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77 solutions

Bond Energy

Q. Suppose you did not have the molar enthalpy of formation for the following reaction: CH4(g) + H2O(g) → 3 H2(g) + CO(g). You could estimate ΔH° from the bond enthalpies. First, draw the dot structure for the reactants and products. Now calculate ΔH° from bond enthalpies of the reactant and products.

Solved • Dec 4, 2019

Bond Energy

Q. Use the molar bond enthalpy data in the table to estimate the value of ΔH°rxn for the equation: CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g).

Solved • Dec 3, 2019

Bond Energy

Q. What is the approximate enthalpy of reaction (in kJ mol^-1) for the following combustion reaction CH4(g) + O2 (g) --> CO2(g) + H2O (g) using the given bond enthalpies (given bond enthalpies (given in kJ mol^-1)? (O-H)459 (C-H) 411 (O-O) 142 (O=O 494. (C-O) 358 (C=O) 799 a) -688 b) -378 c) -1095 d) -1692

Solved • Dec 2, 2019

Bond Energy

Q. Calculate the enthalpy of combustion using the bond energies

Solved • Dec 1, 2019

Bond Energy

Q. Calculate the enthalpy of the following reaction based on average bond enthalpies from the textbook: N-H = 391 kJ/mol, H-H= 432 kJ/mol, N (triple bond) N = 945 kJ/mol.

Solved • Nov 29, 2019

Bond Energy

Q. Estimate ΔE for the reaction: C2H6(g) + Cl2(g) ---> C2H5Cl(g) + HCl(g) given the following average bond energies in kJ/mol: C-C, 348; C-H, 414; Cl-Cl, 242; C-Cl, 327; H-Cl, 431

Solved • Nov 26, 2019

Bond Energy

Q. Consider the following gas phase reaction: F2(g) + I2(g) → 2 FI(g) You will note from the data provided that the bond energy for FI(g) is greater than the bond energies of either F2(g) or I2(g). 1. Speculate on why the bond enthalpy of FI(g) is greater than the bond enthalpies of either F2(g) or I2(g). 2. Based on the bond energies, do you expect the above reaction to be endothermic or exothermic? Explain your reasoning. B. Now use bond energies to estimate ΔH° for the above reaction. Does your answer agree with your prediction in I.A. 1 above?

Solved • Nov 21, 2019