posted by jim on .
assume that 44.3g Na2O are formed during the inflation of an air bag.How many liters of CO2-density=1.35g/L are needed to completely react with the Na2O?Explain
This reaction is unknown to me. Air bags typically are formed with N2 as the active gas. Do you have the reaction?
This is the entire essay question that was presented to me as an assignment.
It just asks how many liters of CO2(density=1.35g/L)are needed to completely react with the Na2O.
I can'y find help anywhere whis this question
Then I will assume that we are talking about Na2O + CO2 ==> Na2CO3 although I understand that airbags have KNO3 and SiO2 in order to react with the Na2O produced to produce products other than Na2CO3.
mols Na2O = 44.3 grams/molar mass = ?
Mols CO2 = mols Na2O
g CO2 = mols CO2 x molar mass CO2
volume CO2 = mass CO2/density CO2.