Problem: Ozone is depleted in the stratosphere by chlorine from CF3Cl according to the following set of equations:CF3Cl + UV light → CF3 + ClCl + O3 → ClO + O2O3 + UV light → O2 + OClO + O → Cl + O2What total volume of ozone measured at a pressure of 25.5 mmHg and a temperature of 226 K can be destroyed when all of the chlorine from 15.5 g of CF3Cl goes through ten cycles of the above reactions?

FREE Expert Solution

Concept: Ideal Gas Law with Stoichiometry.

First find the overall reaction per one cycle.

Next calculate the moles of O3 consumed per 1 cycle of reaction.

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Problem Details
Ozone is depleted in the stratosphere by chlorine from CF3Cl according to the following set of equations:

CF3Cl + UV light → CF3 + Cl
Cl + O3 → ClO + O2
O3 + UV light → O2 + O
ClO + O → Cl + O2

What total volume of ozone measured at a pressure of 25.5 mmHg and a temperature of 226 K can be destroyed when all of the chlorine from 15.5 g of CF3Cl goes through ten cycles of the above reactions?

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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 Gas Stoichiometry concept. You can view video lessons to learn Gas Stoichiometry. Or if you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

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