Question detail
What is the definition of mean bond enthalpy?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Energetics
Question
- A. The average energy required to break one mole of bonds in a gaseous molecule.
- B. The total energy released when one mole of bonds is formed in a gaseous molecule.
- C. The energy change associated with the formation of one mole of a compound from its elements.
- D. The energy required to convert a solid into a gas at constant pressure.
Answer
The average energy required to break one mole of bonds in a gaseous molecule.
Explanation
Mean bond enthalpy is defined as the average energy needed to break one mole of a specific type of bond in a gaseous state, reflecting the strength of the bond.
Common mistake
Mean Bond Enthalpy Confusion
Students often confuse mean bond enthalpy with the actual bond enthalpy of specific bonds in a molecule.
Mean bond enthalpy is an average value for a bond type across different compounds. To define it, state: Mean bond enthalpy is the average energy required to break one mole of a specific type of bond in a gaseous molecule. For example, the mean bond enthalpy for a C-H bond is calculated by averaging the bond energies from various compounds containing C-H bonds.
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