Practice - Standard enthalpy of formation (ΔHf0)
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
Define standard enthalpy of formation (ΔHf0).
💡 Hint: Think about the energy change involved when making a compound.
Is ΔHf0 zero for elements under standard conditions?
💡 Hint: Consider how we refer to pure elements in enthalpy calculations.
4 more questions available
Interactive Quizzes
Quick quizzes to reinforce your learning
What is the value of ΔHf0 for elements in their standard states?
💡 Hint: Consider the basic definition of standard enthalpy.
True or False: ΔHr can be directly calculated from the sum of standard enthalpies of formation.
💡 Hint: Reflect on the relationship of products and reactants' enthalpy.
1 more question available
Challenge Problems
Push your limits with advanced challenges
A reaction involving 1 mole of CO2 being formed from C and O2 has ΔHf0 of -393.5 kJ/mol. Calculate the heat change associated with forming 2 moles of CO2.
💡 Hint: Consider how enthalpy changes with moles. What do you multiply by?
You have the following ΔHf0 values: C(s) = 0, O2(g) = 0, CO2(g) = -393.5 kJ/mol. Calculate ΔHr for the reaction: C(s) + O2(g) → CO2(g).
💡 Hint: Remember to apply the correct formula and where to pull values from.
Get performance evaluation
Reference links
Supplementary resources to enhance your learning experience.