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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

SOLUTION This solution is FREE courtesy of BrainMass!

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Equation:

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