1. A 15‚67g sample of hydrate of magnesium carbonate was carefully heated‚ without decomposing the carbonate‚ to drive off the water. The mass was reduced to 7.58g.What is the formula of the hydrate? (10) 2. Construct balanced equations (including state symbols) to describe the following reaction: Potassium metal reacts with water to form potassium hydroxide solution and hydrogen gas (dihydrogen). (8) 3. Anhydrous lithium perchlorate (4.78g) was dissolved in water and recrystallized. Care was taken
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GAS HYDRATES AND THE ENVIRONMENT POTENTIAL FUTURE FUEL FOR THE ECONOMY GAS HYDRATES AND THE ENVIRONMENT POTENTIAL FUTURE FUEL FOR THE ECONOMY Thomas Harding SEDV 601 Thomas Harding SEDV 601 Fariha Abedin‚ Nisa Choudhary‚ Romaine Mcleary Fariha Abedin‚ Nisa Choudhary‚ Romaine Mcleary Contents ABSTRACT 1 INTRODUCTION 2 DISTRIBUTION 3 WHAT ARE NATURAL GAS HYDRATES? 4 WHERE DO NATURAL GAS HYDRATES FORM? 5 POSSIBLE PRODUCTION METHOD: 6 Thermal Injection: 6 Inhibitor Injection:
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January 4‚ 2013 Chemistry Honors Title: Hydrates Purpose: To find the mass percentage of water in the hydrate. Materials: * Watch glass * 2.82 g hydrated crystal (CuSO4*5H2O) * Evaporating dish * Bunsen burner * Electronic balance * Metal tongs * Ring stand Procedure: 1) Determine the mass of evaporating dish and watch glass. 2) Add between 2 and 3 grams of the hydrated crystal to the evaporating dish. 3) Determine the mass of the dish and crystal
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lab in which we conducted last Tuesday was an analysis of a hydrate and what happens to it when it is heated. A hydrate is a crystalline compound which water molecules are chemically bound to it. In the lab‚ we were to analyze the difference in grams of the hydrate and the anhydrate. An anhydrate is the crystalline compound without the water molecules bound to it. During our lab‚ we were to heat up the crucible‚ the crucible with hydrate‚ and the crucible with an anhydrous and write down each weight
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Determining Percent of Water Crystallization and the Chemical Formula of a Hydrate Aim: To determine the percent water of crystallization and the chemical formula of a hydrate Materials * 400 ML beaker * Glass rod * 3 to 5 grams of hydrated copper (II) sulfate CuSO4 (crushed) * Bunsen burner * Spatula * Heating pad * Clamp and stand * Electronic balance Procedures Refer to Lab sheet Observations 1. The powder seems to be very bright and shiny before any heating 2.
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Determination of Water in a Hydrate DESIGN – Aspect 1: Defining the problem & selecting variables Research Question: What percentage of Copper Sulfate Hydrate is water? Background Information: There are many ionic compounds that contain one or more waters of hydration in their formulae. They exists either in anhydrous or hydrated form. Most anhydrous compounds have a strong tendency to absorb water from the humidity in the atmosphere and shifts into a hydrated form. Because of
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tests. The hydrate is solid crystals compound and appears to be dry: since an ionic compound (salt) is crystallized from an aqueous solution (water)‚ by heating the hydrate the water is released from ionic structure; therefore it is possible to measure the weight of the ionic compound and calculate its ratio to the liquid in the hydrate. The goal of the lab is to establish the identity of a given hydrate (“wet salt”) by comparing the results with known hydrate percentages. Hydrates are ionic compounds
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Lisa Margonelli examines what methane hydrates are‚ the capabilities of methane hydrates‚ and the potentially detrimental affects methane hydrates can have on global warming. Methane hydrates exist in the seabed along coastlines around the world and are massive deposits of gas that are trapped in large‚ icy structures underneath the coastal sea floor. Despite inadequate funding‚ scientists around the world are conducting experiments to determine if methane hydrates can serve as a solution to the energy
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Experiment 5 – Percent Water in a Hydrated Salt Pre-Lab Hints 1. Note definition of deliquescent in the introduction. 2. See side notes for part A‚ as well as part 1 of Technique 15C (pg 27). 3. Mass of water in sample is the mass lost by heating (initial minus final). Water % is 100 times the g of water divided by the initial g of hydrate sample. 4. a. See step A1 in the procedure. b. A hot sample on the balance creates air currents and causes thermal expansion‚ both of which decrease
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Shawn Dubbs Lab 1 The Mole Concept of and the Chemical Formula of a Hydrate Abstract: The objective of this lab was to conduct an experiment to analyze the molar components in alum. This was conducted by heating the alum till the water had evaporated and then determining the number of moles for each component. Then using the these amounts to figure out the empirical formula for alum. Results: In order to determine how much of each separate component a total mass was taken before hand for
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