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Explain why the bond enthalpy of a molecule is usu­ally

Chapter 9, Problem 68P

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QUESTION:

Explain why the bond enthalpy of a molecule is usu­ally defined in terms of a gas-phase reaction. Why are bond-breaking processes always endothermic and bond-forming processes always exothermic?

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QUESTION:

Explain why the bond enthalpy of a molecule is usu­ally defined in terms of a gas-phase reaction. Why are bond-breaking processes always endothermic and bond-forming processes always exothermic?

ANSWER:

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Bond enthalpy can be described by doing the measurement of the heat required in order to break one mole of a molecule into different atoms. Bond energy is defined as the energy that is required to break only one mole of bonds in the gas phase. A higher value of bond energy indicates higher stability.

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