Kinetics Rate Of Reaction

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The study of stoichiometry is a branch off Chemistry its the study of the amounts of substances that are involved in reactions. For this experiment kinetics is a huge part of it. Kinetics is explained as the reaction speed and or rate of reaction. To observe these reactions made by having reactants, sodium hydrogen carbonate, NaHCO3 known as baking soda and acetic acid, CH3COOH that is vinegar being mixed together. The products were carbon dioxide, water, and sodium acetate. Because this reaction will be based on its speed according to the difference in temperature, the higher the temperature the faster the reaction will occur creating a direct relationship. The balanced equation is as follows:

NaHCO3 (aq)+ CH3COOH (aq) →
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Hypothesis: Increasing the temperature of Hydrogen Carbonate and Acetic acid should result in a faster rate of reaction (faster production of H2O, CO2, and C2H3NaO2). This is because when the temperature increases of the solution, the faster the particles move the more frequent the collisions between reactant particles.

Safety precautions: When dealing with these solutions there isn’t very much to worry about, as the solutions are things that are worked with daily. These are water, vinegar, baking soda, and carbon dioxide. However when dealing with the hot plate gloves should be worn and the beakers needed to be carried with carefulness, as the beaker will be hot after being on the hot plate. When dumping the liquids in the sink there isn’t any problem except the heat of the beaker. It is recommended to wait till the beaker cools down so it will be easy to handle the
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Once it is set, acquire a weigh boat and add 4.2 grams of baking soda to the weigh boat. After doing so repeat steps 1 and 2, four more times, which would mean five weigh boats of 4.2 grams of baking soda. Once that is completed, place the weigh boats somewhere safe and move on to part 2.

Part 2: Preparing the Acetic acid Wash the 100mL-graduated cylinder and dry it with paper towels. Then get the Acetic acid and pour exactly 100mL of it into the graduated cylinder (This should almost fill it up). When that is completed repeat steps 1 and 2 four more times, which would mean five graduated cylinders of 100mL of Acetic acid.

Part 3: Carrying out the reaction Wash the 250mL-beaker and dry it with paper towels. Add one of the 4.2 grams of catalyst (Sodium Hydrogen Carbonate) that has been obtained in step one into the beaker. Making sure that the beaker is dry before hand. Get the stopwatch ready to record the time of the reaction. Apply one of the 100mL Acetic acid into the beaker and start the stopwatch as soon as the two substances meet. Record the qualitative data observed in the

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