In this mini lab our chemistry class experimented with different white powders and liquids that when mixed together produced a gas. First it was vinegar and sodium bicarbonate. The result was fizzing which produced a gas. We had 1.405g of sodium bicarbonate, which when added to the vinegar produced 1.587g of CO2. We also had a percent error due to the fact that the solution fizzed over the top onto the table which caused a larger amount of gas to be recorded because that mass was lost from the mixture. We did this similar experiment three different times with 3 combinations added together. The result always being a 1:1 molar ratio. This means for every 1 mole of powder used, there should be one mole of gas produced. With the exception of the last experiment, all the experiments had this quality. For the last equation we had to balance the compounds. We put 2’s in front of NaHCO3 and CO2. This resulted in a 2:2 molar ratio because we had to balance the equations. Now this ratio does not apply to all chemical equations. Each different combination of compounds will have a different reaction causing more or less gas. But for that equation the theoretical ratio should be constant. There is a molar relationship between the two substances. Although it may change, there is always a line of best fit that tags along with the data. The theoretical relationship you should calculate with every experiment demonstrates the precise ratio one should get when doing the experiment.