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
Lead compounds have been released into the atmosphere for many years, which rested into the soils. In this lab, the amount of lead in the contaminated soil will be determined using stoichiometry. The five objectives include: comparing the amount of lead in the contaminated soil with researched information; calculating the amount of lead (II) nitrate present in the contaminated soil; calculating the amount of lead present in the original contaminated sample; filtering out the solid precipitate; and
and the other may be limited. The reactant that is completely consumed is called limiting reactant, whereas unreacted reactants are called excess reactants. Amounts of substances produced are called yields. The amounts calculated according to stoichiometry are called theoretical yields whereas the actual amounts are called actual yields. The actual yields are often expressed in percentage, and they are often called percent yields. In this experiment we combined sulfuric acid and aqueous barium chloride
I choose to focus on the use and repetition of ratios and proportions as my major theme in chemistry. Throughout this sequence of instruction, my goal was for the students to seamlessly tie mathematics into the science curriculum. I wanted students to recognize the interconnectedness of the two subjects by emphasizing the association of ratios throughout chemistry and to realize the importance of ratios in real life. Ratios are found in all aspects of life and I wanted to open their eyes to this
congregate on the inside of the micelle and polar ionic ends at the outside surface of the globule. The nonpolar inside dissolves the grease molecules and the ionic outside is washed away. As the result, the myristic acid will form. Based on the stoichiometry of the reaction, one mole of trimyristin yields three moles of sodium myristates, therefore three moles of myristic acids are produced. In this experiment, 0.062 grams of trimyristin produced 0.05 grams of myristic acid. The percent yield is 84
element or compound will run out first and be limited. These instructions will help to determine how much product will be produced in the chemical reaction. Any high school or undergraduate chemistry student with basic knowledge of chemistry and stoichiometry will be able to complete these instructions. Materials • Pencil with an eraser • At least one sheet of ruled paper • Math calculator (ex. TI-30XA or TI-84) Warning Be sure to include all
Stoichiometry is a chemical branch that studies amounts of substances that are involved in reactions. Stoichiometry will help you to find out how much of the mixture you will need, or how much you started with. The calculations of a stoichiometry problem depends on a balanced chemical equations. The factors of the balanced equations signifies the molar ratio (the number of moles of each reactant needed to form a certain numbers of moles of each product) of the reactants and products taking part in
Through the completion of this experiment, the dynamics of stoichiometry are demonstrated by preforming a chemical reaction in a solution. This procedure will ultimately show how limiting reactants are factored into a reaction by using a varying amount of reactants involved. To better understand this concept, it is vital to define stoichiometry; stoichiometry is a way of documenting the amounts of products and reactants involved through a series of coefficients that describes the ration in which
Stoichiometry of Reactions Jessica Scanlan Experiment No. 7 CHMY 142-25 10/14/14 Trenton Hopkins I. Introduction The purpose of this experiment was to examine how the stoichiometry, “the quantitative relationships between substances involved in a chemical reaction”, can be applied to determine the quantity of sodium hypochlorite found in a bleach product. This experiment allowed it to determine how much oxidizing agent is in a cleaner by using a redox reaction, which is a
on both sides of this equation, it is already balanced. Balancing a chemical equation is also called stoichiometry. Stoichiometry allows us to calculate the proportions of reactants to products. This has to do with the law of multiple proportions. This law states that a specific mass of one element combines with a specific mass of another in a ratio of whole numbers. Another use of stoichiometry is to convert to moles. The mole, a constant discovered by Avogadro, allows us to compare any substance
