Please, help! Chemistry problem help

You carefully measure 19.00 g of powder and add it to 76.95 g of solution in a reaction flask of known mass. You notice bubbles as a reaction takes place. You then determine that the contents of the flask have a mass of 88.16 g. The relevant equation is
Assuming no other reactions take place, what mass of CO2 was produced in this reaction?
Chemical formula is: CaCO3+2HCl-->H20+CO2+CaCl

I am so lost, we've just started covering stoichiometry and I understood everything in the chapters and then WHAM, this. :( Please explain?

CaCO3(s) + 2HCl --> CaCl2 + CO2 + H20

Actual moles of CaCO3 : 19 / 100 = .19 mol
Theoretical mass of HCl: 2 *.19 * 36.5 = 13.87g ( < actual mass of 76.95g)
Thus CaCO3 is limiting reactant!
Mass of CO2 produced: .19 * 44 = 8.36 g

Find the limiting reactant first:

CaCO3(s) +2HCl(aq) >>>>>>>>>>>> H2O(g) + CO2(g) + CaCl2(aq)

mass HCl required = (19.00 grams CaCO3) * (1 mol CaCO3 / 100.09 grams CaCO3) * (2 mol HCl / 1 mol CaCO3) * (36.453 grams HCl / 1 mol HCl) = 13.84 grams HCl required.

This means HCl is the excess reactant, and CaCO3 is the limiting reactant.

mass CO2 produced = (19.00 grams CaCO3) * (1 mol CaCO3 / 100.09 grams CaCO3) * (1 mol CO2 / 1 mol CaCO3) * (44 grams CO2 / 1 mol CO2) = 8.35 grams CO2