Estimate the enthalpy of reaction for 2 H₂(g)+ O₂(g)$\to$ 2 H₂O(g)using bond energies.

Question

Quizplus · Accepted Answer

To calculate the enthalpy of the reaction using bond energies, we need to break all the bonds in the reactants and form all the bonds in the products, and take the difference between bond energies of reactants and products bonds. Reactants: 2 H₂(g): 2(S-H) + 2(S-S) + 2(U-B) = 2(413+265+149) = 1654 kJ/mol O₂(g): (O=O) + 2(S=U) + 2(B-O) = (498) + 2(385) + 2(358) = 1986 kJ/mol Total Energy required to break all reactant bonds = 1654 + 1986 = 3640 kJ/mol Products: 2 H₂O(g): 2(S-H) + 2(S=U) + 2(B-O) = 2(413+385+358) = 2312 kJ/mol Total Energy released to form all the product bonds = 2312 kJ/mol Enthalpy of the reaction = Total Energy required to break all reactants bonds - Total Energy released to form all the product bonds = 3640 - 2312 = 1328 kJ/mol Therefore, the correct choice is D) F1F1F1S1F1F1F10482 kJ/mol.

Estimate the Enthalpy of Reaction for 2 H2(g)+ O2(g) →\to→ 2 H2O(g)using Bond Energies

Estimate the Enthalpy of Reaction for 2 H₂(g)+ O₂(g) $\to$ 2 H₂O(g)using Bond Energies