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5 cards from this section. Quick, good the night before a test.
What are standard conditions in thermochemistry?
Think about the definitions we discussed.
What does ΔH_f° represent?
Remember the definition we talked about!
What is the standard enthalpy of formation (ΔH_f°)?
Think of what formation means in thermodynamics.
True or False: Standard enthalpy of combustion (ΔH_c°) is always positive.
Consider what happens during the combustion of fuels.
Given the enthalpy changes: ΔH_f°[C₆H₁₂O₆] = -2,803 kJ/mol (glucose), calculate the heat liberated when burning 1 mole of glucose completely in excess oxygen using combustion data.
Think back to combustion reactions and their enthalpy definitions.
Utilize Hess's Law to find ΔH for the reaction: C₂H₄ + 3 O₂ → 2 CO₂ + 2 H₂O, using: ΔH_f°[C₂H₄(g)] = +52.3 kJ/mol, ΔH_f°[CO₂(g)] = -393.5 kJ/mol, ΔH_f°[H₂O(l)] = -285.8 kJ/mol.
Reference the formation equation while collecting enthalpy values.
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