A The % Composition and Empirical Formula of a Hydrate: It Doesn’t Hold Water‚ Or Does It? 1. To determine the percent water in an unknown hydrate. 2. To calculate water(s) of crystallization for an unknown hydrate. 3. To determine the formula of an unknown hydrate. OBJECTIVES SKILLS Proper use of the following equipment: Dial-O-Gram balance (Laboratory Technique I)‚ electronic balance (Laboratory Technique II) and Bunsen burner (Laboratory Technique III). Dial-O-Gram balance‚ electronic
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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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THE MOLE A mole (symbol Mol) is the base unit of quantity of a substance in the metric system. A mole is the quantity of a substance that contains 6.02 x 1023 units. A "unit" is the smallest measurable entity in the substance‚ generally either an atom or a molecule. The number of units in a mole was determined by Italian chemist (a scientist specializing in the composition‚ structure‚ properties‚ and reactions of matter) Amedeo Avogadro (1776-1856)‚ one of the founders of modern physical chemistry
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In this lab we studied stoichiomentry. We also reviewed the mole-mole relationship between copper and iron in a chemical reaction. The stoichiomentry of mass is that during the heating the experiment does loose mass .This mean that mole and mass did change. An Example of real world is Masses and volumes of products are extremely important in key reactions such as the deployment of air bags in vehicles‚ carbon dioxide production to help bread rise‚ and the Production of ammonia gas for industries
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AP* Chemistry CHEMICAL EQUILIBRIA: GENERAL CONCEPTS THE NATURE OF THE EQUILIBRIUM STATE: Equilibrium is the state where the rate of the forward reaction is equal to the rate of the reverse reaction. At these conditions‚ concentrations of all reactants and products remain constant with time once equilibrium has been established at constant temperature. (In stoichiometry‚ we dealt with equations that went to completion; often equilibrium equations are going to fall short of this goal.) Reactions are
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crystal lattice in a specific ratio. 2b. For every mole of copper sulfate‚ there are five moles of water. 2c. The molar mass of copper (II) sulfate is 159.61 grams/mol 2d. The molar mass of 5H2O is 90.10 grams/mol 2e. The molar mass of the entire compound is 159.61 + 90.10 = 249.71 grams/mol 2f. The percent of water in the compound is mass of water/mass of compound = 36% Mass of crucible before heating | 40.00 grams | Mass of crucible + hydrate before heating | 41.38 grams | Mass of crucible
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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 mole of anhydride were then calculated
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Title: Finding the Ratio of Mole of Reactants in a Chemical Reaction Purpose of Lab: To find the coefficients of two chemical reactants that appears in a balanced chemical equation using the continuous variations method. Pre Lab Questions: 1. 2AgNO3(aq) + K2CrO4(aq) → 2KNO3(aq) + Ag2CrO4(s) 2. There is enough to make a valid conclusion because‚ on the graph‚ one can clearly see that the two lines intersect. Thus‚ one can also determine the mole ratio. The mole ratio is approximately 2:1
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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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purpose of this lab was to study the composition of hydrates. Hydrates are ionic compounds that are chemical compositions made of water and salt. A main objective was to remove water from the hydrate by heating‚ and determine the amount of water that was in the hydrate. After doing this‚ one had to predict the empirical formula for hydrated copper sulfate. In doing this lab‚ one was able to see the gradual change in the composition of a hydrate into an anhydrous salt. The lab was carried out with
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