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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Chapter 8: Salts 1. Salts A salt is an ionic compound. The anion part comes from the acid while the cation part comes from a base. Example: KCl‚ KOH(aq) + HCl(aq) KCl(aq) + H2O(l) A salt is a compound formed when the hydrogen ion. H+ from an acid is replaced by a metal ion or an ammonium ion‚ NH4+. Salts Nitrate salts Carbonate salts Chloride salts Soluble All nitrate salts Potassium carbonate‚ K2CO3 Ammonium carbonate‚ (NH4)2CO3 Sodium carbonate‚ Na2CO3 All chloride salts Except Sulphate salts
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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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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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2x + (-2) 4 = -2 x= 3 e)N in HNO2): +3 f) Cr in Cr2O72- +6 4.56) a) Mn(s) + NiCl2 (aq) -> MnCl2((aq))+Ni(s) b) Cu(s) + Cr(C2H3O2) (aq)-> NR C) 2Cr(s)+ 3NiSO4(aq) -> Cr2(SO4)3(aq)+ 3Ni(s) d) Pt(s) + HBr(aq) -> NR e) H2 (g) + CuCl2 (aq) -> Cu(s) + 2HCl (aq) 4.64) Calculate the mol of Na + at the two concentrations; the difference is the mol NaCl required to increase the Na + concentration to the desired level. 0.118mol/L *4.6L =
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Chem 201 Lab October 21‚ 2011 Lab #6: Preparation of 2-chloro-2-methylbutane – an Sn 1 Reaction Purpose The purpose of this experiment was to prepare an alkyl halide‚ 2-chloro-2-methylbutane by reacting 2-methyl -2-butanol (t-amyl alcohol) with hydrochloric acid. Alkyl halides are of wide interest because they are widespread and have diverse beneficial and detrimental impacts .The overall reaction is given below: Procedure 1 ml of 2-methyl-2-butanol was measured using 1 ml syringe and
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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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percent yields will be determined and reported. Objective: To determine the limiting reactant‚ theoretical yield‚ actual yield‚ and percent yield in a chemical reaction between solutions of potassium iodide and lead (II) nitrate. Introduction: Stoichiometry‚ mass‚ and mole relationships have been important throughout the history of chemistry. The simplest whole number relationship between the products and the reactants is a chemical equation. If the masses or number of moles of reactants are known
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