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Consider the hypothetical elements X and Y. Suppose the enthalpy of formation for the compound XY is ƒ{336 kJ/mol, the bond energy for X2 is 414 kJ/mol, and the bond energy for Y2 is 159 kJ/mol. Estimate the XY bond energy in units of kJ/mol.

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    X2 + Y2 => 2XY delta H format = 2*336 kJ.

    X2 = 414 = bond energy = B.E.
    Y2 = 159
    (sum B.E.reactants-sum B.E. products) = delta H rxn.
    (414+159)-(2*B.E. products)= -672
    NOTE: It isn't clear to me what the sign is for delta Hf for XY. I have assumed you intended to type a - sign; however, whatever the sign is for delta Hf that goes in for the 672. I have multiplied by 2 since there are two moles involved.
    You can work out the B.E. products as the only unknown in the equation. You can check the number by the following:
    [(414/2)+(150/2)]-(B.E. product you calculate) = delta Hf.

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