Research Lab Report Stoichiometry

Stoichiometry: A branch of chemistry that deals with the relative quantities of reactants and products in chemical reactions.

Stoichiometry is a very important part of chemistry. Stoichiometry refers to calculating the masses of molecules and their products . The reactants are usually given and stoichiometry is used to find the products of the equations as well balancing the equation. An example of this would be sodium chloride (NaCl). Stoichiometry will say that if there are ten thousand atoms of sodium and one atom of chlorine, only one molecule of sodium chloride can be made and that fact can never be changed.

Question of the day: What is the stoichiometric ratio of reactions in the chemical synthesis of the (2, 4-pentanedianato) iron (III) complex ion?

3. If Iron (II) Sulfate were formed, what mass of Copper would be expected and what is the limiting reagent?

The law of conservation of mass is when the total mass of the products must equal to the total mass of the reactants. Plus, it illustrates the product when magnesium is oxidized with oxygen gas with energy as a form of a heat source. The findings from the experiment are that there was 0.04550g of magnesium, 0.01740g of oxygen and 0.06290g of magnesium oxide. These are the weights of the reactants and products in this chemical reaction which is used to find percent composition and percent error. The amount of magnesium used in the chemical experiment was determined by subtracting the mass of the crucible and lid from the mass of the crucible, lid and magnesium strip. A similar math was used to determine the mass of oxygen by subtracting the mass of the crucible, lid and magnesium strip from the mass of the crucible, lid and magnesium oxide. Then to find the weight of magnesium oxide, the mass of the crucible and lid was subtracted from the mass of the crucible, lid and magnesium

Subsequently, two porcelain crucibles were used, weighed, and heated for about 10 minutes and then placed into a desiccator to cool. The two empty porcelain crucibles were first heated because the heat would vaporize any impurities that were originally on the crucible. The first crucible weighed 11.9047 g and the second crucible weighed 12.3735 g. Once the mass of the two crucibles

Procedure: This lab starts off by making sure the logger pro and temperature probe are in proper condition. Then, the data collection must be adjusted to 15 minutes and 12 samples/ min. After that a Bunsen burner must be set up by assembling a ring-stand, ring, and wire gauze, and a crack-less beaker is used to boil some water. First the beaker and the large watch glass need to be weighed and the mass has to be recorded using a triple beam balance. Next, the beaker with 200g of ice is placed on the ring stand, and immediately heated over medium flame. An important note is to make sure the flame is perfectly adjusted so the ice does not melt on the counter while trying to adjust the flame. Furthermore, place the temperature probe in the ice so it is not resting at the bottom of the beaker, it is best to secure it with a small clamp. Additionally, click the green start button on the computer and stir continuously with a glass rod until the ice is completely melted. Once the ice has melted which is somewhere between 3-5 minutes, the stirring rate will slow

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

The samples were synthesized from a synthesis solution by dissolving 7.98 g sodium hydroxide pellets (A.R) and 11.01, 8.01, 6.79, 2.73, 1.64, 0.9 g of aluminum sulphate, aluminum chloride, aluminum isopropoxide, sodium aluminate, alumina and aluminum metal (Aldrich), respectively in 69.5 g deionized water in a beaker. The mixtures in the beaker were thoroughly mixed and a 50 g Ludox AS30 colloidal silica (Aldrich) was slowly added to the above solution under stirring at high speed. The molar composition of the resulting synthesis gel was 12Na2O: 100SiO2:2Al2O3: 500H2O. Prior to being transferred to a Teflon-lined stainless steel autoclave, the above synthesis solution was aged for 20 hr at room temperature and then hydrothermally treated

In regards to the upcoming exam I am truly unsure. I feel as though I am prepared and have practiced by completing all of the assignments on ALEKS, doing the reading and attending lecture, doing the practice problems in the books and going CleRC for help and clarification as needed. However, I still need to do more preparation in regards to completing the practice exam and getting help if needed. I feel decently prepared for the exam, but I am truly unsure about the testing style and what it will actually be like.

Stoichiometry is the numerical relationship between products and reactants;from its calculations, one can predict the products when only the reactants are known or vice versa. Most calculations in chemistry use this in some way (Graves, 2013). Along with stoichiometry, dimensional analysis can also be used, and through the use of both one can calculate the moles of a substance, limiting reagents of a reaction- the substances that limit a reaction’s potential yield, substances that are in excess, number of atoms of a substance, analysis of a combustion reaction,and the molarity of a solution (Burdge and Overby, 2012).

The mass of a piece of filter paper was measured. The paper was folded and placed in a ceramic Buchner funnel. Then, Wet the paper with RO water. The liquid was poured from the beaker into the Calculations funnel using a rubber policeman. The precipitate was carefully transferred to the funnel. Rinse the beaker and a rubber policeman with RO water. Additional water was added to rinse the precipitate. The filter paper was transferred to a beaker using the watch glass and placed the beaker on the Bunsen burner to dry the filter after all the water has passed through the funnel. The mass of the filter paper and precipitate was measured after the precipitate was completely dried.

Use a weigh boat and scoopula to measure out 0.75 g of agarose onto a digital scale. Make sure to tare the digital scale before weighing the powder. Pour the powder into a 125 mL Erlenmeyer flask.

Chemical equilibrium is the study of change within a chemical reaction and how far it will go to reach a dynamic equilibrium (Burdge). Dynamic equilibrium is defined as the constant movement of species in a chemical reaction, gone to incompletion while the rates of production and consumption are equal (Kf = Kr ) (Burdge). It differs from static equilibrium in that species are constantly being consumed and produced, it is dynamic movement (Fox). The concentration of such species do not change, it remains constant (Fox). The rate at which species are being consumed and produced is known as the equilibrium constant (K) (Burdge). Due to the fact that the concentration

A bomb calorimeter with the Parr design was used for the apparatus, which would lead to an experiment to measure temperature in degrees Celsius as time increased. Two different sample pellets were used, one being benzoic acid while the other was naphthalene. These measured findings were then used to determine the change in temperature for each experiment, which for benzoic acid…