Problem: The stratospheric ozone (O3) layer helps to protect us from harmful ultraviolet radiation. It does so by absorbing ultraviolet light and falling apart into an O2 molecule and an oxygen atom, a process known as photodissociation.O3(g) → O2(g) + O(g)Use the data in Appendix C in the textbook to calculate the enthalpy change for this reaction.

🤓 Based on our data, we think this question is relevant for Professor Freeman's class at UNC.

FREE Expert Solution

Balanced reaction:

O3(g) → O2(g) + O(g)


Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved:

H°rxn=H°f,products-H°f,reactants


View Complete Written Solution
Problem Details

The stratospheric ozone (O3) layer helps to protect us from harmful ultraviolet radiation. It does so by absorbing ultraviolet light and falling apart into an O2 molecule and an oxygen atom, a process known as photodissociation.
O3(g) → O2(g) + O(g)

Use the data in Appendix C in the textbook to calculate the enthalpy change for this reaction.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Freeman's class at UNC.