Question

An experiment being conducted, the pressure is 0.9 atm and the temperature is 18 ° C. One of the steps of
experience requires the combustion of 500 ml of ethanol (d = 0.78 g / ml). Whereas the burning this amount of ethanol does not significantly alter the enviroments conditions, but releases carbon dioxide. Calculate the volume of CO2 generated (in L) and the CO2 concentration in mol / L

Answer 1

C2H5OH + 3O2 ==> 2CO2 + 3H2O

Determine mass ethanol from density.
mass = volume x density
mass = approx 400 but you need a more accurate answer than that.
mols ethanol = grams/molar mass = about 9 mols. Again you need to confirm an accurate answer.
For every 1 mol ethanol burned you get 2 mols CO2 so mols CO2 produced = approx 18.

Use PV = nRT to calculate volume in L.
(CO2) = mols/L. Plug in your value for mols and L to solve for (CO2).
Post your work if you get stuck.

Answer 2

and molarity of CO2 ?

Answer 3

I did that above.
(CO2) is read as concentration of CO2 in mols/L = M

Answer 4

Thank you :)