Baking Soda Lab: Roshan Gill Background: In this unit, we began to learn about stoichiometry; where we measure and compare how many chemicals we have, before and after the reaction. Balancing moles and balancing equations are large components in setting up a problem. Another component that we have studied is the yield of reaction (how much product you get). When doing a stoich problem the amount of product you get is a theoretical yield. Your actual yield is the measurement you get using a balance. Baking soda plays a huge role in this lab. Baking soda’s chemical name is sodium bicarbonate, and its chemical formula is NaHCO3. In addition, it is used in making dough rise, making soda fizzy, and is inside of our toothpastes. So when we …show more content…
Grab a balancing scale 2. Measure the crucible with absolutely nothing inside it 3. Then pour in 3-5 grams of baking soda into the crucible 4. Measure the crucible with baking soda on the balancing scale 5. After recording the measurements in your journal, place the crucible with baking soda, on the ring stand, between the clay triangle 6. Set up the bunsen burner right under the crucible held between the clay triangle 7. Then turn on the gas for the bunsen burner 8. Use the striker to light up the bunsen burner and make sure the fire is slightly touching the crucible 9.. Let it sit for 30 minutes 10. Come back and close the bunsen burner 10. Pick up the crucible with tongs, and place it on the balance 11. Weigh the crucible with the decomposed baking soda 12. Record the measurement you have gotten into your journals 13. Subtract the weight of the crucible with the decomposed baking soda, with the weight of the empty crucible 14. Observe what has happened to the baking soda 15. Record physical observations you have noticed into your journals 16. Now begin to use this information in creating your stoich …show more content…
After being heated for 30 minutes it weighed only 2.4g. Our group’s goal was to find out the correct formula. So we used stoichiometry in order to find the theoretical yield for each equation. Then all we had to do was compare which theoretical yield would have the closest mass to the actual yield to find the correct formula. Our 2nd equation came closest to weighing the same amount of the actual yield. It weighed in at 2.5g while the actual was 2.4g. So this meant that the second formula was the actual yield. There is evidence for a pattern in chemical activity. The theoretical yields of all four problems have Sodium, but problems #1,#3,#4 have a lighter mass than equation #2. In addition the ones with more mass have a higher yield than the ones with less overall; this is because the gases in each theoretical yield are different. So this means that the mass of the gases in each yield differentiates between which one is the actual yield, and which one is
Then more roasting occurred when the crucible was placed into a ceramic triangle for the Bunsen burner to continue its burning for an additional 90 minutes. Once the burning was officially over, the crucible was placed onto a ceramic tile to cool off. Next the charcoal and copper material were poured onto a paper towel and were separated from carefully distinguishing them one from the other. Then comparisons were down through analysis of the copper (II) oxide smelted.
Coursework Equipment List • Boiling tubes (8) I will use these because this is where I will mix both the sodium carbonate and the strontium nitrate in order to form the precipitate. I need 8 because I am going to add 8 different amounts of strontium nitrate (1-8cm³) to the 8cm³of sodium carbonate. • Measuring cylinder (1) I will use this to measure the 8cm³ of sodium carbonate and the varying amounts of strontium nitrate to put into the test tubes. • Sodium Carbonate (enough to fill 8 boiling tubes with 8cm³/64cm³)
We had to mix baking soda, calcium chloride and water and then as a product we would have rocksalt and calcium carbonate, 2NaHCO₃+CaCl₂===>CaCO₃+CO₂+2NaCl+H₂O. We know that a chemical reaction took place because on the products into reactants equation the elements are equally transfered from one side to the other after the chemical reaction took place. We were given a plastic bag, that way we could do a closed experiment. We had to support that there were endothermic and exothermic reaction and that The Law of Conservation of Mass was present in this
Identification of an Unknown Compound using Quantitative and Qualitative Analysis Lauren Tremaglio Chemistry 1011 Lab, Section 16 Instructor: Steven Belina October 3, 2014 Our signatures indicate that this document represents the work completed by our group this semester. Experimental Design and Discussion of Results The objective of this experiment was to identify an unknown compound through quantitative and qualitative analysis. In order to find the identity of the unknown compound, an initial qualitative test for solubility was performed.
The last goal was to determine the percent yield of a product formed during a reaction with the unknown compound. Experimental Design The first day of lab consisted of various preliminary tests that helped identify the unknown compound.
Cassie Droelle 1510-01501 Chemical Equation 2 Visualizing Stoichiometry – Inquiry Lab Cassie Droelle 1510-01501 4-18-16 Introduction The purpose of this lab is to determine the complete balanced equation of a metathesis reaction with an unknown metal ion by first experimentally identifying the metal ion and then using stoichiometry to determine the rest of the equation. Stoichiometry is “the process by which quantities in a chemical reaction are compared” and is based on the Law of Conservation of Mass (1). The Law of Conservation of Matter “dictates that the mass of the reactants and mass of the products must be equal” (1).
Post Lab Questions: 2Mg + O2 →2MgO 0.29gMg 1molMg24.312molMgO2molMg100= 4.40molMgO ←theoretical yield 2Mg + O2 → 2MgO →2/24 =
First, you place the bunsen burner on the ring stand and tightly place the metal ring and place the clay triangle on it. Before placing the crucible on the ring you must put baking soda in the crucible, and place it on the ring stand. Then with safety precautions light the bunsen burner with the matches provided. In our first experiment we first started with 1.04 grams of NaHCO3 and ended with .60 g Na2CO3. In the second experiment we started with 3.2 g NaHCO3 and had a result of 2.0 grams
Percent yield = (mass of actual yield )/(mass of theorethical yield) ×100% ≐(1.22 grams)/(0.7066 grams) × 100% ≐
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
GRAVIMETRIC DETERMINATION OF MOISTURE AND PHOSPHORUS IN FERTILIZER SAMPLES Magdato, K. C. , Balbuena, J. S. Institute of Chemistry, University of the Philippines, Diliman Quezon City Date Performed: August 27, 29 and September 3, 2014 Date Submitted: September 10, 2014 Abstract The experiment aims to use gravimetric method of analysis in determining the moisture and phosphorus content in a fertilizer sample which is important in plant growth. The procedure included constant weighing of the crucible and sample. The addition of ammonia and magnesium sulfate heptahydrate caused the formation of the precipitate identified as magnesium ammonium phosphate hexahydrate(MgNH4PO46H2O).
Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g). The decomposition reaction was performed in a crucible and heated with a Bunsen burner.
(0.01 moles of NaOH) x (1 mole Ca(OH)2/ 2 moles of NaOH) = 0.005 moles of Ca(OH)2 Tube 1: (0.0020 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.002 moles of Ca(OH)2 (0.002 moles of Ca(OH)2) x (74.08 grams/mole) = 0.1 grams = theoretical yield Tube 2: (0.0035 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.004 moles of Ca(OH)2 (0.004 moles of Ca(OH)2) x (74.08 grams/mole) = 0.3 grams= theoretical yield Tube 3 (0.0050 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.005 moles of Ca(OH)2 (0.005 moles of Ca(OH)2) x (74.08 grams/mole) = 0.4 grams =theoretical yield Tube
PROCESSING OF BISCUITS Mixing: Creaming- The ghee, sugar and vanilla flavor is churned so that flavor may get adhered to the fine droplets of fat. Mixing time is of two minutes.
Ignite the dish again for about 30 minutes, cool and weigh. Repeat this process till the difference between two successive weighings is less than 1 mg. Note the lowest