The law of conservation of mass was discovered by Antoine Lavoisier many years ago. He claimed that “mass is neither created nor destroyed in chemical reactions.” This is the law of conservation. He came to this conclusion by burning phlogiston. Lavoieror took note that by burning phlogiston it lost its phlogiston and made new things. Not only was Lavoisier a chemist, he had many other jobs that may have helped him discover many of the thing that he did. He was eventually killed by getting his head cut off. This happened to him because of many reasons including building a wall around Paris and being a tax collector, and supporting the French revolution. Lavoisier discovered that mass is neither created nor destroyed in chemical reactions. …show more content…
Our experiments’ mass decreased by 3.64% after the reaction. The final balanced equation for this experiment is CaCL2 + 2NaHC3+ H2O = 2NaCl + CaCo3 + Co2 + 2H2O. This balanced equation supports The Law Of Conservation of mass because the mass was only changed by 3.64 which is less than 5%. The experiment being kept in a tight plastic bag, which was a closed system for the reaction to occur helped the mass to be as accurate as possible. The closed system made sure that no other things around the experiment could exchange matter with it. If the bag was opened at all then there would be a higher percent …show more content…
Four of these include the release of energy, which occurred during the reaction, the substance got hot. Change is color, it turned into a yellowish white color after the reaction. There was a change is smell, it smelled like salt mixed with water. And lastly there was a change in state of matter. While the experiment was reacting it was in closed system, the experiment ended up puffing up. The indicator solution made this occur. It caused the bag to puff up because it has high acidity levels and when mixed with the baking soda. This reaction was a exothermic reaction because heat was given off of the experiment. The catalyst or what caused the reaction to start was the indicator solution. This is because once the indicator solution was tipped over the reaction
In addition, a significant amount of liquid leaked out of the 3% and 5% vials. Each vial had an initial air bubble, so that had to be measured and accounted for. As time progressed, there became a wider gap between the 3% and 5% and the 1% and control solutions. As the reaction was taking place, it was evident CO2 was being produced due to the presence of air bubbles. The rate of reaction for 1% was 84.8 mm3/minute, for 3% it was 229.9 mm3/minute, for 5% it was 186.6 mm3/minute, and for the control it was
The experiment is done by reacting the CaCO3 with hydrochloric acid whilst a balance records any change in mass during the set amount of time. The speed of the reaction can be measured by measuring how quickly the carbon dioxide escapes and this is done by weighing the contents of the beaker. When the two are mixed together calcium chloride water and carbon dioxide are produced as shown below in the equation of the reaction: [IMAGE]Calcium Carbonate + Hydrochloric acid Calcium chloride + Carbon dioxide + Water [IMAGE]CaCO3 + HCL CaCl2 + CO2+ H2O This experiment is done by conducting the reaction in an open flask on a balance. Readings will be taken from the balance every 60 seconds, then from those readings we will be able to plot a graph showing loss of mass against time.
