...Preparation of 1-Bromobutane The mechanism is SN2. The overall reaction is: H2SO4 + NaBr + CH3CH2CH2CH2OH 6 CH3CH2CH2CH2Br + H2O + NaHSO4 Boiling Point 118oC Boiling Point 92oC Day 1 CAUTION: Wear gloves during the entire experiment Fill out the table on your lab report form for this experiment INCLUDING YOUR NAME AND DATE and turn it in to the instructors box in NSM B-202 by 10:AM the day of the experiment. BE SURE TO DATE-STAMP YOUR LAB REPORT FORM USING THE DATE STAMP IN THE DEPARTMENT OFFICE (NSM-B-202) BEFORE PLACING IT INTO YOUR INSTRUCTORS BOX. FAILURE TO DO SO WILL RESULT IN YOUR FORM BEING MARKED "LATE". The report form will be returned to you in the lab. At your hood workstation, place a hotplate/stirrer atop a ringstand . Take a 250-mL round-bottomed flask, and clamp the flask to the ringstand, leaving about 1 inch of room between the bottom of the flask and a plastic bowl, whish sits atop the hotplate/stirrer.. Add 0.3 mole 1-butanol and ABOUT 35mL H2O to the flask and begin stirring the solution with the magnetic stirrer. CAREFULLY add 0.3 mole NaBr to the reaction flask. NOW, Add a slurry of ice and water to the bowl beneath the flask. S L O W L Y AND CAREFULLY add 35mL conc. H2SO4 to the flask. Remove the ice bath and replace it with a heating mantle. Add two or three boiling chips to the flask. Equip the flask with a reflux condenser and begin circulating...
Words: 1061 - Pages: 5
...+ ____ Br2 ( ____ CBr4 + ____ F2 7) ____ HCN + ____ CuSO4 ( ____ H2SO4 + ____ Cu(CN)2 8) ____ GaF3 + ____ Cs ( ____ CsF + ____ Ga 9) ____ BaS + ____ PtF2 ( ____ BaF2 + ____ PtS 10) ____ N2 + ____ H2 ( ____ NH3 11) ____ NaF + ____ Br2 ( ____ NaBr + ____ F2 12) ____ Pb(OH)2 + ____ HCl ( ____ H2O + ____ PbCl2 13) ____ AlBr3 + ____ K2SO4 ( ____ KBr + ____ Al2(SO4)3 14) ____ CH4 + ____ O2 ( ____ CO2 + ____ H2O 15) ____ Na3PO4 + ____ CaCl2 ( ____ NaCl + ____ Ca3(PO4)2 16) ____ K + ____ Cl2 ( ____ KCl 17) ____ Al + ____ HCl ( ____ H2 + ____ AlCl3 18) ____ N2 + ____ F2 ( ____ NF3 19) ____ SO2 + ____ Li2Se ( ____ SSe2 + ____ Li2O 20) ____ NH3 + ____ H2SO4 ( ____ (NH4)2SO4 Balancing Equations Worksheet – Answers Note to students: It is acceptable to leave spaces blank when balancing equations – blank spaces are interpreted as containing the number “1”. 1) 1 Na3PO4 + 3 KOH ( 3 NaOH + 1 K3PO4 2) 1 MgF2 + 1 Li2CO3 ( 1 MgCO3 + 2 LiF 3) 1 P4 + 3 O2 ( 2 P2O3 4) 2 RbNO3 + 1 BeF2 ( 1 Be(NO3)2 + 2 RbF 5) 2 AgNO3 + 1 Cu ( 1 Cu(NO3)2 + 2 Ag 6) 1 CF4 + 2 Br2 ( 1 CBr4 + 2 F2 7) 2 HCN + 1 CuSO4 ( 1 H2SO4 + 1 Cu(CN)2 8) 1 GaF3 + 3 Cs ( 3 CsF + 1 Ga 9) 1 BaS + 1 PtF2 ( 1 BaF2 + 1 PtS 10) 1 N2 + 3 H2 ( 2 NH3 11) 2 NaF + 1 Br2 ( 2 NaBr + 1 F2 12) 1 Pb(OH)2 + 2 HCl ( 2 H2O + 1 PbCl2 13) 2 AlBr3 + 3 K2SO4 ( 6 KBr + 1 Al2(SO4)3 14) 1 CH4 + 2 O2 ( 1 CO2 + 2 H2O 15) 2 Na3PO4 + 3 CaCl2 ( 6 NaCl + 1 Ca3(PO4)2 16) 2 K + 1 Cl2 ( 2 KCl 17) 2 Al + 6 HCl ( 3 H2 + 2 AlCl3 18) 1 N2 +...
