Today in class we performed a lab that was based off the law of conservation which states that matter can not be created or destroyed. We were given two beakers, one small and one big, the small one was to have anywhere between .5g to 1.25g of an unknown powder while the big one had two fingers of an unknown liquid. We were to record the mass of the beakers without the substances and we had to known how much of each substance we used. Then we massed the beakers with the correct substance in each beaker; after that we combined the powder into the liquid to watch the reaction take place. It immediately began to bubble and fizz as it turned a milky white color on top. During the chemical reaction it produced a gas which created a smaller mass than the original two components. Then after the reaction had begun to settle, we massed the beakers again. What we were looking for was the amount of gas produced; if you have more powder you will produce more gas and the less powder the less gas produced. In the lab there was a predictable relationship because you could add up the liquid and solid and subtract it by the final mass after the reaction and it would give you the amount of gas released.Matter is conserved in a chemical reaction because when adding up the amounts of each substance and the final mass of the mixture it is proven that the only matter lost was gas. In my group, our point was considered good but it had a higher gas produced than average since it was over the best fit line so it could have been better.When figuring the amount of gas that is released we got 44/88 grams of gas should be produced during the reaction in this lab. There were two ways to find how much gas was produced and one way was calculating and graphing the line of best fit and then finding the slope according to all of the results from each group. Our best fit line we got y=.4256x+.0834 which concluded that for every 1 gram of solid, you get .4265g of gas that is produced. Another way you can figure out the gas is setting up the chemical equation for this lab which is NaHCO3+HCH3COO=NaCH3COO+CO2+H2O which resulted in the mass of CO2 being 44 and the mass of the solid was 84. If .5g of a solid is used you can solve how much gas was produced by taking (44/84)x and plugging 5 into the x to get the answer or you could multiply .4256 by 5 to come up with how much gas was produced as well. The answer is 2.128 grams of gas would be produced and the answer to how much of the solid was used is .08512.; you solve this by dividing .4256 by 5 or the second way is by dividing 44/84 by 5.