Determining the Empirical Formula of Magnesium Oxide‚ students set out to find if there is a true 1:1 ratio in the empirical formula of MgO. This was determined by burning the Magnesium until a white smoke started to protrude. This showed the reaction of Oxygen combining with Magnesium to form Magnesium Oxide. This was then measured again and turned out to be slightly heavier than the measurement before. This added weight is Oxygen‚ forming the combustion of Magnesium Oxide. The formula for Magnesium
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going to determine the empirical formula of a compound? Do Now: 1) What is the percent by mass of oxygen in H2C2O4? H2 = 2(1) = 2 ; C2 = 2(12) = 24 ; O4 = 4(16) = 96 Gram Formula Mass = 90 Percentage of Oxygen = 6490 x 100 = 71% 2) Calculate the percentage of water: -Mass of empty crucible and cover = 11.7g -Mass of crucible‚ cover‚ and hydrate before heating = 14.9g -Mass of crucible‚ cover‚ and anhydrous after heating = 14.53g 14.9g-11.7g = 3.2g (mass of hydrate) ; 14.9g-14.53g = .37g
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heating | 40.00 grams | Mass of crucible + hydrate before heating | 41.38 grams | Mass of crucible + anhydrate after 1st heating | 41.08 grams | Mass of hydrate | 1.38 grams | Mass of anhydrate | 1.08 grams | Mass of water | .2 grams | Formula of anhydrous salt | Cu(SO4) – Copper Sulfate | Data Table Calculations 1. Mass of hydrate = 1.38 grams. Mass of anhydrous = 1.08 grams. Mass of water = .2 grams. 2. Ratio of anhydrous mass to hydrate mass is 5.4. 3. Moles of anhydrous
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ABSTRACT By calculating the difference in the mass of the hydrate copper (II) sulfate and the anhydride we were able to determine the mass of water in the hydrate. This information was then used to determine the empirical formula of the hydrate‚ defined as a compound formed by the addition of water to another molecule. In the first trial‚ the mass of water in the hydrate was determined to be 0.41 g‚ while in the second trial the mass of water was 0.52 g. Moles of water associated with a single
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Empirical Formula of Copper (II) Chloride Gabriella Jane Lukas B1401404 HELP University Empirical Formula of Copper (II) Chloride Objectives 1. To validate that the empirical formula of copper (II) chloride is . 2. To calculate the percent composition of copper in copper (II) chloride. 3. To illustrate the Law of Constant Composition in copper (II) chloride. 4. To study the reaction between copper (II) chloride solution and aluminium metal. Introduction One of the most fundamental statements
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Hydrates Analysis NAME:_____________________________________ PERIOD:_________ Prelab 1. A 6.00g sample of calcium sulfate hydrate (CaSO4.x H2O) is heated until all the water is driven off. The anhydrous compound has a mass of 4.77 g. Calculate the value of x in the formula. 2. For the data in problem number 1 above‚ what is the mass percent water in the hydrate? 3. Calculate the number of grams of water that could be obtained by heating 2.00 g
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Lab #6 Properties of Hydrates Purpose: The purpose of the “Properties of Hydrates” lab is to study hydrates‚ and be able to identify them. This lab also focuses on observing the reversibility of hydration reactions by hydrolysis‚ and also testing substances for efflorescence of deliquescence. Procedure: A. Identification 1. Place 0.5 grams of each compound (Nickel Chloride‚ Potassium Chloride‚ Sodium Tetraborate‚ Sucrose‚ Calcium Carbonate‚ and Barium Chloride) in a small dry test
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Chen and Alexander Van Buren 9/15/11 AP Chemistry Dr. Isotone Lab 1: Determination of the Empirical Formula of Silver Oxide Lab Objective: In this experiment‚ the percent composition and empirical formula of silver oxide will be determined. Silver oxide will be heated until it decomposes to silver metal and oxygen‚ and the percent calculation and empirical formula can be calculated based on combining the ratios of silver and oxygen in the reaction. Summary of Lab Procedure:
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What is the Identity of this Hydrate? Date Performed: May 30‚ 12 Date Submitted: June 6‚ 2012 Name: 2968 Instructor: Reid A hydrate was given to our group and the identity of the hydrate was unknown. The lab workers were told to determine the identity of the unknown hydrate. The identity of the hydrate could be determined by calculating the hydrate’s percent of water. So the lab workers set out to determine the water percent of the unknown hydrate. The percent of any compound or element
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Formula of a Hydrate Lab Design: Problem: What is the chemical formula for a hydrated copper (II) sulphate compound? Controlled Variable: The mass of hydrated copper (II) sulphate. Responding Variable: The mass of dehydrated copper (II) sulphate‚ mass of H2O Materials: Ones on the handout + Hot plate. Procedure: 1. Mass 3.00g of hydrated copper (II) sulphate using electronic balance 2. Measure the mass of a thin‚ crucible dish using electronic balance 3. Gently pour hydrated
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