Heat of Formation of Magnesium Oxide Objetive: To determine the heat formation of MgO (Magnesium Oxide) using Hess’s Law‚ which states the heat within a chemical reaction is independent of the pathway between the initial and final states. Introduction: Chemical reactions require heat energy to complete‚ called an endothermic reaction‚ or produce heat energy‚ and thus called an exothermic reaction. The heat energy produced by such reactions can be measured using a calorimeter‚ a piece
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THE Ksp of Magnesium Oxalate ABSTRACT INTRODUCTION In this experiment the solubility product constant of the salt magnesium oxalate (MgC2O4)will be determined. The system of interest exists as a solid in equilibrium: Precipitation reaction of EXPERIMENTAL METHODS Preparation of the 0.15M Potassium Permanganate (KMnO4) solution {text:list-item} B. Prepare precipitation mixtures 1. Obtain three labeled 20-mL vials from the cart. 2. Burets are set up in the lab with 0.250 M
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Sheep” we measured the temperature of the 10 milliliters of Solution 2. Then we dropped a ball of steel wool into the test tube and measured the temperature again. We stored the test tubes on the test tube rack to observe the next day. A chemical reaction did occur in the lab. There were a color change and an odor change that was observed on Day 2 of the lab. On Day 1‚ the liquid was clear and the smell was very strong. On Day 2 of the lab‚ most of the liquid was gone but the color was a muddy
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Chemical Formulas and Chemical Compounds MIXED REVIEW SHORT ANSWER Answer the following questions in the space provided. 1. Write formulas for the following compounds: CuCO3 a. copper(II) carbonate Na2SO3 b. sodium sulfite (NH4)3PO4 c. ammonium phosphate SnS2 d. tin(IV) sulfide HNO2 e. nitrous acid 2. Write the Stock names for the following compounds: magnesium perchlorate a. Mg(ClO4)2 iron(II) nitrate b. Fe(NO3)2 iron(III) nitrite c. Fe(NO2)3 cobalt(II) oxide d. CoO nitrogen(V) oxide
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Thermodynamics/Calorimetry Introduction: Thermochemistry investigates the relationship between chemical reactions and energy changes involving heat. The amount of heat generated or absorbed in a chemical reaction can be studied using a calorimeter. Purpose: The purpose of this laboratory was to determine the heat capacity of the calorimeter‚ and to understand thermodynamics/calorimetry by applying the calorimetry equation‚ Heat lost=Heat gained. We will use calorimetry to determine
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TOPIC 2 Metals The History of Metals * Uses of metals through history: * Copper Age (3200-2300 BCE) – copper and tin were most common metals‚ and were used for ornaments‚ weapons and tools. * Bronze Age (2300-700 BCE) – copper‚ tin and bronze were used for tools‚ weapons and transport. They produced bronze by heating copper and tin with charcoal. * Iron Age (1000 BCE – 1 CE) – iron steel and lead was used for tools‚ weapons and pipes. Iron is much harder than bronze.
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Introduction We are going to do an experiment to see how surface area effects the rate of reaction when added to hydrochloric acid. I will add calcium carbonate (marble chips) to hydrochloric acid. When calcium carbonate is added to hydrochloric acid a reaction takes place. The solution fizzes and gives off the gas carbon dioxide. I will collect this gas in a gas syringe and will time how long it takes for the reaction to produce 100cm3 of carbon dioxide. CaCO3 +2HCL Co2 +CaCl2 +H2O CalciumHydrochloricCarbonCalciumWater
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Title : Expt.1 Determination of the enthalpy (heat) of reaction of a monobasic acid with sodium hydroxide Experiment no : 1 Experiment title : Determination of the enthalpy (heat) of reaction of a monobasic acid with sodium hydroxide Objectives: 1) To understand the enthalpy chemistry. 2) To determine the calorimeter constant. 3) To determine the enthalpy reaction of acid-base reactions. 4) To study the exothermic reaction. Apparatus and Materials : * Dewar flask‚ stopwatch
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Abstract Chemical equilibrium occurs when a reversible reaction is happening forward and backward‚ at the same time by the same amount‚ is equal. Two procedures were made. First is the Effect of Concentration on Equilibrium. The solution became orange when it was diluted with ammonium hydroxide and the solution became yellow when water was added to the solution. In the second‚ Effect of Temperature on Equilibrium‚ the solution turned into a light brown gas when it was placed in the refrigerator
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Redox Reactions Reactions involving oxidation and reduction processes are very important in our everyday world. They make batteries work and cause metals to corrode (or help to prevent their corrosion). They enable us to obtain heat by burning fuels--in factories and in our bodies. Many redox reactions are complex. However‚ combustion and synthesis (from elements) are two ordinary examples which require very little description. Just a little more involved are the displacement reactions‚ with
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