Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.
Some compounds have very distinctive colors when burned, such as Potassium, which is a white/purple, and sodium, which is a deep red hue. The first step for a flame test is to gather the needed materials. These include beakers, distilled water, the unknown substance, a Bunsen burner, matches, a nichrome wire, tubing to connect the gas line to the Bunsen burner, goggles, and known compounds to compare with. The first step is to make aqueous solutions of all the substances to be tested. This is done by adding .5
When the copper is heated, the flame of the bunsen burner changed from blue to green. The colour of the copper metal changed from a shiny reddish-brown colour to a dull gray-brown colour. When the magnesium is heated, it changed from a dull gray metal to a pale white colour. b) 2Mg (s)+ O2 (g) ----> 2MgO (s) Magnesium + Oxygen ----> Magnesium Oxide 2Cu (s) + O2 (g)----> 2CuO (s) Copper + Oxygen ----> Copper Oxide c)Copper
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
Introduction: Problem: What are some of the properties of ionic compounds? Summary: Ionic compounds are everywhere. They can be found just about anywhere on Earth.
Title: The burning speed of coloured and white candles. Type of project: Pure Science What I will do is take 2 candles and burn them and see how long it takes for each candle to burn. Candles, Advent, ChristmasA yahrtzeit candle, lit on the Proposal Question: Does the composition of materials in candles effect the rate of burning and do colourants have an effect?
Purpose: To recognize the evidence of a chemical change and to prove the law of conservation of mass by observing a series of chemical reactions involving copper. A specific quantity of copper will be transformed through a series of chemical reactions to form new substances and then recovered as solid copper. A percent yield will be calculated to determine the amount of copper recovered from the chemical reactions.
Summary for the H3O+ in the Birnessite (H-Bir) The presence of H3O+ in birenssite had been reported by Johnson1. In this paper, the author discussed that the hydrogen birnessite contained structural water and either hydroxyl hydronium (H3O+), or both. Interlayered H2O molecules inside the birnessite play an important role to the structure.
When the penny was placed in the flame of the bunsen burner, the copper melted and revealed the zinc, so it changed from a copper-color to silver. The color change is an example of a physical property, while the whole reaction is a chemical change. Investigation D: The magnesium reacts with oxygen in the air, and the bunsen burner is a source of heat for the reaction. When this reaction occurs, Magnesium Oxide is formed, making it a chemical change. Investigation E: Copper(II) sulfate is soluble in water.
The magnesium burned did not leave significant odor like matches or candles do because it reacts with the oxygen, which is present within the air. This means that it's not necessarily reacting with the fire as the candles or matches do. Thus, magnesium and oxygen reacting together makes the compound, magnesium oxide as a result. The only reason why is looks likes it's burning is due to the fire is because the reaction between magnesium and oxygen, as they create the heat. This results the bright lighting like that of fire.
THE RESULT OF ADDING DIFFERENT SUBSTANCES TO ROCKET FUEL. Name: Gareth Murdoch/Devan Garland Teacher: Mr Adams Class: Grade 9A Introduction The reason we chose this project was to find out what an inexpensive way to make rocket fuel for Mini projects and to experiment to find what substance you can add to make the fuel more effective in speed and burning rate. Investigative Question How do different substances affect the burning of rocket fuel?
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
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, definitions of each relating factor were researched, leading 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 is formed when two or more nonmetal atoms share valence electrons; covalent compounds are also categorized into two sections: polar covalent and nonpolar covalent. Furthermore, polar covalent compounds dissolve in water, while nonpolar covalent compounds do not.
Introduction: This lab report discusses an experiment to study the difference in the burn rate of various colored candles. The objective of this experiment is to analyse the outcome of burning 5 different colored candles including white under the same control variable for 60 minutes. The white candles used in this experiment are pure and no chemicals or dyes are added to it. They are normally made from paraffin wax with a wick in the middle.
Explain the sequence of thermal stages involved in combustion from preheating and to flaming and glowing. Identify which of these steps are endothermic and which are exothermic. Burning begins with endothermic reactions that absorb energy and ends with exothermic reactions that release energy. The endothermic reactions are known as preignition, the exothermic reactions as combustion, and the point of transition as ignition.
