From this experiment, we all measured the mass of 4 vapors; oxygen, carbon, helium, and lab gas. We took a Ziplock bag, and converted into a non-stretchy balloon, and filled with every gas and measured the apparent mass then computed the actual mass, then find a ratio between mass of oxygen plus the other gasses. We attempted to keep the pressure about the same each time so each of our calculations would be more accurate. We all found out the heaviest was carbon dioxide, and the lightest was helium. In fact , helium and lab gas had a density below 0. Anyways, it had been that our obvious masses were very different from our actual mass calculations; one example is oxygen's obvious mass was 28. 33g but its real mass was 4. 10g. We also available the percentages, and after collecting class data, our carbon dioxide ratio was 1 . 39/1g, our helium ratio was. 21/1g, and our research laboratory gas percentage was. 59/1g. Then there were to come up with two hypotheses to figure out why one particular gas is heavier (denser) than another? Well, we all came up with hypothesis #1: The several molecule mass hypothesis, and hypothesis #2: The more substances in the same volume hypothesis. After having a class discussion, works out that speculation one is more reliable due to Avogadro's hypothesis; in the event that two vapors at the same temperatures and similar volume have equal volume of molecules. So in line with the statement over, the co2 molecules must be 1 . 39x bigger than an fresh air molecule, a helium molecule must be. 21x bigger, and. 59x bigger than a great oxygen molecule.