Explaining Enthalpy Changes (HSC SSCE Chemistry): Flashcards

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Explaining Enthalpy Changes
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Bond energy definition

Energy to break 1 mole of a bond in gaseous molecule

Units of bond energy

kJ mol−1\text{kJ mol}^{-1}

Sign of bond energy value

Always positive

Why is bond energy always positive?

Breaking bonds requires energy input

Bond breaking process type

Endothermic

Bond making process type

Exothermic

ΔH\Delta H formula from bond energies

Energy to break bonds - energy released forming bonds

Condition for exothermic reaction

More energy released forming bonds than breaking them

Condition for endothermic reaction

More energy to break bonds than released forming them

Effect of higher bond energy

More stable and less reactive compound

Explore HSC SSCE Chemistry Revision Notes by Topics

Energy Changes in Chemical Reactions

Enthalpy and Hess's Law

Entropy and Gibbs Free Energy

Explore HSC SSCE Chemistry Model Answers by Topics

Energy Changes in Chemical Reactions

Enthalpy and Hess's Law

Entropy and Gibbs Free Energy

Explore HSC SSCE Chemistry Quizzes by Topics

Energy Changes in Chemical Reactions

Enthalpy and Hess's Law

Entropy and Gibbs Free Energy

Explore HSC SSCE Chemistry Exam Questions by Topics

Energy Changes in Chemical Reactions

Enthalpy and Hess's Law

Entropy and Gibbs Free Energy

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