In the experiment when we combined yeast with other materials such as water, grass, sugar, and cornmeal, it reacted creating CO2. When this reaction happened it caused the Ziploc bags to blow up and fill with many air bubbles. In our group, bag A which contained yeast and water rose the most. Its final
water inside of the popcorn heated up and turned into gas, the popcorn popped releasing
The results from the experiment show that the Law of the Conservation of Mass is correct in the two different experiments. The experiment in an open environment showed that the mass will always stay the same when vinegar and sodium hydroxide react with each other. The mass of each substance was calculated before the reaction, and after the reaction, the mass of the reaction was the same and no mass was lost. In the closed environment experiment that provided gas, the amount of gas complimented to the mass of the other substances and showed that no mass had been destroyed or created. These results prove the hypothesis as the mass of both substances were predetermined before the reaction and proved the mass stayed the same throughout the
I. Purpose We did this experiment to learn how to use stoiciometry with the ideal gas law to figure out the amounts of substances within a compound. II. Hypothesis
The purpose of the Decomposition of Baking Soda Lab was to find the correct formula with the right products, for when baking soda is heated. Scientists hypothesized that when baking soda is heated sodium hydroxide and carbon dioxide would be formed. To test this hypothesis, 2 grams of baking soda was placed into a beaker and then placed on a hot plate set to its highest temp. To do these scientists first had to measure the beaker to subtract its mass from the total of it with baking soda. Both masses were then subtracted to find that the baking soda mass after the experiment the new mass being 1.29 grams. Later the scientists balanced three given equations to find the coefficients and then used those to solve three mass-mass problems. The mass-mass
combustion, his development of a way to classify the elements and the first modern textbook of chemistry led to his being known as the father of modern chemistry. He contributed to much of the research in the field of chemistry. He is quoted for saying, "Nothing is lost, nothing is created, everything is transformed." Lavoisier was born in Paris, France on Aug. 26, 1743. When he was eleven years old he attended a college called Mazain. For Lavoisier's last two years in college he found a great deal of interest in science. He received an excellent education and developed an interest in all branches of science, especially chemistry. Abbe Nicolas Louis de Lacaill taught
Mass of baking soda(g) Mass of crucible and compound after heating (g) Mass of compound after heating (g) 12.42 17.43 5.01 15.58 3.16 (kg) 0,01242→ 0,01 0,01743→ 0,02 0,00501→0,005 0,01558→0,02 0,00316→0,003 Data processing: Balanced equations: 4NaHCO₃ → 2Na₂O + 2H₂O + 4CO₂ NaHCO₃ → NaOH + CO₂ 2NaHCO₃ → Na₂CO₃ + H₂O + CO₂ Molar mass of baking soda: NaHCO₃ Na → 22.989770 H → 1.00794 C → 12.0107 O → 15.994 22.989770+1.00794+12.0107+15.994*3=84.00661 g/mol M =m/n n=m/M m=n*M Na₂O mass: Na-Sodium Atomic weight →22.98976928
Antoine Laurent Lavoisier is thought to be the father of cutting edge science. He unbelievably affected the way the world sees science today. From distinguishing components to finding the significance of combustion, he had a fundamental influence on many logical thoughts and innovations of the world. He was influential to the point that he is said to have an equivalent if not more prominent effect in science as Newton did in physics. Due to these achievements, he is viewed as one of France's and the world's most exceptional researchers.
We observe the color of the solution before adding the sandwich bags to each cup because
I claim, in line with Paul Walden, that “No single man is entitled to the be called the “father of chemistry.” I will look at Lady Ranelagh’s chemical recipe book in relation to The Elements of Chemistry and, by doing so, I will argue that Lavoisier, as a chemist, is not revolutionary, but is, rather, in continuity with the chemical and alchemical tradition that precedes him. First, I
In any reaction, the Law of Conservation of Mass is applicable. This law ensures that the mass of a given reaction is the same in the beginning as in the end. To confirm that no mass
Law of Conservation of Mass The Law of Conservation of Mass states that mass is an isolated system, it is neither created or destroyed. It also states that the mass of the products in a chemical reaction must be equal to the mass of the reactants. All of our experiments in chapter two had to do with mass and in every experiment we found the mass of the reactants and the mass of the products and in each one there wasn’t a significant change in mass. Antoine Lavoisier was the one who introduced the Law of Conservation of Mass. Lavoisier ran many experiments and he was famous for his accurate observations and his insistence on careful measurements. He used accurate balances that could measure very, very small changes in his experiments.
t = time, a = volume of reactant, k is a constant of proportionality; x is the order of reaction. Because k is a constant of proportionality 1/t is directly proportional to the rate of reactant. Then to find out the order of reaction in a catalysed system the volume of ammonia molbydate is varied and the concentration of the other reactants kept the same. Thirdly to investigate the activation energies, the concentrations are kept the same and the temperature is varied.