Abstract In this experiment methyl-3-phenyl-2-propenoate was prepared using a Wittig reaction. Benzaldehyde and methyl (triphenylphosphoranylidene) acetate were used to give a final product. 0.33g of methyl3-phenyl-2-propenoate was found at the end of the experiment therefore the percentage yield of methy-3-phenyl-2-propenoate is 62%. The Rf value of benzaldehyde was found to be 0.85. The Rf value for methyl-3-phenyl-2-propenoate was found to be 0.83, the Rf values are almost the same therefore the
Ion exchange resin (Amberlyst 36) was purchased from Sigma–Aldrich (total pore volume 0.20 mL/g). According to the information offered by the supplier, the average pore diameter and surface area of the resin are about 240 Å and 33 m2/g, respectively. Pt/C (Sigma-Aldrich, 5wt% loading) was used for the consecutive hydrodeoxygenation reaction. 2.2. Fast pyrolysis of yellow poplar Yellow poplar (Liriodendron tulipifera) was ground, passed through a 0.5 mm sieve, and pyrolyzed. Fast pyrolysis was accomplished
Introduction: A balanced chemical equation has reactants and product that has to represent a formulae. The amount of each element, number needs to be the same on either side of the equation. (E.g., HCl(aq)+NaHCO3(s) reacts to produce NaCl(aq)+H2O(I)+CO2(g)). This helps us view the study of the Law of Conservation of Mass, and how it works in this equation. The calculation for formula, mass helps us to determine if you need to convert grams to a particular substance to moles, from a product. Moles
Chapter 1—Birth of Glass and Emergence of Diversified Glassware Believed to date back about as many as 5,000 years, the birth of glass had something to do with a copper-refining technique. Glass was reportedly generated when substances contained in fire clay, stone, and other materials in a copper refining kiln, started to melt and mix with each other at high temperature. It is considered that, in early days after the birth of glass, people mainly produced glass beads to use them as accessories,
performed an experiment and using the law of conservation of mass which says that mass is conserved during a chemical reaction, the law of definite proportions which says that a compound is always made of the same proportion of elements by mass, and stoichiometry to properly balance the equation. The first part of the experiment was to measure an amount of baking soda to start out with. For the first and second time we performed the experiment we used 1 g of
in the experiment of the Atomic Wight of the Element Silver. We react excess amount of copper with silver nitrate solution. To determine the amount of copper reacted and silver that is produced. The first thing that we did was rinsed 150 ml beaker with distilled water. Second, we dispense 10.00 ml of silver nitrate into rinsed beaker. Then we added 100 ml of distilled water to the beaker. Third we obtain a precut copper wire and then winded around large wide mouth test tube to produce a helix or
Sodium Hydrogen Carbonate and Acetic Acid Reaction Introduction Not knowing whether calculations on a paper or an experiment are conducted correctly is one of the problems faced in chemistry. Luckily to ensure both calculations are correct, getting a one hundred percent yield is a necessity. “The actual yield of a product as a percentage of theoretical yield,”1 is how to determine the percent yield of a reaction. Actual yield is the amount, in grams, that a reaction actually produces while theoretical
Procedure: A sand bath was set atop a hot plate set at power level 5, while a 10 mL round bottom was prepared with the addition of 14 (0.33 mL) drops of olive oil and 1 mL of cyclohexene. Once the contents of the 10 mL round bottom were mixed thoroughly, a boiling chip was added, and the round bottom was attached to a reflux condenser apparatus. The reflux was run for 20 minutes starting at the point in time when the mixture within the round bottom flask (that was submerged in the heated sand bath)
Experimental Overview: In this experiment, I was making a sample of aspirin and then testing it in order to see how pure the sample of aspirin was. By doing this experiment, I was leaning how to crystalize products, and then used the theoretical yield, along with the percentage yield in order to calculate the amount of aspirin that I had created in the sample. Aspirin is an anti-inflammatory, and analgesic, meaning this medication can reduce inflammation, fever, and pain by blocking the enzymes
The synthesis of .525 g of para-methoxyacetophenone and .49 g of para-chlorobenzaldehyde using 95% ethanol and catalytic aqueous sodium hydroxide yielded .587 g (61.7% yield) of chalcone 1. The product of chalcone 1 was then confirmed through several different tests. Testing with TLC showed that the product contained a pure substance with only one dot present. The melting point was tested and showed similar characteristics to that of the literature melting points2. The 1H-NMR was analyzed and the