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# Bond Energies: Enthalpy Change

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Dinitrogen monoxide (or nitrous oxide), N_2O(g), can decompose to nitrogen and oxygen gases:

2 N_2O(g) -> 2 N_2(g) + O_2(g)

Use average bond energies to estimate the enthalpy change for this reaction.

https://brainmass.com/chemistry/bonding/bond-energies-enthalpy-change-482401

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Equation:

Computing for the enthalpy change of the reaction:
âˆ†Hreaction = âˆ‘m(BE of reactants) - âˆ‘n(BE of products)
âˆ†Hreaction = [2(BE of N N) + 2(BE of N O)] - [2(BE of N N) + 1(BE of O O)
âˆ†Hreaction = [2 mol(945 kJ/mol) + 2 mol(201 kJ/mol)] - [2 mol(945 kJ/mol) + 1 mol(498 kJ/mol)
âˆ†Hreaction = 2292 kJ - 2388 kJ
âˆ†Hreaction = -96 kJ

Note: the multiplier 2 takes into account the total number of bonds to be broken as affected by the coefficient of the substance in the balanced equation.