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 25.0 mmHg and a temperature of 235 K can be destroyed when all of the chlorine from 15.5g of CF3Cl goes through ten cycles of the above reactions?
Reaction Stiochiometry Involving Gases - bobpursley, Sunday, October 25, 2009 at 1:59pm
how many moles of CF3Cl are in 15.5 grams?
I appears to me that two moles of ozone per cycle are destroyed per one mole of CF3Cl