Name: Ashrith Epuri Lab Members: Ian, Averi, Serena Percent Yield Lab Objective: Determine the percent yield of NaCl in a chemical reaction. Materials: Evaporating dish Watch glass Digital balance Sodium bicarbonate Wire mesh Scoopula Plastic pipette Hydrochloric acid Hot plate Crucible tongs Methods: First, the mass of the empty, clean, and dry evaporating dish and watch glass was recorded using the digital balance, while the hot plate was set to 450 degrees Fahrenheit. 1 gram of sodium bicarbonate was added into the evaporating dish and the mass was recorded again. A plastic pipette was used and filled with HCl, which was added to the sodium bicarbonate. The two reactants, NaHCO3 and HCl, were mixed together and the reaction was observed. …show more content…
During the reaction, NaHCO3 and HCl fizzed and bubbled when reacting. Both reactants started to condense, and vapor and steam were present as the dish became foggy. Intense bubbling occurred and steam escaped from the evaporating dish. After heating, NaHCO3 and HCl started to solidify and dried …show more content…
The addition of HCl to NaHCO3 causes a rapid release of CO2 gas and the reaction also produces NaCl, which remains dissolved in the aqueous solution. After the reaction in the lab was complete, the evaporating dish contained a mixture of NaCl and excess water. The water needed to be removed to isolate the NaCl product, which was done by heating the evaporating dish to evaporate the water, causing a lot of steam to form inside the evaporating dish.. Once the water was evaporated, only the solid NaCl product remained in the evaporating dish. The mass of the NaCl product is used to calculate the percent yield of the reaction, a measure of how efficient the reaction was in producing the desired product. This lab demonstrates the concept of limiting reactants because the amount of product that can be produced is limited by the amount of reactant that is present in the smallest amount. The reactant that is completely consumed is the limiting reactant, and the amount of product that can be produced is determined by the amount of limiting reactant present. In this reaction, HCl was added in excess and NaHCO3 was the limiting
conclusion: The results show that when sodium bicarbonate is heated, it decomposes to form sodium carbonate (1.51g), and carbon dioxide gas. This is most likely because the percent yield was only 3.1% off. Sodium carbonate is known to be a solid crystal substance which agrees with the crystal structure substance formed on the crucible furthering the idea that sodium carbonate actually formed. We could have also tested this by dropping water onto the substances produced to see if it dissolves or not since sodium carbonate dissolves in water. In this experiment NaHCO3 decomposes into Na2CO3, CO2 and H2O when heated.
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.
Lab 27. Stoichiometry and Chemical Reactions Report In our lab we were asked Which Balanced Chemical Equation Best Represents the Thermal Decomposition of Sodium Bicarbonate. Sodium Bicarbonate is a chemical compound with the formula NaHCO3, also known as baking soda. In the process to answer our guiding question we have to determine how atoms are rearranged during a chemical reaction.
Procedure The various solids and liquids were used for this lab. The first experiment had effects of the temperature towards the chemical reaction. The first experiment had two test tubes filled with same amount of substances to react, but one was at 10 ºC while the other one was at 50 ºC. The second experiment involved different molar concentration of substances reacting. Individual test tube was filled with 1.0,
After the reaction finishes, the amount of CO2 that was released is calculated and then using the molemap, it is possible to solve for the amount of the unknown substance. The grams of the unknown powder are then divided by the moles of the substance to get the molar mass. This molar mass is then compared to the molar mass of the known substances. Unknown substance A is lithium carbonate since the molar mass produced in the experiment is 66.68 g/mol and the molar mass of lithium carbonate is 73.89 g/mol. Unknown substance B has a molar mass of 146.70 g/mol which is inconclusive since it is too different from the other molar masses.
Using this number as well as the theoretical yield, the percentage yield was calculated and can be seen below in Figure 5. % Yield: (0.1805 g)/(0.3064 g) x 100 = 58.92% Figure 5: The calculations of the percent yield. The percentage yield was calculated to be 58.92% and this represents that a portion of the reactants were lost during the experiment due to a small spill or improper collection of the product during the purification process. Next, the spectrum of the product was obtained.
Then, using two coffee cups, observe the temperature increase from the first thermometer in the calorimeter. After it has stopped increasing, record the final temperature. Next, weight a small portion of your unknown sample and record the mass and place it in the water bath for ten minutes and record the temperature. Pour the unknown element into the calorimeter. Monitor the temperature and record it in the data table.
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
The needed mass for reactant A was 3.52 grams and the needed mass for reactant B was 2.12 grams. The moles of product C (CaCO3) were also required to have been calculated using mass- to- mole conversion, but the mass was already established, so its mass was not calculated. Results Calculations used to determine the percent error 2.3 g CaCO3 - 2.00 g CaCO3 2.00 g CaCO3 x 100 = 15 % Reactants A and B’s masses were not similar, but the numbers were also not drastically different. Obviously, product C’s solution is different because moles were calculated as opposed to a mass.
In this experiment, groups were given two different unidentified substances with the goal of being able to figure out what chemical each substance was. Unidentified substance “2” was proven to be Tin (II) Chloride and the Unidentified substance “4” turned out to be Sodium Chloride. The conclusion that substance “2” was Tin (II) chloride could be proven due to the fact that it reacted with Zinc and Sodium Hydroxide. When Tin (II) chloride reacted with Zinc, it began bubbling. This occurred because there was a single replacement reaction between Tin (II) Chloride and Zinc.
Purpose The purpose of the lab was to determine the mass percent of carbon in sodium bicarbonate, also known as baking soda, by the means of measuring the mass of carbon dioxide gas produced in the chemical reaction. Expected Results The expected, or theoretical result was 52.39 percent composition of carbon dioxide in the equation. To find this value, the molar mass of carbon dioxide was calculated, being 44.01g, which was utilized in the formula to find percent composition, %CE
Results The data obtained from the experiment had undergone statistical analysis using t-tests and the results were recorded in Figure 1.0 and Figure 1.1 above. According to the data obtained in Figure 1.0, the p-value is less than 0.05 in all 5 treatment solutions. It is also shown intensity Figure 1.0, the calculated t-value of each concentration of NaHCO3 in each treatment is greater than the critical t-value.
The actual yield of the reaction was 4.411 grams of copper and was obtained through the experiment
Investigation of the effect of NaCl concentration on the evaporation rate of water. Chemistry HL Internal Assessment Vitaebella Tsang Ao Ling Contents page Contents page 2 Introduction 3 Design 4 Research question 4 Variables 4 Method 5 Results 6 Discussion 9 Evaluation 9 Bibliography 10 Introduction Many recipes call for salt to be added to the water when cooking pasta to add flavor, but there has been common belief or misunderstanding that adding salt will make the water boil faster. However, it is now known that that is not the fact, and that adding salt will do the opposite and make the water boil more slowly instead.
However, the percent yield of this experiment was 109.96% (Fig. 5). Ultimately, the product mass collected after the reaction was a greater amount than the initial mass used in the original