AIM/PURPOSE
The purpose of this experiment was to prepare two solutions and use them to perform a precipitate reaction. Then using the results and mass gathered from the experiment, to determine the limiting reagents and to calculate percent yield.
BACKGROUND INFORMATION
The limiting reagent was calculated in this experiment. The limiting reagent is the reactant that limits the reaction and the amount of product that can be formed. The reactions stops only when all of the limiting reagent is consumed. However, it prevents the reaction from reaching its full potential. The excess reagent is the reactant that remains and is left over when a reaction stops and the limiting reagent is completely used up. The excess reagent is whatever is left over since there is nothing left for the excess reagent to react with. (Department of Chemistry Texas A&M University, n.d.)
To calculate the limiting reagent, first and foremost the balanced chemical equation for the reaction needs to be obtained. Next, the molar mass of
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These coefficients can also determine the relative number of molecules, formula units, along with the moles involved in a chemical reaction. (Oklahoma City Community College, n.d.). Based on the experimental data, the mole ratio of limiting reagent to precipitate is 1 where the moles of the limiting reagent is 4.717426×10-3 moles and by multiplying by the ratio obtained from the balanced equation, the moles of the precipitate also 4.717426×10-3 moles. When we compare this to the ratio found within the balanced equation it is observed that the ratio is 1mol/1mol=1 or 1:1. Similarly through the experimental data, the ratio is 4.717426×10-3mol/4.717426×10-3mol = 1 again this is also 1:1. This indicates that for every one mole of the limiting reagent there is one mole of the precipitate, for every two moles of the limiting reagent there is two moles of the precipitate, and so
The purpose for this experiment was to determine why it was not possible to obtain a high percent yield when Calcium Nitrate Ca(〖NO_3)〗_2 with a concentration of 0.101 M was mixed with Potassium Iodate KIO_3 with concentration of 0.100 M at varying volumes yielding Calcium Iodate precipitate and Potassium Nitrate. Filtration was used to filter the precipitates of the solutions. The percent yield for solution 1 was 87.7%, and the percent yield for solution 2 was 70.8%. It was not possible to obtain a high percent yield because Calcium Iodate is not completely soluble and some of the precipitates might have been rinsed back to the filtrates when ethanol was used to remove water molecules in the precipitate.
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
For example, a balanced chemical equation of a certain reaction specifies that an equal number of moles of two substances A and B is required. If there are more moles of B than of A, then A is the limiting reactant because it is completely consumed when the reaction stops and there is an excess of B left over. Increasing the amount of A until there are more moles of A than of B, however, will cause B to become the limiting reactant because the complete consumption of B, not A, forces the reaction to cease. Purpose
We finally took 1ml of the 0.01% solution from test tube using the glucose pipette and adding it to test tube 4, we then used the H2O pipette and added 9ml of H2O to test tube 4 creating 10ml of 0.001% solution.
Thorough analysis of the graph displayed enough evidence suggesting that an increase in substrate concentration will increase the height of bubbles until it reaches the optimum amount of substrate concentration, resulting in a plateau in the graphs (figure 2). Hence; supported the hypothesis.
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
Theoretical yield is the maximum amount of product that can be produced during a reaction (French et al. 83). The numbers used to find theoretical yield must be those of the limiting reagent (French et al. 83). Because parts of the material used are inevitably lost during experiments, the actual yield will be smaller than the theoretical yield (French et al. 83). To test the efficiency of the reaction, calculate the percent yield as shown below:
100% of the reaction, the moles of acid are stoichiometrically equal to the moles of base. The
Once the mixture had been completely dissolved, the solution was transferred to a separatory funnel. The solution was then extracted twice using 5.0 mL of 1 M
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
Many factors influence rates of chemical reactions. Some of these factors include: the nature of reactants, for example the formation of salts, acid-base reactions, and exchange of ions are fast reactions, while in reactions where bigger molecules are formed or break apart are typically slow; temperature, frequently, the higher the temperature, the faster the reaction; concentration effect, the reliance of reaction rates on concentrations are called rate laws. Rate laws are expressions of rates in terms of the concentra...
The last way is to note how long it takes for a precipitate to form
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.
borate) and 1.0 g. of sodium hydroxide in 20 mL of warm water. It may
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).