The Cl-Cl bond energy is 243 kJ/mol. Therefore the formation of a single bond between chlorine atoms ? A) should require the absorption of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed. B) should result in the release of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed.

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The Cl-Cl bond energy is 243 kJ/mol. Therefore the formation of a single bond between chlorine atoms ? A) should require the absorption of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed. B) should result in the release of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed.

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Answer 1 · 2015-04-24T23:36:59

The bond energy, or bond enthalpy, expresses the energy needed to break a chemical bond, that's why it will always be listed as a positive value.

In your case, 243 kJ of energy are required to break the $Cl-Cl$ $"Cl-Cl"$ bond per mole of $C l_{2}$ $Cl_2$ molecules.

On the other hand, when a $Cl-Cl$ $"Cl-Cl"$ bond is formed, 243 kJ of energy are released per mole of $C l_{2}$ $Cl_2$ molecules.

Bond making is an exothermic process, while bond breaking is an endothermic process.

Therefore, the answer is B) - the formation of a $Cl-Cl$ $"Cl-Cl"$ bond will release 243 kJ per mole of $C l_{2}$ $Cl_2$ formed.

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The Cl-Cl bond energy is 243 kJ/mol. Therefore the formation of a single bond between chlorine atoms ? A) should require the absorption of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed. B) should result in the release of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed.

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The Cl-Cl bond energy is 243 kJ/mol. Therefore the formation of a single bond between chlorine atoms ? A) should require the absorption of 243 kJ per mole of Cl2Cl_2 formed. B) should result in the release of 243 kJ per mole of Cl2Cl_2 formed.

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The Cl-Cl bond energy is 243 kJ/mol. Therefore the formation of a single bond between chlorine atoms ? A) should require the absorption of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed. B) should result in the release of 243 kJ per mole of $C l_{2}$ $Cl_2$ formed.