Name __________________________________ Period _________ GAS STOICHIOMETRY WORKSHEET Please answer the following on separate paper using proper units and showing all work. Please note that these problems require a balanced chemical equation. 1. Carbon monoxide reacts with oxygen to produce carbon dioxide. If 1.0 L of carbon monoxide reacts with oxygen at STP‚ a. how many liters of oxygen are required to react? b. How many liters of carbon dioxide are produced? 2. Acetylene gas (C 2H2) undergoes
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Chemistry 1035 – General Chemistry I Fall Semester‚ 2013 3 hours credit‚ CRN 91627 Office Hours (Randolph 144) Preston Durrill‚ Instructor M 8:00-9:00‚ 1:30-5:00 Randolph Hall‚ Room 144 Tu 9:00-11:00‚ 4:00-5:00 Office phone: 540-231-6774 W 8:00-9:00‚ 1:30-5:00 Home phone: 540-961-5179 Th 9:00-12:00‚ 4:00-5:00 e-mail: pdurrill@vt.edu F 8:00-9:00‚ 1:30-3:00 Class times: 2:00-3:15 Tuesday and Thursday in McBryde 100. Evening help sessions: Wednesdays 5:00-6:30 p.m. in Hancock
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cupric sulfate is reduced and the iron powder is oxidized. (Copper goes from a +2 oxidation state to a zero oxidation state while iron goes from a zero oxidation state to a +2 oxidation state.) 2 Purpose Statement We will determine the meaning of a mole and stoichiometry relations using oxidationreduction and single replacement reaction. We will determine the reaction that iron powder has with cupric sulfate in a onetoone ratio. Materials Cupric Sulfate pentahydrate‚ (CuSO4 x 5H2O‚
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ACID BASE TITRATION OBJECTIVES 1. To demonstrate the basic laboratory technique of titration 2. To learn to calculate molarity based on titrations INTRODUCTION Molarity (M) or molar concentration is a common unit for expressing the concentration of solutions. It is defined as the number of moles of solute per liter of solution (or millimoles of solute per milliliter of solution). The concentration of a basic solution can be determined by titrating it with a volume of a standard acid solution (of
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details go to http://research.lonestar.edu/cat/catsrch.asp Catalog Description: This course is a preparatory course for students who have never had chemistry and covers the metric system‚ atoms and elements‚ bonding‚ solids‚ liquids‚ gases‚ stoichiometry‚ solutions‚ reactivity‚ and acids and bases. The lab includes experiments in inorganic chemistry. This course is appropriate for some nursing students‚ as well as students who will pursue higher level chemistry. Student Learning Outcomes: 1
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Ratios: NaOH and HCl & NaOH and H2SO4 Reactions Contents Introduction 3 Materials & Procedure 4 Raw Data 8 Processed Data 15 Graphs 16 Conclusion & Evaluation 17 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
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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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Introduction to the Magnetic Treatment of Fuel By R.J. Kita Hydrogen is the lightest and most basic element known to man. With its simple structure comprised of only one proton and one electron‚ it is one of the major constituents of all hydrocarbon based fuels. By studying the response of hydrogen with respect to magnetic fields and the accompanying increased energy output‚ much can be learned and applied to other related fuels. In the oxidation/combustion of hydrocarbon fuels‚ it is the outer shell
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Lab Report: Titration Lab Prepare a solution of a given concentration; understand titration including acid-base reactions‚ pH‚ stoichiometry and molar equivalence. Chemicals and equipment: NaOH pellets close to purity‚ HCl 3M‚ phenolphtalein Beckers‚ flasks‚ burette‚ magnetic or manual stir pHmeter Waste management: The waste disposal will be handled through neutralization of your excess reactant to a pH between 4.0 and 10.0 and disposal with abundant rinsing. As a preparation for the
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prepare the standard. Reagents used as standards are divided into primary reagent and secondary reagent. A primary reagent can be used to prepare a standard containing an accurately known amount of analyte. A primary reagent must have a known stoichiometry‚ a known purity (or assay) and be stable during a long term storage both in solid and solution form. The purity of a secondary reagent in a solid form or the concentration of a standard prepared from a secondary reagent must be determined relative
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