The question I was trying to answer is Which balanced chemical equation best represents the thermal decomposition of sodium bicarbonate. Using that question to guide us we were trying to determine which of the four chemical equations show how atoms are rearranged during thermal decomposition. We concluded it was the second chemical equation, we know that because: During our investigation we first decided how much sodium bicarbonate we would be using. We decided on 11 grams which was about half of the crucible. We then used the bunsen burner to heat up the sodium bicarbonate. We heated the sodium bicarbonate expecting there to would be a chemical reaction and the atoms would be rearranged during thermal decomposition. We heated the sodium
Each subsequent trial will use one gram more. 2.Put baking soda into reaction vessel. 3.Measure 40 mL vinegar. 4.Completely fill 1000 mL graduated cylinder with water.
The theoretical weight was 599.6 mg. This yields a percent yield of 3.7%. Table 1 also illustrates the experimental melting point of 99.3-102.1◦C. A melting point that has a range larger than 3◦C is indicative of impurities in the sample. A few possibilities of impurities could have been unreacted norbornene, and water. Evidence that supports that there was unreacted norbornene in the final sample was the fact that the product was a jelly-like structure. Norbornene by itself has a jelly-like structure. However, once norbornene reacted with the acid-catalyst (H2O2), then it should have changed the chemical structure of the molecule and once the solution was brought back down to room temperature, crystals should have formed. Since a jelly-like, or oil-like product was present at the end of the reaction, then this is indicative that there was unreacted norbornene in the sample. The second impurity that may have been present in the final product was water. Instead of adding 3 mL of sodium bicarbonate and then 3 mL of brine, 3 mL of brine was added first and then 3 mL of sodium bicarbonate was added. This experimental error caused excess aqueous solution to be added to the diethyl ether. Since excess water was added to the final product, about 4x the amount of anhydrous sodium sulfate was needed in order to remove the water from the product. This was another indication that there was too much water in
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
Procedure: Anisole (0.35mL, 0.0378mol) was obtained and placed in a pre-weighed 25 mL round bottom flask, along with 2.5 mL of glacial acetic acid and a magnetic stir bar. Then the reaction apparatus was assembled, the dry tube was charged with conc. sodium bi sulfate, the 25 mL round bottom was attached to the apparatus, and 5 mL of Br2/HBr mixture was obtained and placed in the round bottom. The reaction took place for 20 minutes. An orange liquid was obtained and placed in a 125 mL Erlenmeyer flask along with 25 mL of water and 2.5 mL of conc. Sodium bisulfate soln. The solution was then placed in an ice bath to precipitate and then the solid product was filter in a Buchner funnel. These crystals were then re-dissolved minimum amount of hot solvent (heptane) and recrystallized. Once a dry product was obtained, a melting point was established (2,4-Dibromoanisol mp 55-58 C) and percent yield was established (52%).
Experimental: The experimental procedure outlined in the OU Physical Chemistry Laboratory Manual was followed without any deviations.
Baking soda is a white crystalline powder better known to chemists as sodium bicarbonate. Bicarbonate of soda sodium hydrogen carbonate. The native chemical and physical properties of “baking soda” account for its wide range of applications cleaning deodorizing, buffering, and fire extinguishing. Baking soda can neutralize chemical smells and all types of other smells.
By this I mean that we will set up the apparatus in a way that would give us a large temperature rise in a short amount of time, e.g. 2 or 3 minutes. Then the s Here is a diagram of how we set up the apparatus. To perform this experiment we needed. * Electric weighing scales * A measuring cylinder 5 spirit burners (1 for each fuel). * A copper calorimeter with a lid *
The Enthalpy Values for the Reaction Between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride
In this experiment, we will look at the concentration of sodium bicarbonate in the light reaction of photosynthesis. This will be carried out using three different colored filters to identify the effect on the light reaction of photosynthesis. Since, photosynthesis is the process whereby light energy is captured by plant, algal, or bacterial cells and is used to synthesize organic molecules from carbon dioxide and water. Although, photosynthesis is atmospheric carbon dioxide is removed and transformed into oxygen and carbohydrates. Elodea is an aquatic plant of a genus that includes the ornamental waterweeds. Sodium bicarbonate is commonly known as baking soda. On the other hand, there are four primary photosynthetic pigments found in the chloroplast
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
It's impressive. That. One. Last. Molecule. And everything as it was will seize and transform. Precision amongst what seems to be chaos, something new is born from that calculated dance. I've often had to covertly wipe the tears from my eyes as I sit, surrounded by my seemingly unmoved peers (academy awards should be handed out if I misjudged even the smallest nuance of tension in their foreheads and strain in their eyes as anything other than confusion), listening to a lecture about how this is more reactive than that, how this repels or attracts that, how bonds are formed, broken, their strength, and how usually heat, hot hot heat activates transformation and gives birth to something different, old things made anew, and how cooling down, by removing heat can suspend a process, and sometimes you can control what the outcome is, other times you have to dispose of it all, placing the waste in the proper receptacle using the appropriate means bc haphazardly submerging it under water in the sink will only cause more problems involving words like purge and evacuate. I often wonder if anyone would understand if I followed through with the compulsion to shout, "Preach!" (lol) as my professor droned on. Sometimes I think abt bringing these things up among my peers (secretly, with hopes that I can meet my future
The Enthalpy Change of the Thermal Decomposition of Calcium Carbonate. Results: The 'St For CaCO3: T1 = 17. T 2 = 19 DT = 02 using 2.57g of CaCO3. For CaO: T1 = 18.
The crucible and lid are heated at the beginning of the experiment before being weighed so that any moisture in the crucible is burned away.
Www2.estrellamountain.edu, (2014). CHEMISTRY I: ATOMS AND MOLECULES. [online] Available at: http://www2.estrellamountain.edu/faculty/farabee/biobk/biobookchem1.html [Accessed 20 May. 2014].
And the symbol equation for it is:. Na2S2O3 + 2HCl, S + SO2 + 2Na + H2O. Before conducting my experiment, I will research into, amongst other things, the factors that affect the rate of a reaction. This is so that I may have enough information to understand the effect of temperature on the rate of a reaction and also gain appropriate understanding to make a suitable prediction as to what the outcome of my experiment will be. Reactions occur when the particles of reactants collide together continuously.