1.4.1 - Enthalpy of Formation (ΔH_f°)
Enroll to start learning
You’ve not yet enrolled in this course. Please enroll for free to listen to audio lessons, classroom podcasts and take practice test.
Practice Questions
Test your understanding with targeted questions
What is the standard enthalpy of formation for elements in their standard state?
💡 Hint: Remember the definition of standard enthalpy of formation.
Write the reaction equation for the formation of water.
💡 Hint: Think of what elements combine to form water.
4 more questions available
Interactive Quizzes
Quick quizzes to reinforce your learning
What is the enthalpy of formation of elements in their standard state?
💡 Hint: Think about the baseline for enthalpy.
Is the enthalpy of formation for water negative or positive?
💡 Hint: Recall what happens during process energy release.
1 more question available
Challenge Problems
Push your limits with advanced challenges
Acetylene (C₂H₂) undergoes combustion to form CO₂ and H₂O. Given ΔH_f° is -1,203 kJ/mol for C₂H₂, -393.5 kJ/mol for CO₂, and -285.8 kJ/mol for H₂O, calculate the ΔH for the combustion reaction.
💡 Hint: Balance the reaction before plugging in enthalpy values.
Use Hess's law to find ΔH for the reaction 2NH₃(g) + 3O₂(g) → N₂(g) + 3H₂O(l). Given provided formation values, calculate and show steps.
💡 Hint: Break it down into multiple known reactions to build it out stepwise.
Get performance evaluation
Reference links
Supplementary resources to enhance your learning experience.