Words: 397 - Pages: 2
......
Words: 1192 - Pages: 5
...UNIVERSITI TUNKU ABDUL RAHMAN Centre Course Year/ Trimester Lecturer : : : Centre for Foundation Studies Foundation In Science Year 1 Trimester 1 Unit Code Unit Title Session : : : FHSC1114 Physical Chemistry 2015/05 : Ms. Amelia Chiang, 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 unbalanced equation as below: Al2S3(s) + H2O(l) → Al(OH)3(s) + H2S(g) (a) Find the excess reactant. (Ans: H2O) (b) Find the mole of the excess reactant that remains after the reaction. (Ans: 14.742 mole) [Sep 2014] 3. Consider the reaction below: 2Al(s) + 3I2(s) 2AlI3(s) (a) Determine the limiting reagent and the theoretical yield of the product if 1.20 moles of aluminium and 2.40 moles of iodine are used. (Ans: 489.218 g) (b) Calculate the percentage yield of the product if 450 g of AlI3 is obtained. (Ans: 91.98%) 4. A salt solution is produced when 2.9 g of sodium chloride, NaCl dissolved in 200 ml of water. Calculate the molality (m) of the NaCl solution...
Words: 365 - Pages: 2
...UNIVERSITI TUNKU ABDUL RAHMAN Centre Course Year/ Trimester Lecturer : : : : Centre for Foundation Studies Foundation In Science Year 1 Trimester 1 Unit Code Unit Title Session : : : FHSC1114 Physical Chemistry 2014/05 Ms Azlina Banu, Mr Tam Yun Hong, Ms Chong Pui Kuan, Ms Amelia Chiang Kar Mun, Ms Farhanah, Ms Wong Jing Tyng, Ms Jamie Anne, Ms Lau Mei Chien, Mr Ng Sweet Kin, Ms Phang Ying Ning, Ms Precilla, Ms Rachel Tham, Ms Rajalakshmi, Mr Tan Jun Bin, Ms Tan Lee Siew Tutorial 3 : Chapter 3 Stoichiometry and Solution Concentration 1. Balance the following equations: (a) Al(s) + NH4ClO4(s) → Al2O3(s) + AlCl3(s) + NO(g) + H2O(g) (b) GaBr3(aq) + Na2SO3(aq) → Ga2(SO3)3(aq) + NaBr(aq) 2. Ethanol, C2H5OH, is a liquid with a density of 0.789 g ml-1 at 25 °C. Calculate the molarity of ethanol solution made by dissolving 20.00 mL of ethanol at 25 °C in enough water to make 250.0 ml of solution. [Ans: 1.37 mol L-1] 3. Copper sulfate is widely used as a dietary supplement for animal feed. A lab technician prepares a “stock” solution of CuSO4 by dissolving 79.80 g of CuSO4 in enough water to make 500.0 mL of solution. (a) Determine the molarity of the CuSO4 “stock” solution prepared by the technician. [Ans: 1 mol L-1] (b) Calculate the volume of CuSO4 “stock” solution that should be diluted to give 2.5 L of [Ans: 0.25 L] 0.1 M CuSO4. 4. Aluminum is a limiting reactant in the reaction with sulfur gas to form aluminum sulfide. Initially, 1.18 mol of aluminum and 2.25 mol of...
Words: 447 - Pages: 2
...Reaction Products (cont.) For each of the following double replacement reactions, determine what the products of each reaction will be. When you have predicted the products, balance the equation and use a solubility to determine which of the products (if any) will precipitate (be insoluble). Assume all reactions take place in aqueous solutions (aq). 1) ____ Ca(OH)2 + ____ HF ( 2) ____ Pb(NO3)2 + ____ K2CrO4 ( 3) ____ NaC2H3O2 + ____ H2SO4 ( 4) ____ Cu(OH)2 + ____ H3PO4 ( 5) ____ AgNO3 + ____ Na2CO3 ( 6) ____ Pb(OH)2 + ____ Hg2S ( Predicting Reaction Products - Solutions Balance the equations and predict the products for the following reactions: 1) 3 Na + 1 FeBr3 ( 3 NaBr + 1 Fe 2) 2 NaOH + 1 H2SO4 ( 1 Na2SO4 + 2 H2O 3) 1 C2H4O2 + 2 O2 ( 2 CO2 + 2 H2O 4) 1 NH3 + 1 H2O ( 1 NH4OH 5) 1 PbSO4 + 2 AgNO3 ( 1 Ag2SO4 + 1 Pb(NO3)2 6) 4 PBr3 ( 1 P4 + 6 Br2 7) 2 HBr + 1 Fe ( 1 H2 + 1 FeBr2 OR 6 HBr + 2 Fe ( 3 H2 + 2 FeBr3 8) 2 KMnO4 + 1 ZnCl2 ( 2 KCl + 1 Zn(MnO4)2 9) 1 MnO2 + 1 Sn(OH)4 ( 1 Mn(OH)4 + 1 SnO2 10) 7 O2 + 1 C5H12O2 ( 5 CO2 + 6 H2O 11) 1 H2O2 ( 1 H2 + 1 O2 OR 2 H2O2 ( 2 H2O + 1 O2 12) 1 PtCl4 + 1 Cl2 ( 1 PtCl6 Reaction Products Worksheet - Key For each of the following reactions, determine what the products of each...
