Stoichiometry Lab Report

Limiting reagents can be easily determined on paper with stoichiometry, however, observing how it actually works is essential. This lab is focused on putting stoichiometry to use by determining and observing  the limiting reagent in the given, balanced reaction. In the field of chemistry, many want to produce a product by reacting to reactants that will create a certain amount of a product. In order to complete this, a chemist requires a balanced equation that states the exact amounts of reactants required to produce an exact amount of a product.

Introduction/Purpose: This report discusses an experiment done with copper metal. Several reactions were ran with it, which produced different copper compounds to in the end finally recover the original amount of copper. This experiment is important because it proved the Law of Conservation of Mass.

Example Problem Stoichiometry 4NH3(g) + 6NO(g)→5N2(g) + 6H2O(g) How many moles of each reactant were there if 13.7 moles of N2(g) is produced? ×4 moles NH3(g) = 10.96 moles NH3(g)

So if 0.38 is divided by 0.49 and multiplied by 100 then the percent yield for Zinc Sulfide would be 77.6%. When it comes to Sodium Chloride, the theoretical yield is 0.58 grams and the actual yield is 0.45 grams. So when 0.45 grams is divided by 0.58 grams and multiplied by 100, the percent yield would be 77.5% of Sodium chloride. The actual yield is directly taken from the mass of the products in the experiment while the theoretical yield is determined by using stoichiometric calculations. To determine the theoretical yield, the reactants should be converted from grams to moles based on the coefficients in the chemical equation and the moles should be incorporated into the mass of the reactants.

Background: The study of stoichiometry is a branch off Chemistry its the study of the amounts of substances that are involved in reactions. For this experiment kinetics is a huge part of it. Kinetics is explained as the reaction speed and or rate of reaction. To observe these reactions made by having reactants, sodium hydrogen carbonate, NaHCO3 known as baking soda and acetic acid, CH3COOH that is vinegar being mixed together.

ADI Lab: Stoichiometry and Chemical Reactions The guiding question of this ADI lab was, “Which balanced equation best represents the thermal decomposition of sodium bicarbonate?” The goal of this lab was to use our knowledge of stoichiometry with the mole ratio to identify the correct chemical equation for the decomposition of sodium bicarbonate. Information that was given going into this investigation was the definition of the law of conservation of mass and the atomic theory which states that no atoms can be created nor destroyed during a chemical reaction. Also the mole ratio which is used to determine how much of a product will be produced in a chemical reaction using the given chemical equation.

Scientists found that the stoichiometry of compounds changed periodically. If one ordered the elements by their atomic mass, you could group them by their chemical properties row after row. This grouping of elements by the compounds that they make became the periodic table. An example of a periodic chemical property is the reaction of metals with halogens (group VII elements) to make metal halides.

Analysis Questions: 1. In step #1, when water was mixed with CuSO4, the water turned a blue colour. Can you definitely confirm it is a physical or chemical property? Support your answer. I am unable to confirm that the action stated in this question is a physical or a chemical property.

What type of chemical reaction will a balloon receive when filled with an acid and base? Acids and bases are around us everywhere in various types of liquids. They are in the foods we eat and the things we use on a daily basis, for example liquid dishwashing soap. Acids are usually sour and bases are silky, giving it a bitter taste. Water can act like both, depending on the situation.

The purpose of this lab will be to identify the percent yield of copper in the unbalanced equation _Al(s) + _CuCl2(aq) → _Cu(s) + _AlCl3(aq). This will be determined by cutting a piece of aluminium 9cm by 9cm, recording its mass in grams, preparing a copper (II) chloride solution using the weight tray and electronic scale to measure 5.0g of CuC12 and adding it to 100 mL of distilled water. Then, a stirring rod will be used to dissolve the piece of aluminium into the CuCl2 solution until it is no longer visible. Additionally, the mixture will be filtered using a filter paper (which was previously weighted) on a funnel and weighted after it is fully filtered. Furthermore, the chemical equation will be balanced, stoichiometry will be used to find

After completing the lab, the actual data collected was not the same as the theoretical values. The theoretical yield was 2.75g of PbSO4, but the actual yield was 2.90g of PbSO4. A possible component that caused the error was the inaccurate weighing of the reactants. It is nearly impossible for someone to collect the exactly 3.00g of the given reactants. If exactly 3.00g of the reactants are not measured out, then it will cause an error in the experiment.

In this experiment the relationship of calcium chloride and sodium iodate in a reaction that produces calcium iodate. The calcium chloride and the sodium iodate undergo a precipitation reaction to produce calcium iodate. The goal is desirable for gaining understanding of limiting reagents in reactions and moles in equations. The purpose of the experiment was to determine how different amounts of calcium chloride and sodium iodate affect how much calcium iodate is produced. The chemical equation used in this reaction is: CaCl2 (aq) + 2NaIO3 (aq) → Ca(IO3)2 (s) + 2NaCl (aq) and this equation, (Concentration of

After the reaction is finished, the percentage composition of each element in the product can be found and used to calculate the empirical formula, which is the lowest whole number ratio

Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, research of definitions of each relating led to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound forms when two or more nonmetal atoms share valence electrons; covalent compounds are also

This first quarter of Second semester in a new class has been very good because I have kept my notebook very organized and up to date. For example from the left side of my notebook on page 92, I annotated and highlighted important information for this activity. This work shows high quality because of the use of different color and the annotations about specific ideas that we would be learning from this packet. Using color and making annotations has made it easier for me to use conversions with stoichiometry. The Relative Mass and the Mole work taught me about how to find the ratios of two atoms, the molar mass of elements, and Avogadro’s number.