Basic Lab Measurements and Equipment Purpose This lab experiment displays the accuracy of scientific measuring equipment. This experiment also helps to familiarize the students with these instruments. Procedure: Measure Volumes and Masses 1. Obtain a 400mL beaker and record its mass in grams. 2. Add 40mL of water to the beaker and record the volume. 3. Records the beaker’s mass now with the added water 4. Transfer the water from the beaker to a 50mL graduated cylinder and record the measurement
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Stoichiometry and Limiting Reagents Theodore A. Bieniosek I. Purpose and Theory The purpose of the experiment is to study and apply the processes of stoichiometric calculation on a controlled chemical reaction. We will be adding variable amounts of reactants in a chemical reaction in order to demonstrate the effect of limiting reagents. Based on the volumes of the reactants‚ and their respective molarities‚ we can calculate the theoretical yield of the reaction and compare it to the
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experimental research‚ the percent oxygen of potassium chlorate can be determined using tactics such as stoichiometry‚ a technique used to determine the amount of substances that are in a reaction. Stoichiometry is an efficient way to determine how much of a certain substance is within a certain compound‚ which is used in many practical ways‚ such as pharmaceutical companies using stoichiometry to determine how much of a particular chemical is needed to use within a drug. However‚ within certain gas
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Stoichiometry 04/09/12 Chemistry I B Ms. Norton Introduction/Pre-laboratory Assignment: 1. Write out and balance each of the following equations. A. CuSO4 + Fe Cu + FeSO4 B. 3CuSO4 + 2Fe 3Cu + Fe(SO4)3 2. If Iron (III) Sulfate were formed‚ what mass of Copper would be expected and what is the limiting reagent? C. 2.26 g Cu D. Fe 3. If Iron (II) Sulfate were formed‚ what mass of Copper would be expected and what is the limiting reagent?
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Chemistry 1: PROBLEM SET SY 2012/2013 CLASS #: _______________ NAME_________________________________________ SECTION: ______________________ Stoichiometry II - Mole Calculations/ Limiting and Excess Reagent – Lecture Notes 1. Given the balanced equation N2(g) + 3H2(g) 2NH3(g) How many moles of ammonia are produced when 0.60 mol of nitrogen reacts with hydrogen? 2. Given the equation: SiO2 + HF SiF4 + H2O a. Calculate the number of moles HF that would completely react with 2.5 moles of
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something + 2Fe+2 Equation 2: 8H+ + 5Fe+2 + MnO4- --> 5Fe+3 + Mn+2 + 4H2O Equation 3: 6H+ + 2MnO4- + 5H2C2O4 --> 2Mn+2 + 10CO2 + 8H2O Conclusion: Therefore the concluded reaction would be: NH3OH+ + 2Fe+3 --> N2O + 2Fe+2 This was obtained by using stoichiometry half reactions the product of that reaction was determined to be N2O. Some systematic errors could be if the wrong molarity was determined for the permanganate because then that would though off the calculations for the Fe+2 and the rest of the
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moles-stoichiometry-practice-problems Now you’re ready to use what you know about conversion factors to solve some stoichiometric problems in chemistry. Almost all stoichiometric problems can be solved in just four simple steps: 1.Balance the equation. 2.Convert units of a given substance to moles. 3.Using the mole ratio‚ calculate the moles of substance yielded by the reaction. 4.Convert moles of wanted substance to desired units. These "simple" steps probably look complicated at first
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Name: Brian James|Date:3/10/13| Exp 9: Stoichiometry of a Precipitation Reaction|Lab Section: 73426| Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 CaCl2.H2O(aq)= m/M =1/147 =0.0068 mol CaCO3(s)=0.0068*1/1 =0.0068 mol CaCO3(s)= CaCO3 (s)= CaCO3 mol *CaCO3 g =0.0068 mol*100.01 g =.68 g Step 4: Mass of weighing dish _0.6_g Mass of weighing dish and Na2CO3 .72_g Net mass of the Na2CO3 .12_g Step 6: Mass of filter paper
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combining the elements‚ instead of having it naturally do so‚ made a significantly fully more bright color. In Theophilus’s “recipe” for vermillion‚ it is stated that there should be far more sulfur than a stiochiometric reaction should require. Stoichiometry
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Title: Stoichiometry of a Precipitation Reaction Purpose: The purpose is to predict the amount of precipitation using stoichiometry. Another purpose is to measure and calculate percentage yield. Procedure: 1. Weigh out 1.0g of CaCl2*2H2O and put it into a 100mL beaker. 2. Add 25mL of distilled water and stir. 3. Using stoichiometry to determine how much Na2CO3 is needed for a full reaction. 4. Weigh the calculated amount and put it in a small paper cup. Add 25mL distilled water and stir
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