Introduction to Chemistry Laboratory: A Lesson on Tools‚ Techniques and Measurements PURPOSE: The purpose of this set of experiments (3 total) is to become familiar with the common types of laboratory glassware and equipment‚ and how to obtain and analyze data from these items. LEARNING OBJECTIVES: By the end of this experiment‚ the student should be able to demonstrate the following proficiencies: 1. Know which glassware (beakers‚ burettes‚ pipettes‚ graduated cylinders‚ flasks‚ etc) should
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Introduction Background Information Stoichiometry is a critical component in chemistry‚ and helps in understanding the quantitative relationship between the number of moles of reactants and products in a reaction. Objective In this experiment‚ the reactions between sodium hydroxide and hydrochloric acid‚ and sodium hydroxide and sulfuric acid will be studied. Beginning Questions When will the maximum extent of the reaction occur? Which will the limiting reagent? Which of the two acid-base combinations
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Reaction Equation: Theoretical Yields: Based on limiting moles of product -Based on C7H14O 24 mL C7H14O x (0.910 g C7H14O/1 mL C7H14O) x (1 mol C7H14O/114.19 g C7H14O) = 0.191 mol C7H14O 0.191 mol C7H14O x (1 mol C7H12/1 mol C7H14O) = 0.191 mol C7H12 C7H14O is the Limiting Reagent -The acids are not counted as reagents in this reaction and serve only as catalyst. Theoretical Yield = mol of limiting reagent x M.W. = 0.191 mol x 96.17 C7H12
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calcium chloride were used up. Also to see if there’s any alterations like mass differentials. Objectives: 1. To introduce the concept of “limiting factor” in a chemical reaction 2. To practice a. Writing a balanced equation b. Determining the number of moles of each reactant and product c. Deciding which chemical is the limiting factor d. Predict theoretical yield e. Determine actual yield f. Use error discussion Materials: * 2 beakers * 2
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experiment was demonstrated by adding the reagents like 16M HNO3‚ Distilled water‚ 6M NaOH‚ 6M H2SO4‚ Acetone‚ Zinc metal and Methanol into the beaker with the copper wire. The experiment was also demonstrated to observe how copper reacts while different reagents were being added. It was also demonstrated to practice the common laboratory techniques such as methods of separation involving filtration‚ sedimentation‚ decantation and extraction. While different reagents were added to the copper wire‚ different
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Ms. Azlina Banu‚ Ms. Farhanah‚ Ms.Gurpreet‚ Ms. Jamie‚ Ms. Lau Mei Chien‚ Ms. Lily Lee‚ Ms. Nabilah‚ Mr. Ng Sweet Kin‚ Ms. Phang Ying Ning‚ Ms. Precilla‚ Ms. Rachel Tham‚ Ms. Rajalakshmi‚ Mr. Sivabalan‚ Ms. Tan Lee Siew Tutorial 3: Chapter 3 Stoichiometry and Solution Concentration 1. Balance the following equations: (a) (b) 2. V2O5(s) + CaS(s) CaO(s) + V2S5(s) GaBr3(aq) + Na2SO3(aq) Ga2(SO3)3(aq) + NaBr(aq) 316.0 g of aluminum sulfide‚ Al2S3 reacts with 493.0 g of water‚ H2O. Given the
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greater than 50° C. Our results displayed 5.70% 2‚4-dinitrotoluene and 1.53% 2‚6-dinitrotoluene. The compound is mixed with diethyl ether to isolate the organic products. This resulted in a light yellow mixture. It was then washed twice with 5% Na2CO3 because it is an ionic solution (more ionic than water) and will bond to the H+ ions. This resulted in a bright yellow mixture. Anhydrous CaSO4 is used as a drying agent. It absorbs all of the H2O in the mixture. If H2O is present‚ then the product
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drops of our product and the other different compounds into different test tubes along with 1mL of ethanolic silver nitrate reagent. We are comparing these by seeing how they react and if there is no reaction after 5 minutes we will place the test tubes in a beaker of water that is heated at a temperature of 70oC-80oC and observe what happens. Experimental Stoichiometry Compound | Molecular Weight | Quantity | Moles |
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of CaCl2·2H2O and .72 or .8 g (slight excess) Na2CO3 Should give a CaCO3 theoretical yield as follows: 1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol CaC03 x 100 g CaC03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol CaC03 To double-check‚ we can calculate CaCO3 theoretical yield by using Na2CO3 0.72 g Na2C03 x 1 mol Na2C03 x 1 mol CaC03 x 100 g CaC03 = 106 g Na2C03 1 mol Na2C03 1 mol CaC03 www.LabPaq.com 56 ©Hands-On Labs‚ Inc. Experiment Stoichiometry of a Precipitation Reaction Questions A. From
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is titrated with an HCl titrant‚ standardized by 1o Na2CO3. The indicators used are phenolphthalein for basicity and methyl orange for acidity. The two volumes of the titrant are then used to calculate percent composition of soda ash analyte. Statistical parameters such as relative standard deviation and confidence limits are also calculated. At the end of the experiment‚ the calculate percent /calculated average percent by mass of Na2CO3 is 27.6% with a relative standard deviation of 64.1 ppt
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