Calculate the amount of energy released by the reaction
$\mathrm{H}_{2}+{\textstyle{\frac{1}{2}}}\mathrm{O}_{2}\to\mathrm{H}_{2}\mathrm{O}$

at 1 atm pressure using the following bond enthalpies in normal conditions (298 K, 1 atm): H – H = 432 kJ/mol, O – O = 494 kJ/mol, and H – O = 460 kJ/mol.

Question

Calculate the amount of energy released by the reaction

[latex]\mathrm{H}_{2}+{ extstyle{\frac{1}{2}}}\mathrm{O}_{2} o\mathrm{H}_{2}\mathrm{O}[/latex]

at 1 atm pressure using the following bond enthalpies in normal conditions (298 K, 1 atm): H – H = 432 kJ/mol, O – O = 494 kJ/mol, and H – O = 460 kJ/mol.

Accepted Answer

The energy is estimated from the number of bonds broken and formed. It costs energy to break bonds. Energy is released when bonds are formed: 2(460) − 494/2 − 432 = 241 kJ/mol

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