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2 cards from this section. Quick, good the night before a test.
What is the definition of enthalpy?
Think about the relationship between heat and the energy of the system.
Describe what an exothermic reaction is.
Consider the temperature changes in the surroundings during such reactions.
What does a negative ΔH signify?
Consider how temperature might change in the surroundings.
True or False: Hess's Law allows you to calculate reaction enthalpy regardless of the reaction pathway.
Consider what Hess's Law helps in determining.
Determine the enthalpy change for the reaction 3 H₂(g) + N₂(g) → 2 NH₃(g) using standard enthalpy of formation values: ΔH_f°[NH₃(g)] = –45.9 kJ/mol ΔH_f°[H₂(g)] = 0 ΔH_f°[N₂(g)] = 0
Think about how to apply the standard enthalpy of formation equation in practice.
Using bond enthalpies, estimate ΔH for the reaction: C₂H₄(g) + H₂(g) → C₂H₆(g). Assume average bond enthalpies are: C=C = 614 kJ/mol, C–C = 347 kJ/mol, C–H = 413 kJ/mol.
Use average bond energies for the calculations involved.
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