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
Then the mass of the copper metal and the percentage of Cu were obtained and compared throughout different groups and a mean and standard deviation was calculated for the
The chemical elements are divided into two broad groups, the metals and the non-metals. In this experiment, you will examine some members of the metal group and identify similarities and differences in their physical and chemical properties. Metals are the elements that are found in the left of the periodic table with high electrical and thermal conductivity. Metals lose electrons to create positive ion charges. Metals have a unique shine, are prone to forming, have a high tendency to form cations, and combine with oxygen to give mostly basic oxides.
To better understand this law, Cu(s) was transformed with different reactions only to return back to Cu s). The initial and final mass of Cu(s) was recorded to give the percent recovery of copper product at
Abstract In this experiment the separation of a copper (II) chloride and sodium chloride mixiture was attempted. The main aim was to separate the compounds from eachother while receiving as much of the original mass of both substances as possible - in perfect conditions the original mass will be received after seperation. Many techniques were considered but dissolution, filtration and evaporation proved to be easiest and most reliable in a school environment with school equipment. The copper (II) chloride and sodium chloride mixture was dissolved in a methanol solution and filtered out leaving the sodium chloride behind.
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)
Different Mole Ratios And It’s Reactions Introduction: Chemical reactions play an important role when it comes to mole ratios.
The actual yield of the reaction was 4.411 grams of copper and was obtained through the experiment
Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.
Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g). The decomposition reaction was performed in a crucible and heated with a Bunsen burner.
INTRODUCTION A gas chromatograph (GC) can be utilized to analyze the contents of a sample quantitatively or in certain circumstances also qualitatively. In the case of preparative chromatography, a pure compound can be extracted from a mixture. The principle of gas chromatography can be explained as following: A micro syringe is used to inject a known volume of vaporous or liquid analyte into the head or entrance of a column whereby a stream of an inert gas acts a carrier (mobile phase). The column acts as a separator of individual or chemically similar components.
The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.
(0.01 moles of NaOH) x (1 mole Ca(OH)2/ 2 moles of NaOH) = 0.005 moles of Ca(OH)2 Tube 1: (0.0020 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.002 moles of Ca(OH)2 (0.002 moles of Ca(OH)2) x (74.08 grams/mole) = 0.1 grams = theoretical yield Tube 2: (0.0035 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.004 moles of Ca(OH)2 (0.004 moles of Ca(OH)2) x (74.08 grams/mole) = 0.3 grams= theoretical yield Tube 3 (0.0050 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.005 moles of Ca(OH)2 (0.005 moles of Ca(OH)2) x (74.08 grams/mole) = 0.4 grams =theoretical yield Tube
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
Copper is mainly used due to its better resistance in corrosion than other metals and its unwillingly nonreaction with most strong acids. To investigate and identify the nature of the reactions of copper, one can synthesize copper into a series of chemical reactions and explore its physical and chemical properties. The pure substance undergoing the chemical reaction, in this instant copper, takes on different chemical reactions. There are four types of chemical reactions: combination or synthesis reactions, decomposition reactions, substitution or single replacement
Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.