3 Stoichiometry | |HM2 | | |9/9 Lab |Exp. 1 Densities of Liquids & Solids |ASA6 |ASA1 | | |9/11 Lec |Ch. 3 Stoichiometry |Homework 3 (HM3) | | |4 |9/16 Lec |Ch. 4 Stoichiometry
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Title: Experiment 5D – Investigating the Differences in Activity of Metals Purpose: To make observations of the types of reactions‚ write equations for those chemical reactions‚ practice balancing those reactions while determining the relative activity of the metals included in the lab. Materials: Apparatus Test-tube rack 4 test tubes (25 mm x 150 mm) 4 beakers (150 mL) Safety goggles Lab apron Plastic gloves Full face shield Reagents Zinc Magnesium Iron Copper 1M hydrochloric
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Lab #3: Stoichiometry of a Precipitation Reaction October 14‚ 2014 Abstract: The purpose of the lab‚ Stoichiometry of a Precipitation Reaction‚ is to be able to calculate the amount of a second reactant we need to react with the reactant one. You must calculate the amount of the second reactant using stoichiometry to figure out what amount is needed. After the amount is calculated‚ you then can add it to the first reactant and it will give you a full reaction. To figure out what you
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determine the reaction stoichiometry and the valency of magnesium Introduction Stoichiometry is the study of the quantitative relationship between amounts of reactants and products of a reaction. Stoichiometry can be used to calculate the amount of a product formed when given the reactants and a percentage yield. In the case of this experiment‚ a known starting mass of magnesium ribbon and the amount of collected hydrogen gas will be used in order to determine the reaction stoichiometry Magnesium is used
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60% SUMMARY OF LEARNING OUTCOMES 1. Describe composition of matter and chemical change. 2. Explain trends within the periodic table. 3. Describe Chemical Bonding in its various forms 4. Calculate chemical quantities and stoichiometry 5. Explain Oxidation - Reduction reactions 6. Demonstrate a knowledge of Organic Chemistry (Optional Element) LEARNING OUTCOME | ASSESSMENT CRITERIA | 1. Describe composition of matter and chemical change. | 1.1 Describe the nature
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for Cu(OH)2(s) equilibrium Test tube | Reagent to be added | 1 | 2.0 mL distilled water | 2 | 2.0 mL 1.0 M H2C2O4 solution | 3 | 2.0 mL water + pinch of Zn dust | 4 | 2.0 mL of 1.0 HNO3 | 5 | 2.0 mL of 6.0 M NH3 | 6 | 2.0 mL of 0.10 M Na3PO4 | 7 | 2.0 mL of 0.10 M Cu(NO3)2 | Each mixture was shaken thoroughly. The observations‚ specifically‚ the change in colour or amount of precipitate for each test tube are shown in Table 2. Table 2. Changes in the precipitate in each test tube
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this we can check the actual equation and the actual oxidation number of iron in this reaction. This process will finally end us up of finding out which oxidation number of iron is used in this experiment. So‚ if the oxidation number is 2: Fe (Ⅱ) + CuCl2 (aq) → Cu + FeCl2 If the oxidation number is 3 the reaction equation will be: 2Fe (Ш) + 3CuCl2 (aq) → 3Cu + 2FeCl2 In addition‚ we will need to find the percent yield of copper. Percent yield is a measure of the mass of what was produced ("experimental
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II. Materials A. Reagents 0.1 M potassium ferricyanide‚ K3Fe(CN)6 ferrous sulphate‚ FeSO4 sodium hydroxide‚ NaOH sodium chloride‚ NaCl hydrochloric acid‚ HCl potassium hydroxide‚ KOH potassium nitrate‚ KNO3 nitric acid‚ HNO3 trisodium phosphate‚ Na3PO4 sodium thiocyanate‚ NaSCN sulfuric acid‚ H2SO4 distilled water‚ dH2O B. Apparatus test tubes iron ring 250-mL beaker iron stand bunsen burner C. Others iron nails copper strip sand paper zinc strip pliers 2 III. Procedure A. Reactions
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CHEMICAL BONDS Chemical Bonds I. Introduction Chemical compounds are formed by the joining of two or more atoms. A stable compound occurs when the total energy of the combination has lower energy than the separated atoms. The bound state implies a net attractive force between the atoms called a chemical bond. The two extreme cases of chemical bonds are the covalent bonds and ionic bonds. Covalent bonds are bonds in which one or more pairs of electrons are shared by two atoms. Covalent bonds
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calculations just specific intervals Instantaneous Rate: The slope of the tangent to the curve of the concentration versus time graph; this is used for all chemical applications Rate Reaction and Stoichiometry The rates at which reactions are consumed and products are formed depend on stoichiometry of the reaction. Ex. 2HBr(g) H2(g) + Br2(g) *For every 2 mol of HBr that react‚ 1 mol of each product forms. The same 2:1 ratio applies to the rate of the reaction as well. For example
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