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3 cards from this section. Quick, good the night before a test.
Define enthalpy.
Think about the energy balance in reactions.
What sign does ΔH have in an exothermic reaction?
Reflect on energy being released.
What does a negative ΔH indicate?
Remember the definitions of exothermic and endothermic.
Is the following statement true or false? 'Endothermic reactions result in a positive ΔH.'
Reflect on what happens to energy during these reactions.
Consider a chemical reaction with the following enthalpy values: Reactants = 250 kJ, Products = 300 kJ. Classify the reaction based on ΔH. What does this mean in terms of energy exchange?
Use the enthalpy formula to classify the reaction.
A reaction has a ΔH of -75 kJ. How can you apply this knowledge in an industrial process? Provide an example.
Think about processes that benefit from released energy.
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