Answer is b) Benzene.
Because in benzene involve resonance thus double bonds are not purely single nor purely double hence error in benzene is most. Also number of double bonds involve in resonance in benzene is more as compared to butadiene.
Which of the following molecules has the largest error if you use mean bond energies to...
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 table below lists the average bond energies that you would need to determine reaction enthalpies. Use bond energies to calculate the enthalpy of formation of NH3 in kJ/mol. Express your answer numerically, in terms of kJ/mol and to three significant figures.
Use the average bond energies in the text to estimate the enthalpy changes of the following reactions: N_2(g) + O_2(g) rightarrow 2 NO(g) C(s) + CO_2(g) rightarrow 2 Co(g)
10. Using the tabulated bond energies, determine the approximate enthalpy change for each of the following rear (a) Ha(e)+Br3(g)--2HBr(e) osing the tabulated bond energies, determine the approximate enthalpy change for each of the following reactions (b) C.H.(8)+302(B) 2Co(s)+2H2O() 12. Which compound in each of the following pairs has the larger lattice energy? Note: Baand K' have similar radil;s and i have similar radil. Explain your choices. (a)KO or Na20 (b) K.S or Bas 13. Draw all possible resonance Lewis structures...
Calculate enthalpy of reaction using bond energies Use the References to access important values if needed for this question. Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. I2(g) +Cl2(g) 2ICI(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...
Use the Bond Energies Table to estimate the enthalpy change in each of the following reactions. (Enter your answer to the nearest integer.) (a) CH4(g) C(g) 2 H2(g) 4.0 X kJ/mol (b) ICH3(g) + H20(g) H3COH(g) HI(g) 4.0 X kJ/mol HC CH(g)2 H2(g)H3C-CH 3 (g) (c) 4.0 X kJ/mol
Which of the following statements are FALSE, given the following bond dissociation energies? Assume that bond energies accurately determine heats of reaction. Check all that are false. BE[H-H] = 436 kJ/mol BE[H-N] = 393 kJ/mol BE[H-O] = 460 kJ/mol BE[O=O] = 499 kJ/mol 1. NH(g) + H2(g) ---> NH2(g) + H(g) is an exothermic reaction. 2.ΔH°f[H(g)] = 218 kJ/mol 3. ΔH°[H2O(g) ---> 2 H(g) + O(g)] = 920 kJ/mol 4. An H-H bond is stronger than an H-O bond. 5....
.127. Use average bond energies to estimate the enthalpy changes of the following reactions: N2(g)+3 H2(g)2 NH(g) b. N2(g)+2 H2(g)H,NNH2(g) c. 2 N(g) + O(g)2 N,O(g) a. 9.103. Consider the following molecular ions: N2, O2, C2, and Br22. Using MO theory, (a) write their orbital electron configuration; (b) predict their bond orders; (c) state whether you expect any of these species to exist.
The table below lists the average bond energies that you would need to determine reaction enthalpies. Use bond energies to calculate AHrxn for the following reaction: 2 NO (g) + 5 H2 (g) → 2 NH3(g) + 2 H20 (g) Enter your answer numerically, in terms of kJ and to three significant figures.
Sample A has a larger standard error of the mean than Sample B. Which sample mean would you trust to be a better estimate of the population mean? a. both samples would provide equally good estimates of the population mean b. unable to determine with the provided information c. Sample A d. Sample B