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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Stoichiometry February 28th‚ 2013 Abstract: The reactions of the Sodium Hydroxide and two acids‚ Hydrochloric Acid and Sulfuric Acid were performed. The heat given off by these two reactions was used to determine the stoichiometric ratio and the limiting reactants in each experiment. Introduction: Coefficients in a balanced equations show how many moles of each reactant is needed to react with each other and how many moles of each product that will be formed. Stoichiometry allows us to
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4.1 & 4.2: General properties of aqueous solutions and Precipitation Reactions: 1. (Brown 4.11) When asked what causes electrolyte solutions to conduct electricity‚ a student responds that it is due to the movement of electrons through the solution. Is the student correct? If not‚ what is the correct response? 2. (Brown 4.15) Specify what ions are present in solution upon dissolving each of the following in water: a. ZnCl2 c. (NH4)2SO4 b. HNO3 d. Ca(OH)2 3. (Brown 4.16 ) Specify
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purposefully 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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Stoichiometry Lab Name Questions A. From your balanced equation‚ what is the theoretical yield of your product? Theoretical yield of the CaCO3 is expected to be .69g. B. According to your data table‚ what is the actual yield of the product? The mass of the filter paper was 1.1g‚ and the total mass of the filter paper when dried with the CaCO3 was 1.8 total. Thus the actual yield of the product was .70g. C. What is the percent yield? Percentage yield is actual yield over the theoretical
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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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STOICHIOMETRY OF GASOLINE. AN INTRODUCTION The internal combustion engines burn fuel to create kinetic energy. The burning of fuel is basically the reaction of fuel with oxygen in the air to form water and Carbon dioxide as the major end product . The amount of oxygen present in the cylinder is the limiting factor for the amount of fuel that can be burnt that is to say it determines the level of burning in our combustion engine. If there’s too much fuel present‚ not all fuel will be burnt and un-burnt
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Stoichiometry lab 1 Purpose: The purpose of this lab is to find the limiting reactant‚ also to find the percentage yield and percentage purity of the reaction that happens between Calcium Chloride and Sodium Carbonate. The other purpose was to know how the reaction can be balanced and created. Hypothesis: In this lab we are going to see a precipitation reaction. This is a reaction where two soluble salts Sodium Carbonate and Calcium Chloride are added together and the result is the precipitation
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Determining the Limiting Reactant and Percent Yield in a Precipitation Reaction Objectives: Observe the reaction between solutions of sodium carbonate and calcium chloride. Determine which of the reactants is the limiting reactant and which is the excess reactant. Determine the theoretical mass of precipitate that should form. Compare the actual mass with the theoretical mass of precipitate and calculate the percent yield. Materials: Balance 0.70 M sodium carbonate solution‚ Na2CO3(aq)
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EXPERIMENT 4 TITLE Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction‚ or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft & Constable‚ 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution‚ it considered as precipitate. Commonly‚ the solid will fall out of the
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