Mukund Balaji, Jacob Jiang, Carolyn Zheng Honor Chemistry Mrs. Marino May 1, 2023 Thermal Decomposition of Sodium Bicarbonate Introduction: In this experiment, heat is added to a compound known as sodium bicarbonate, or in a chemical sense, NaHCO3. This compound is also known as baking soda in a domestic setting and has several uses due to its chemical nature. This lab tests the thermal decomposition of this compound by heating this compound under a Bunsen burner. There are four possible equations that will theoretically be used. These equations are as follows: NaHCO3 (s) → NaOH (s) + CO2 (g) 2NaHCO3 (s) → Na2CO3 (s) + CO2 (g) + H2O (g) 2NaHCO3 → Na2O (s) + 2CO2 (s) + H2O (s) NaHCO3 → NaH (s) + CO (g) + O2 (g) This lab will determine the correct …show more content…
Light the Bunsen burner. Heat the crucible for two minutes and then turn off the Bunsen burner. Wait for the crucible to cool to room temperature. Measure and record the mass of the crucible Keep the crucible on the mass balance and tare the mass balance. Pour about 2.00g of sodium bicarbonate (NaHCO3) into the crucible. Measure and record the actual mass of the sodium bicarbonate. Place the crucible with sodium bicarbonate onto a ring clamp above the bunsen burner. Light the Bunsen burner. Heat the crucible for 15 minutes and record any observations. Wait for the crucible to cool to room temperature. Measure and record the mass of the crucible and its contents. Place the crucible back on the ring clamp. Heat the crucible again for 2 minutes. Rerecord the mass of the crucible and its contents. Repeat steps 14-16 until the difference between the existing and new measurements is lesser than 0.02 grams. …show more content…
To begin with, the fact that the mass was reduced shows that there is some sort of reaction that did take place. In all cases of reactions, the law of conservation of mass states that mass cannot be created or destroyed. With this in mind, it can be concluded that the mass that was “lost” was transferred into a different substance, which in this case was carbon dioxide and water vapor. These substances, as they are in their gaseous state, do not remain in the crucible, and escape into the surrounding area. This situation causes a reduction in the mass of the sodium
Click here to unlock this and over one million essaysShow More
Modifications of this procedure include the use of hot plates instead of Bunsen burners, and heating t-butyl alcohol to 60-65 ℃ instead of 50 ℃. Other modifications include the use of weighing boats to measure an amount of unknown instead of weighing paper, and completing one run of unknown 2 instead of two runs of unknown 2. Summary of
Once all the information was gathered over the block, it was determined to be copper. The block was heated in water to 99℃ then put into a calorimeter with room temperature water. Once the temperature of the block in the calorimeter was taken, the specific heat was able to be calculated. With the information found the specific heat of copper is 0.349 j/g℃. When researched the specific heat of copper is very close at 0.385 j/g℃.
After we put the substance on the burner, we weighed it. Each time after we put it on the burner came with the exact same number: 21.16 grams. After we found the mass of the crucible, cover, and hydrated sample, and the mass of the crucible, cover, and dehydrated sample, we subtracted the two values to get the mass of water evolved: 0.24 grams. Then, we subtracted that value to the mass of the hydrated sample to get the mass of the dehydrated sample: 0.76 grams.
Put the beaker with the water and the metal on the wire gauze of the ring stand that has the bunsen burner under it. Fill the graduated cylinder with enough water to about fill the calorimeter and record the amount of water and the temperature of the water that is in the graduated cylinder. When the water starts to boil in the beaker, use the thermometer to record the temperature of the water. Pour the water from the graduated cylinder into the calorimeter. Use the crucible tongs to take the metal out of the beaker and place the metal into the calorimeter and close the
Next, fill the graduated cylinder with water, then put a hand over it and flip into the pneumatic trough. While doing this step make sure the least bubbles get in. This can affect the results of the experiment. Stick the tubing into the cylinder and put the sodium bicarbonate into the side arm erlenmeyer flask. Put the other end of the tubing on the erlenmeyer flask.
Monitor the reaction and when when the reaction is near completion let some smoke escape by tilting the lid of the crucible When the reaction ceases, turn off the Bunsen burner and let the crucible cool completely before handling it. Weigh the crucible and record the weight Using a pipette, add a small volume of water to the solids in the crucible Stir the mixture with a glass rod until the mixture forms a paste Return the crucible to the Bunsen burner and heat it for several minutes until all the water has evaporated and the solids have turned light grey → indicating conversion to magnesium oxide. Turn off the Bunsen burner and let the crucible cool completely Weigh the crucible with the lid and record the weight Subtract the initial weight of the crucible and lid from the final weight of the crucible, lid, and magnesium oxide to obtain the mass of magnesium that reacted with oxygen. → this information will be used to calculate the empirical formula for magnesium oxide and prove it. Clean the crucible thoroughly to ensure it's ready for the next use.
The evaporating dish was placed on top of the wire gauze and covered with the watch glass. The Bunsen burner was used to heat the water to a boil until the water had evaporated, leaving a dry, white solid (salt). The evaporating dish with the watch glass containing the salt residue was then weighed and recorded to 0.001 g. The mass of the evaporating dish and watch glass containing the salt residue was subtracted from the mass of just the evaporating dish and watch glass which gave the mass of the
Decomposition of Baking Soda Lab Introduction Chemical reactions are essential to the understanding of chemistry, and arguably the least straightforward type of chemical reaction is decomposition. The main reason for this difficulty is that a single compound can feasibly decompose in many different ways. An example of this is NaHCO3, more commonly known as baking soda, which can hypothetically decompose in three different ways, each leaving different solid products: NaOH, Na2O, and NaCO3. Our goal for this lab was to determine which of these decomposition reactions actually occurs. The way we did this was by using a chemistry principle called stoichiometry.
The scientist recorded the mass of the Sodium Hydroxide in the data table. After the mass gets recorded, the scientist takes the graduated cylinder off the scale, while the Sodium Hydroxide remains in the graduated cylinder. Next, the scientist took the beaker and the test tube and placed the two materials on the digital scale. The scientist pressed the zero on the digital scale to zero out the scale. While the materials stay on the scale, The scientist took the pipette and filled the pipette up with Copper Nitrate.
To do this you first have to place the weighing boat on the scale and hit tare, so it reads zero and then place copper(II) sulfate pentahydrate on the weighing boat. Transfer the copper(II) sulfate into a 250-mL beaker. Rinse the weighing boat with 5 mL of purified water in small quantities to rinse off leftover chemical into the beaker. Spin the beaker gently to dissolve the solid. Rinse the sides of the beaker with small amounts of the 5 mL of purified water.
Heat the solution until it is at 100 ˚C then continue heating for 75 minutes. Evolution of CO2 and NH3 is observed during heating. e. After 75 minutes of heating, stop stirring. Draw a little clear solution with a pipette, cool the solution to room temperature and measure its pH value with pH paper.
the triple beam balance scale to measure the mass of the cup and the jar 3.Mix sugar and water in a beaker 4.Place the mixed solution onto a hotplate 5.Stir the solution 6.After stirring measure the temperature of the solution 7.Create a cross with
The Effects of Acetic acid on Sodium Bicarbonate Introduction: Acids and bases are one of the main components of chemistry. They are both substances with unique chemical properties and can use them to neutralize each other. An acid is any substance that produces positively charged hydrogen ions when reacting to a solution containing water. However, a base is a substance that neutralises positively charged hydrogen atoms, which is the reason why an acid and base always form a salt and a water, In this experiment, sodium bicarbonate ( a base) will be combined with vinegar ( an acetic acid) to form Co2 bubbles.