Jack Zhou
Eric Lonrenzo
Chemistry section #
Date
Chemical Reactions
Introduction: The purpose of the lab was to create and observe the 4 kinds of chemical equation, and to identify reactants and products of those reactions. The four kinds of chemical reactions are synthesis, decomposition, single-displacement and double-displacement.
Materials: Bunsen burner, sparker, tongs, 5 test tubes, scoop, wooden splint, lead(II)nitrate, magnesium wire, copper(II) carbonate, hydrochloric acid, zinc, potassium iodide, test tube tack, googles, apron, gloves and a metal test tube holder.
Methods:
Experiment 1: Synthesis 1, Obtain a piece of magnesium wire. 2, Light the Bunsen burner
3, using the tongs, hold the wire in the flame of the burner. Do not
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Experiment 2: Decomposition 1, place two scoops of cooper (II) carbonate in a test tube.
2, Heat the test tube with the sample for three minute. Do not point the test tube toward anyone.
3, remove the tube from the burner and light the wooden splint. Insert it into the test tube and observe the reaction
Experiment 3: Single-displacement 1, Put about 5mLs of hydrochloric acid into a test tube and place it in a test tube rack. 2, add a piece of Zinc and invert another test tube over this one and observe 3, Look for gas being released, and tries to collect this gas.
4, keep the tube with the gas inverted. Insert a glowing splint into the test tube and observe the reaction.
Experiment 4: Double-displacement 1, obtain two test tubes. Place 2mLs of potassium iodide into one of them. 2, in the second, place 3 mLs of Lead (II) nitrate. 3, slowly pour the lead (II) nitrate into the potassium
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After the reaction, the remaining aluminum was blacked and bubbled. Heat was also produced by the reaction, its chemical equation is 2Al + 3CuCl2 ----> 3Cu + 2AlCl3.
The fours experiment was complex and is Pb(NO3)2(aq) + 2KI(aq) ----> PbI2(s) + 2KNO3(aq), it is a reaction became the color of the solution turned yellow.
Discussions. The first experiment was clearly a synthesis, as the Magnesium and the flame reacted and combined, forming 2MgO. The reason of the 2 Mg is because all chemical equation must be balanced, and the total electron number must be zero. A O have a -2 charge, while Mg have a +1 charge. The sign that this was a chemical reaction is the formation of a new solid, and the flashes and heat produced during the reaction.
The second lab was a decomposition, as when the Copper (II) dioxide was heated, it broke down into carbon dioxide and Cupper (II) oxide. It fit into the AB-->A+B formula for decomposition. The indicator that a reaction had occurred is the smell and the change of color.
The third experiment was a single displacement reaction, as it fit into the AB+C-->AC+B formula.The Al was added with CL, while the CuCl just became Cl. Of courses that wasn’t the equation as it still needs to be balanced of the
The experiment is to observe a variety of chemical reactions and to identify patterns in
Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.
This experiment was designed to illustrate the relationship between quantities of reactants and the amount of product produced by a chemical reaction. When a chemical reaction occurs, there is usually a limiting reagent, which is the chemical that is totally consumed at the end of the chemical reaction, and the reagent that limits the amount of product that can be formed. The purpose of this lab was to determine which reactant was the limiting reagent and to see how much of the other reactant was used. The reaction tested in this experiment was between Copper (II) Chloride and Aluminum metal.
When the tip of the rod touched the pH paper, the color of the pH paper became blue.
(15 points) There was one combination that did not have any reaction when tested. This combination was the MgSO4 and CH3COOH. The reason that the reaction did not happen is because they created a mixture and not a chemical change. 3.
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?
In this experiment you will observe some physical and some chemical changes. You will observe that energy must be used to start some chemical reactions, and that it is produced in others.
The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical.
There was an assortment of different changes indicating that chemical changes were taking place such as change in color or chemicals bubbling when combined with another chemical.
Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, 1M NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9, ammonia which was identified by its pungent odor, was added, an inky dark blue color was made. Iron (Fe (NO3)3) was determined to be in test tube K-2. KSCN was found in test tube K-11 since Fe (NO3)3 and KSCN makes a bloody color when mixed together. Flame tests were conducted in which K-8
Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.
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.
Safety glasses: Wear safety glasses to protect eyes from substances, acids and flames that can irritate or damage the eyes.
Materials We did several different examples of chemical equilibriums using different stresses and conditions. This includes adding or removing reactants, changing temperature, or adding additional compounds. Our materials included a large variety of chemicals and equipment used to conduct our labs.
This paper is about chemical reactions and chemical reaction types. All the data gathered was from conducting multiple experiments. Each experiment was performed carefully and analyzed to obtain the necessary information for the paper. That information included the four signs of a chemical change, the rnx type, and more.