s) 302(g)2CuO(s)+ 2SO2(g) AfH / kJ mol at 298K, standard Substance state 1 bar. CuO(s) -157 SO2(g) -297 CuS(s) -53 Select one: a. -802 kJ mol1 b. +401 kJ mol1 c. +802 kJ mol1 d. -507 kJ mol1 e. -401 kJ mol1
1. Calculate the bond energy of the CI-F bond using the following data: Cl2(g) + F2(g) → 2CIF(g) AH = -108 kJ Bond enthalpies (kJ/mol): CI-CI (239); F-F (159) CI-C1 = 239 F.F : 159 1 2. Find the experimental Lattice energy of aluminum oxide using a Born-Haber cycle using the following information: AH® (aluminum oxide) = -1676 kJ/mol IE, (aluminum) = 577.6 kJ/mol IE, (aluminum) =1816.7 kJ/mol IE(aluminum) = 2744.8 kJ/mol AH® (aluminum atom, g) = 329.7 kJ/mol AHⓇEAI...