Words: 487 - Pages: 2
...are mixed, by using a table of solubilities. The table indicates the solubilities of ionic substances in water under normal laboratory conditions. Solubility of common ionic substances* Soluble anions | Exceptions | Insoluble anions | Exceptions | NO3- | None | OH- | Na+, K+, Ba2+ soluble; Ca2+ slightly soluble Note: NH4OH exists as NH3(aq) | Cl- | Ag+ insoluble, Pb2+ | | | Br- | | | | I- | | | | SO42- | | | | AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) Equation with formulas The net ionic equation most accurately represents what occurs when the reaction takes place. Examples of precipitation reactions Solutions mixed | Precipitate formed | Net ionic equation | AgNO3 and NaBr | AgBr | Ag+(aq) + Br-(aq) > AgBr(s) | | | | | |...
Words: 419 - Pages: 2
...1. (a) By referring to electrons, explain the meaning of the term oxidising agent. ..................................................................................................................................... (1) (b) For the element X in the ionic compound MX, explain the meaning of the term oxidation state. ..................................................................................................................................... (1) (c) Complete the table below by deducing the oxidation state of each of the stated elements in the given ion or compound. |Oxidation state| Carbon in CO|| Phosphorus in PCl|| Nitrogen in Mg3N2|| (3) (d) In acidified aqueous solution, nitrate ions, NO, react with copper metal forming nitrogen monoxide, NO, and copper(II) ions. (i) Write a half-equation for the oxidation of copper to copper(II) ions. ........................................................................................…............................... (ii) Write a half-equation for the reduction, in an acidified solution, of nitrate ions to nitrogen monoxide. ........................................................................................…............................... (iii) Write an overall equation for this reaction. ........................................................................................…............................... (3) (Total 8 marks) 5. (a) The following is an equation for a redox reaction. ...
Words: 5069 - Pages: 21
...tKapitel 1, Grundstoffer og kemiske forbindelser 1.1 a) Ag nr 47, latin: argentum, Argentina b) Sc nr 21, scandium, Scandia, latin for Skandinavien Eu nr 63, europium, Europa Am nr 95,americium, de amerikanske kontinenter Yb nr 70, ytterbium, Ytterby i Sverige Hf nr 72, hafnium, Hafnia latin for København Cu nr 29, kobber, Cypern c) Cl nr 17, chlor, græsk: gulligt – grøn Br nr 35, brom, græsk: bromos = stank Cr nr 24, chrom = krom, græsk: chroma = farve P nr 15, phosphor = fosfor, græsk: phôs = lys phoros = bærende Os nr 76, osmium, græsk osme = en lugt Rb nr 37, rubidium, latin rubidus = mørkerød (rubiners røde farve) d) Cm nr 96, curium, Marie og Pierre Curie som fandt radium No nr 102, nobelium, Nobel institut i Sverige, Alfred Nobel som opfandt dynamit Es nr 99, einsteinium, Albert Einstein som udtænkte relativitetsteorien Md nr 101, mendelevium, Dmitrij Mendelejev som opstillede det periodiske system Bh nr 107, bohrium, Niels Bohr, atomets opbygning og kvantemekanik e) He nr 2, heliun, græsk Helios = Solen Np nr 93, neptunium, planeten Neptun Pu nr 94, plutonium, dværgplaneten Pluto Se nr 34, selen, græsk: Selene = Månen Te nr 52, tellur, latin: Tellus = Jorden U nr 92, uran, planeten Uranus 1.2 a) og b) Guld Au nr 79, aurum, latin: gul, glødende daggry (Sol) Sølv Ag nr 47, argentum, latin fra gammel græsk: hvidt, skinnende (Månen) Kviksølv Hg nr 80, hydragyron, græsk: vandsølv, flydende sølv, (Merkur) ...
