Gas Laws and Stoichiometric Calculations - Essay Example

The data relating to the first two trials of H2 was not considered for the fact that the gas had gotten away from the flask; that is why the average of H2 produced in moles appears lesser than moles of CO2 produced.

The reaction of Mg and HCl gave a more ideal gas product than the gas product from the CaCO3 reaction. The Ideal Gas Law has its limitations in assuming that the gas particles do not attract each other and they do not have any finite volumes. These assumptions explain the difference between actual yields and the theoretical yields of the gases. If the van der Waals equation is to be used for calculations then the difference will significantly narrow down because the equation bears in mind the volumes and attraction of the gas particles.

Gas particle leakages further explain the inaccuracy of the results. It would be appropriate to repeat the experiment with the correct volume of the gas in the system to eliminate this discrepancy.