Formula of a Hydrate Lab Wednesday October 29‚ 2014 Chemistry Honors Purpose This lab was done to determine the percentage of water in a hydrate‚ which was CuSO4 ?H20. Not only the percentage of water can be found‚ the moles of water can be found per one mole of anhydrous salt. An anhydrous salt is a hydrate that lost its water. Using various lab equipment such as burners‚ crucible‚ and balance‚ and techniques such as the mass-to-mole ratio and mass to percentage‚ the percentage of water in a hydrate
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oxide to copper (II) sulfate. Our last conversion was from copper (II) sulfate back to a copper metal. During each experiment‚ we will write down observations seen during the chemical reactions. Some reaction will change colors. Others will generate heat. Our goal for this experiment is to “verify the Law of the Conservation of Mass” (CHM111 Laboratory Manual). Procedure The procedure for this experiment was followed using the guidelines found in CHL111 General Chemistry I Laboratory Manual Fall
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reaction) of heat energy. When measured at constant pressure‚ the heat evolved (qp < 0) or absorbed (qp > 0) is equal to the enthalpy change‚ symbolized by ΔH. ΔH is positive for an endothermic process and negative for an exothermic one. If H f is the enthalpy of the final state and Hi of the initial state‚ the enthalpy change for a chemical reaction is given by Equation (1). ∆Hrxn = Hf - Hi (1) The process of measuring ΔH is called calorimetry. This involves “trapping” the heat evolved (or absorbed)
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water streams. The objective of is to evaluate the ability of the EFC process in reducing the volume of a 5 wt% CuSO4 aqueous waste water stream significantly while simultaneously producing potable (drinking) water. In order to evaluate this effectiveness‚ the yield and purity of only the ice product is investigated before and after a number of wash cycles. A 1000g solution of 5 wt% CuSO4 underwent crystallization for one hour with the use of ice crystal seeding and the agitation of a stirrer at
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is mixed in. This mixture is known as Portland Cement. Chemically‚ its main components are 26% dicalcium silicates ( Ca2SiO4); 51% tricalcium silicates (Ca3SiO5); and 11% tricalcium aluminate (Ca3Al2O6). When water is added‚ a number of complex hydration reactions take place. A typical idealized reaction can be represented as 2 Ca2SiO4(s) + 4 H2O(l) Ca3Si2O7. 3H2O(s) + Ca(OH)2(s). The hydrated silicate‚ called tobermorite gel‚ forms strong crystals that adhere by means of strong silicon-Oxygen
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Lab #5 Chemical Reactions & Balancing Equations Objectives Observe and classify several chemical and physical changes. Give evidence for the occurrence of a chemical reaction. Write a balanced equation for a chemical reaction. Identify a reaction as a combination‚ decomposition‚ replacement‚ or combustion reaction. Background Physical properties can be observed without changing the chemical composition of the substance. Common physical properties that can be measured without changing the chemical
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CHEMICAL REACTIONS OF COPPER AND PERCENT YIELD Objective To gain familiarity with basic laboratory procedures‚ some chemistry of a typical transition element‚ and the concept of percent yield. Apparatus and Chemicals |0.5 g piece of no. 16 or no. 18 copper wire |evaporating dish | |250 mL beaker (2) |weighing paper | |concentrated HNO3 (4 – 6 mL)
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fillings - sodium chloride - magnesium ribbon - hydrochloric acid - paper (5 cm x 10 cm) - silver nitarate - birthday candle - sulfur - matches Procedure: 1. Place a small amount of wax from a birthday candle into a test tube. Heat gently over a burner flame until the wax melts completely; then allow the sample to cool. Next‚ light the candle‚ secure it to a glass square‚ and allow it to burn until it extinguishes itself. Proceed with rest of the experiment while the candle burns
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Iron powder will react with cupric sulfate in a onetoone ratio (1 mole to 1 mole). The students will also be able to more easily visualize the size of a mole of iron and copper. The result obtained in this lab usually have less than a one percent error. Fe(s) + CuSO4 (aq) > FeSO4(aq) + Cu(s) Iron powder cupric sulfate ferrous sulfate copper In the reaction‚ iron will be the limiting reagent; it will be completely used up in the reaction. Cupric sulfate will be in excess; not all of it will be used up in the reaction
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Chemical Reactions and their Classifications 26 October 2012 Abstract: Ordinary laboratory ware was used to determine how many of what type of chemical reactions occurred. This yielded three decomposition reactions‚ four substitution reactions‚ and three metathesis reactions. Introduction There are many different types of chemical reactions in the study of chemistry; A composition reaction (also known as synthesis) is defined as the reaction that occurs when two single compounds combine in
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