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Balanced chemical equations contain a large amount of information that can be interpreted by people who have knowledge of the information. A chemical reaction contains reactants and products that are separated on the left and right sides by an arrow. When working with chemical equations, they should always be balanced with the number of reactant atoms equaling the number of products that are produced. This can be obtained by using coefficients on the reactants and product sides of the equation.
Stoichiometry shows the quantitative relationship between the reactants and products that are shown in a chemical equation. In the lab that was conducted, the stoichiometric relationship of the reaction of sodium chloride (NaCl) and silver nitrate (AgNO3) was being observed and investigated. It was hypothesized that one mole of sodium chloride (NaCl) would react with one mole of silver nitrate (AgNO3), allowing the production of one mole of sodium nitrate (NaNO3) along with one mole of solid silver chloride (AgCl), which will be a precipitate.
Before starting the limiting reagent lab, information about stoichiometry and balanced equations had to be known.
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Prior to starting the lab, the chemical equation that was being observed needed to be checked to make sure that its reactants and products were balanced. After having the chemical equation balanced, it was then time to begin the lab. To complete this lab, the following materials were needed:
After gathering the materials that are needed for the lab, it is time to start the experiment and to test one's ability to perform stoichiometric calculations and observe different types of chemical reactions.
First, the Erlenmeyer flask containing '1.00 g NaCl' would be observed, and data taken from the solution. The value of its concentration, such as the molarity, should be recorded for the sodium (Na) and chlorine (Cl). After taking the molarity of each element, the calculations should be performed to find the number of grams of each and should also be recorded. Next, the Erlenmeyer flask containing '1.00 g AgNO3' would then be used, and 100 mL of distilled water should be added to the flask. This should be done by taking a 250 mL beaker and measuring out 100 mL of water. After measuring out the water in the beaker, it should then be poured into the Erlenmeyer flask containing '1.00 g AgNO3.' When completing this, the Erlenmeyer flask should then be observed, and the molarity of each element should be recorded. Then, after taking its molarity, it should then be calculated to find the mass of the molarity that was found, and it should also be recorded. At this point in the lab, one should have the right agents to perform the reaction. For the reaction part of the lab, the entire amount of the NaCl solution should be poured into the flask that contains the AgNO3 solution. Once this step is completed, the flask containing the mix of reagents should then be observed, and the molarity of each element should be recorded. The mass of the product (AgCl) should also be recorded in grams. Finally, after this step, the lab is completed, and one is now able to look back at their data and analyze it.
When completing the lab, the following data was found. The tables below show all the information that was found and the results from the calculations that were made. While completing the lab, the molarity of each element was given when the solution was being looked at, but after having the molarity one would then have to find the grams. In the following data, the grams can be found by taking the molarity given and multiplying it by the volume of the liquid in liters, and this will provide the moles of that element. Once the moles of the element are found, one would then take that number and multiply it by the molar mass to calculate the number of grams in the element. By using the calculations, the following information was found throughout the lab.
| Erlenmeyer Flask Containing '1.00 g NaCl' | ||
|---|---|---|
| Species | Molarity | Grams |
| N | 0.107529 | 0.39337913 g |
| Cl | 0.107529 | 0.6065807 g |
| Erlenmeyer Flask Containing '1.00 g AgNO3' with 100 mL of distilled water added | ||
|---|---|---|
| Species | Molarity | Grams |
| N | 0.0586647 | 0.365053 g |
| Ag | 0.0586647 | 0.635031 g |
| Flask Containing Mixed Reactants | |
|---|---|
| Species | Molarity |
| N | 0.0293733 |
| Ag | 3.27027e-9 |
| N | 0.0853807 |
| Cl | 0.0560074 |
AgCl that was formed
| Species | Grams |
| AgCl | 0.843704 g |
It was hypothesized that one mole of sodium nitrate (NaNO3) along with one mole of solid silver chloride (AgCl) would be produced from the chemical reaction of one mole of sodium chloride (NaCl) and one mole of silver nitrate (AgNO3). The results that were found through this later supported the hypothesis that was made. By being given the moles of each reactant and then using the given information to calculate the number of grams, this is why it is believed that the hypothesis made beforehand is supported. The limiting reactant in this chemical reaction would be the NaCl, and the excess is AgNO3 because the ratio of the stoichiometry is one to one. The limiting reactant is in a chemical equation that allows the amount of the product that can be formed to be limited. From the findings of this lab, someone who may take interest or care would be a chemist or scientist because the meaning of what was found is the reaction that took place and the stoichiometry calculations that had to be performed to find certain data. Someone performing this lab should be excited about their findings because they could possibly help a chemist or scientist out with the information that was found even if it is not one hundred percent correct. The most exciting part about this lab should be what was learned throughout completing the lab and the information that one was able to complete while doing the lab.
After finding the data of the chemical reaction, it was then thought of if solution 1 contained 2.00 g of NaCl, how many grams of AgNO3 would have to be added for there to be a complete reaction. From the calculations performed, it would take 5.81 g of AgNO3 to completely react with 2.00 g of NaCl. By taking the molar mass of AgNO3 and dividing it by the molar mass of NaCl and multiplying it by 2 g, this is how it was concluded that this 5.81 g of AgNO3 should be added to cause a complete reaction with NaCl.
Next, it was thought that given solution 2 contains 3.00 g of NaCl, if excess NaCl would be added to the solution, how many grams would be formed of AgCl solid. After looking back at calculations and at the stoichiometry, it was concluded that 2.5312 g of AgCl solid would be formed. This was found by using the calculation of the given molarity of Ag was then multiplied by the volume of the flask and then multiplied by the molar mass per mole of AgCl. Using this calculation, it was found that 2.5312 g would be formed of AgCl solid.
In conclusion, this laboratory experiment aimed to explore the stoichiometric relationship between sodium chloride (NaCl) and silver nitrate (AgNO3) in a chemical reaction. The hypothesis that one mole of NaCl would react with one mole of AgNO3 to produce one mole of sodium nitrate (NaNO3) and one mole of solid silver chloride (AgCl) was supported by the experimental results.
Throughout the experiment, we carefully measured the molarity of each element involved and used stoichiometric calculations to determine the number of grams produced. Our findings confirmed that the limiting reactant in this chemical reaction was NaCl, and the excess reactant was AgNO3, consistent with the balanced stoichiometry of one-to-one.
These results hold significant importance for chemists and scientists as they provide valuable insights into the reaction mechanisms and stoichiometry calculations involved. While the data may not be entirely precise, it contributes to a better understanding of the chemical process at hand.
Furthermore, the experiment allowed us to make predictions for scenarios involving different quantities of reactants. For instance, if a solution containing 2.00 g of NaCl is used, it would require 5.81 g of AgNO3 to ensure a complete reaction. Similarly, if solution 2 contains 3.00 g of NaCl and excess NaCl is added, 2.5312 g of AgCl solid would be formed.
In summary, this laboratory exercise provided a hands-on opportunity to apply the principles of stoichiometry and observe the outcomes of a chemical reaction. It highlighted the importance of balanced equations and the careful consideration of reactant quantities in achieving desired products.
Stoichiometry of NaCl and AgNO3 Reaction: Experimental Analysis. (2024, Jan 17). Retrieved from https://studymoose.com/document/stoichiometry-of-nacl-and-agno3-reaction-experimental-analysis
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