Furthermore, stoichiometry helps to figure out the limiting reactants and the excess reactants. The limiting reactant is the reactant that limits the amount of product formed in the chemical reaction. Which also means the reaction will stop when all of the limiting reactant is consumed. In the other hand, excess reactant is a reactant that completely used up and it remains when a reaction stop when the limiting reactant. Moreover, stoichiometry can be used to figure out the actual yield which is the amount actually produced of a product vs. the amount of products calculated from the complete reaction of the limiting reactant which is theoretical yield. Also, stoichiometry assists to calculate the percent yield, which is the ratio of …show more content…
So, each lab group was assigned to different trial.
Table 1
Trial KI mL .400M Pb(NO3)2 mL Average PbI2 produced per volume of KI for the class (g)
1 0.500 mL 2.00 mL .020
2 1.00 mL 2.00 mL .076
3 2.00 mL 2.00 mL .151
4 3.00 mL 2.00 mL .230
5 4.00 mL 2.00 mL .294
6 5.00 mL 2.00 mL .358
7 6.00 mL 2.00 mL .375
8 7.00 mL 2.00 mL .388
9 8.00 mL 2.00mL .397
Using two graduated cylinder, dispensed 2.00 mL of KI solution into a clean, dry 100 mL beaker and dispensed 3.00 mL of KI into a different 100 mL beaker. Moreover, dispensed 2.00 mL of Pb(NO3)2 into a clean, dry, small beaker using the digital Micropipette.
While stirring one solution, slowly added the other to it. Rinse the empty beaker with 40 mL of RO water.
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.
Results
The
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.
After added, pick up the beaker and swirl it around lightly for a short period of time.
A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?
Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions.
• Serially dilute the 4 mg/ml solution with buffer A to make working solutions of 400 µg/ml and 40 µg/ml.
NH3. Add 20 mL water to the beaker by filling and emptying the 10 mL cylinder into the beaker
Fill a test tube about 1/3 full with cold tap water for use in step 34.
The wet, crude product was placed into the 50 mL Erlenmeyer flask. Small amounts of CaCl2 were added to dry the solution. The flask was sealed and the mixture was swirled and left to settle. Once
The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.
If the relative amount of reactants is altered, then the limiting reactant may change accordingly. 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.
In order to minimize errors and to "place" the solutions in the same environment, the same volume should be extracted from each solution using the syringes.
The purpose of this experiment is to familiarize oneself with the general procedures determining a partition coefficient at the microscale level and learn in weighing milligram quantities of materials on an electronic balance, the use of automatic pipets, the use of transfer pipet, and the use of a vortex mixer. Also, to familiarize oneself with extraction
XII. Take the 250 ml beaker to your lab bench. Set up a gravity filtration with a plastic funnel, folded wet filter paper, and an Erlenmeyer flask. Pour the content in the 250 ml beaker slowly through the filter paper. Wash the filter paper with deionized water. Dispose of the filtrate in the proper labeled waste container.
1) Pour 25 mL of the 1 M hydrochloric acid into the beaker and rinse the solid by swirling the acid around in the bottom of the beaker.
Stoichiometry has many uses in the real world. In the chemical industry and in professional scientific experiments, scientists use stoichiometry to save money. Scientists use stoichiometric calculations to determine the amount of a substance they need to purchase for a specific reaction. There are four possible reactions that can occur when sodium bicarbonate thermally decomposes. In this lab, stoichiometry was used to find out which balanced chemical equation out the four best represents the thermal decomposition of sodium bicarbonate.