Stoichiometry Lab Report

In Experiment B the limiting reactant was determined to be CaCl2 when two drops of the test reagent 0.5 M CaCl2 was added to the supernatant liquid in test tube 1, and a precipitate formed. Since there was a reaction, there was C2O42- in excess and Ca2+ is the limiting reactant in the original salt mixture present in test tube 1 . This was further confirmed when two drops of the test reagent .05M K2C2O4 was added to the supernatant liquid in test tube 2. There was no precipitate because Ca2+ was not present since it was the limiting reactant and instead C2O42- was in excess.

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.

In the experiment I performed it was proven that, the moles of a solute, the volume of the solvent, and the molarity of an aqueous solution share a mathematical relationship. Solutions, solutes and molarity are all terms that are crucial to chemistry. A solution is defined as a liquid mixture in which the solute is distributed into the major component, and a solute is defined as the minor component within a solution. The molarity of a solution is the number of moles of solute per liter of solution and it is used to express the concentration of a solution. Both the solute amount and the solution volume can be determined in experiments to aid finding the solution concentration or molarity of a substance that they are included in. I state confidently

The limiting reactant lab was constructed to provide a better understanding of precipitation reactions, by using filtration techniques. Also, it was created to help determine the limiting reactants in a solution, and to calculate theoretical and percent yield. Within the experiment two metal salts were prepared. Part A formed the precipitation of cobalt (II) carbonate, while Part B formed the precipitation of nickel (II) phosphate. The experiment concluded, the calculated theoretical yields of 0.120 g for CoCO3 and 0.184 g for Ni3(PO4)2.

Stoichiometry is a branch of chemistry which involves the study of the amount of substances which are involved in a reaction. More specifically, stoichiometry is the use of the product reactant relationship in a chemical equation to acquire a desired quantitative outcome. This process can be used to measure a variety of components in a chemical reaction such as molar ratios, molecular weights, the number of products produced in a reaction, and the quantity of the reactants which will be used in a chemical reaction. In this experiment, stoichiometry was used in order to determine the amount of aluminum needed to produce between 0.1 and 0.2 grams of copper when given copper (II) chloride in excess. However, in order to determine the amount of aluminum needed to produce between 0.1 and 0.2 grams of copper, first one must analyze the reaction which occurs between the aluminum and copper (II) chloride.

Objective: The objective of this lab is to determine the identity of an unknown alkali metal in a carbonate by the use of it in a precipitation reaction, and then the use of gravimetric analysis of the reaction. Introduction: In order to determine what the unknown alkali metal carbonate was, the unknown was reacted with calcium chloride of a known concentration. A double-replacement precipitation reaction occurred, therefore, a calcium carbonate precipitate formed, and it then was completely separated from the aqueous solution it was in so its mass could be measured. In order to separate the products entirely, first a filter paper in a funnel separated the precipitate from the aqueous solution.

The purpose of this experiment was to determine how much KMnO4 was needed to titrate approximately 1 mL of an Unknow X101 concentrated solution of Oxalic Acid. A standardized KMnO4 solution was used on a known solution of Oxalic acid to help determine the unknown percent oxalic acid in unknown X101. The unknown sample for this experiment was sample x101 which theoretically was a % Oxalic Acid dehydrate sample but, the average of all three trials determined it to be a 6.7% percent Oxalic acid.

After labeling each of the tubes, 250 mL of CaCl2 was added to all the tubes and

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

It is not reasonable to perform a percent yield calculation separately for the two products because the filtrate reserved from the formation of maleic acid was used to produce fumaric acid in the second part of the experiment, and we could not determine how much maleic acid dissolved without additional data. However, because the isomers have the same molecular mass, we could perform a

The final yield of this experiment was determined to be 0.02 or 2%. This measurement may have occurred because of experimenters fault. Mistakes while measuring stating material weight may have led to a human error which resulted in such inaccurate results. Also,

The Objectives for Part C of the experiment include (1) To calculate the dilution necessary for various molarities of a specific solution (2) To use these calculations to prepare such solutions (3) To use such solutions to understand the relationship between the concentration of a dilution

a) The main topics studied during the unit Quantities in Chemical Reactions were separated into two sections: Quantities in Chemical Formulas and Stoichiometry in Chemical Reactions. The first section involved qualitative and quantitative analysis, using the mole as a unit of calculation, calculating mass, molar mass and number of entities, calculating percentage composition and dealing with empirical and molecular formulas. The second section of the unit involved, mole ratios and mass relationships in chemical equations, determining limiting reagents and calculating percentage yield.

The resulting Ca(OH)2 solid was filtered from the NaCl liquid. The NaCl was then tested, in equal proportions, with NaOH and CaCl2 to determine the excess reagent and the limiting reagent. As different amounts of CaCl2 were added, the expected results did not match the actual results. This could be due to a number of errors in conducting the experiment such as inaccurate measurements. One point where the data does slightly reflect the expected outcomes is in the mass of precipitate recorded. These values do appear to plateau though the recorded values are much higher than the calculated ones. The actual yield did not reflect the theoretical yield accurately. Though both did increase, there is a significant difference between the values. From this experiment, concepts about reactions were learned including limiting and excess reagents as well as the disparities between actual data and experimental

The purpose of this experiment was to use stoichiometry to calculate the volume and percent yield of CO₂ produced from a reaction of acetic acid (vinegar) with baking soda.