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2 cards from this section. Quick, good the night before a test.
What is bond enthalpy?
Think about what happens when you break a bond.
Why do bond enthalpy values vary?
Consider different molecules containing the same type of bond.
What is bond enthalpy?
Consider what happens when you need to separate atoms in a bond.
Is ΔH positive or negative for an exothermic reaction?
Think about how energy flows in an exothermic process.
Estimate the reaction enthalpy for the combustion of butane: C₄H₁₀(g) + 6 O₂(g) → 4 CO₂(g) + 5 H₂O(g), given average bond enthalpies: C–C = 347 kJ/mol, C–H = 413 kJ/mol, O=O = 498 kJ/mol.
Ensure you breaking down every bond energy clearly for products and reactants!
Calculate the total energy change of the hydrogenation reaction of a diene compound with given bond enthalpies. Analyze why this estimate might deviate from actual values due to molecular geometry.
Pay attention to bond type changes during hydrogenation and apply realistic bond strength corrections.
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