15. Given that the bond energy of the O-H bond is 463 kJ mol?1, use the data in the table below to estimate ?Hfº of O (g) in kJ mol?1. Substance | ?Hfº / kJ mol?1 H (g) | +216.0 H2O (g) | ?241.8
Added by Xavier G.
Close
Step 1
8 kJ mol-1. We also know that the bond energy of the O-H bond is 463 kJ mol-1. This means that it takes 463 kJ of energy to break one mole of O-H bonds. Since there are two O-H bonds in each molecule of water, it takes 2 * 463 = 926 kJ to break all the O-H bonds Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 74 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
Given the following data: $$ \begin{array}{ll}{\mathrm{NO}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{O}(g)} & {\Delta H=233 \mathrm{kJ}} \\ {2 \mathrm{O}_{3}(g) \longrightarrow 3 \mathrm{O}_{2}(g)} & {\Delta H=-427 \mathrm{kJ}}\end{array} $$ $$ \mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g) \quad \Delta H=-199 \mathrm{kJ} $$ Calculate the bond energy for the $\mathrm{O}_{2}$ bond, that is, calculate $\Delta H$ for: $$ \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{O}(g) \qquad \Delta H=? $$
Average Bond Enthalpy (kJ/mol): 413, 495, 799, 463 Bond: C-H, O=O, C=O, O-H Use the bond enthalpies in the table above to estimate ΔH for the following reaction: H H-C-H + 2 O=O → O=C=O + 2 H-O-H H -377 kJ -808 kJ 2170 kJ -354 kJ -2831 kJ 1244 kJ
Suman K.
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