using bond enthalpies , how much energy is required to create one mole of formaldehyde, CH2O?
Added by Emily I.
Step 1
The bond enthalpies for the relevant bonds are as follows: C-H bond: 413 kJ/mol O=O bond: 498 kJ/mol We have 2 C-H bonds and 1 O=O bond to break. So, the energy required to break these bonds is: (2 × 413 kJ/mol) + (1 × 498 kJ/mol) = 826 kJ/mol + 498 kJ/mol = Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 77 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
How much energy, in joules, is required to break the bond in one chlorine molecule? The bond energy of $\mathrm{Cl}_{2}$ is $242.6 \mathrm{~kJ} / \mathrm{mol}$.
What is bond energy? How can you use average bond energies to calculate enthalpies of reaction?
CO (g) + 2H2 (g) → CH3OH (l) ΔHrxn = -128 kJ Calculate the C—H bond energy given the following bond enthalpies: D(C≡O) = 1072 kJ, D(H-H) = 436 kJ, D(C-O) = 358 kJ, D(O-H) = 463 kJ
David C.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD