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9 March, 10:18

Given: 2H2O2 → 2H2O + O2 structure of H2O2: H-O-O-H Bond Bond Energy (kJ/mol) O-H 459 O=O 494 O-O 142 Based on the given bond energies, what is the enthalpy change for the chemical reaction? A. - 352 kJ B. - 210 kJ C. - 176 kJ D. - 105 kJ

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  1. 9 March, 13:51
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    B. - 210 kJ

    Explanation:

    ∵ ΔHrxn = ∑ (bond energies) products - ∑ (bond energies) reactants.

    The bond formation in the products releases energy (exothermic). The bond breaking in the reactants requires energy (endothermic).

    The products:

    H₂O contains 2 O-H ( - 459 kJ/mol) bonds. O₂ contain 1 O=O ( - 494 kJ/mol) bond.

    The reactants:

    H₂O₂ contain 2 O-H (459 kJ/mol) bonds and 1 O-O (142 kJ/mol) bond.

    ∵ ΔHrxn = ∑ (bond energies) products - ∑ (bond energies) reactants.

    ∴ ΔHrxn = [2 (2 x (O-H bond energy) + (1 x (O=O bond energy) ] - 2 [ (2 x (O-H bond energy) + (1 x (O-O bond energy) ] = [2 (2 x - 459 kJ/mol) + (1 x - 494 kJ/mol) ] - 2 [ (2 x 459 kJ/mol) + (1 x 142 kJ/mol) ] = ( - 2330 kJ) + (2120 kJ) = - 210 kJ.
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