Words: 5371 - Pages: 22
...Welcome to CH 125 Inorganic Chemistry for Microbiology Course Description This course covers inorganic reactions and phenomenon present in microbiological systems. The chemistry of the predominant biological elements of groups I to VII will be discussed. The students will explore the principles of inorganic chemical phenomenon including partially soluble substances, weak acids and bases, buffer systems and redox reactions. In addition, a basic understanding of the chemistry of the biologically important elements (H, C, N, O, K, Na, Ca, Mg, P, S, Cl and some transitional elements) will be explored. Course Learning Outcomes Upon successful completion, students will be able to: • Predict cation and anion concentrations of partially soluble solids dissolved in pure water and in a solution containing a common ion. • Apply knowledge of acids and bases in order to predict the pH of a solution containing a weak acid or base. • Demonstrate the use of common pH and redox indicators in microbiological media. • Select appropriate reagents to make a buffer having a desired pH. • Determine which compounds undergo the process of reduction and which undergo the process of oxidation. • Describe the basic chemistry of the predominant biologically important elements and their function(s) in microbiological systems. Dr. Andrew Baer Office Hours Monday: 10:30 am – 11:20 am Wednesday: 1:30 pm – 2:20 pm Thursday: 9:30 am – 10:20 am or by appointment Email:...
Words: 1551 - Pages: 7
...Chemistry 1B Experiment 16 77 16 Qualitative Analysis Introduction The purpose of qualitative analysis is to determine what substances are present in detectable amounts in a sample. This experiment has two parts. In the first part, you will analyze an unknown solution for the presence of seven common ions. In the second part, you will test an unknown solid to determine which of two possible identities is correct. Part I. Spot Tests for Some Common Ions A simple approach to the qualitative analysis of an unknown solution is to test for the presence of each possible ion by adding a reagent which will cause the ion, if it is in the sample, to react in a characteristic way. This method involves a series of “spot” tests, one for each ion, carried out on separate samples of the unknown solution. The difficulty with this way of doing qualitative analysis is that frequently, particularly in complex mixtures, one species may interfere with the analytical test for another. Although interferences are common, there are many ions which can be identified in mixtures by simple spot tests. In this experiment we will use spot tests for the analysis of a mixture which may contain the following commonly encountered ions in solution: CO32– SO42– PO43– SCN Cl – – carbonate sulfate phosphate thiocyanate chloride acetate ammonium C2H3O2– NH4+ 78 Chemistry 1B Experiment 16 The procedures we involve simple acid-base, precipitation, complex ion formation or oxidation-reduction...
Words: 4527 - Pages: 19
...The Commercial World of Energy Storage: A Review of Operating Facilities (under construction or planned) Septimus van der Linden Principal Brulin Associates 1st Annual Conference of the Energy Storage Council March 3, 2003 Houston, TX AGENDA • INTRODUCTION • TECHNOLOGIES • PROJECTS • FUTURE DEVELOPMENTS • CONCLUSIONS Motivation for Electrical Energy Storage Price of Electricity Power Generation Energy Storage Time - Make Use of Volatile Electricity Prices - INTRODUCTION • Electricity! 3rd Largest Business in the USA $300 billion/per annum. • Demand for Electricity is seldom constant over time. • Excess generation during low demand periods - can be stored. • Stored Energy can provide Electricity during high demand. • Help reduce power system loads. • Improve Efficiency and Reliability. • Make better use of efficient Baseload generation. • Allow use of Renewable Energy technologies. TECHNOLOGIES • • • • Batteries Compressed Air Energy Storage (CAES) Flywheels Pumped Hydro Storage Two Main Categories: • Bulk Energy Storage – CAES-PHS • Distributed Energy Storage – Batteries-Flywheels-Other (capacitors) PROJECTS • OPERATING • UNDER CONSTRUCTION • PLANNED PROJECTS OPERATING • Bulk Energy Storage • PHS (Pumped Hydro) - First introduced circa 1904 in Swiss Alps. – 100,000 MW Europe, Asia & Latin America. – 21,000 MW Japan. – 18,900 MW in USA. (Installed 1970-1990) • CAES (Compressed Air Energy Storage) – Two Highly Successful...
Words: 1830 - Pages: 8
...Oxidation-reduction reactions (or redox) reactions, are a type of reaction in aqueous solutions that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an e-. They occur every day and are vital to some of the basic functions of life. Some examples include photosynthesis (within plants), respiration (within animals), combustion, and corrosion or rusting. To understand these types of reactions, you must first understand oxidation numbers or states. Rules for Assigning Oxidation States The oxidation number corresponds to the number of electrons, e-, that an atom loses, gains, or appears to use when joining with other atoms in compounds. When determining the Oxidation State of an atom there are seven guidelines to follow: 1. The Oxidation State of an individual atom is 0. 2. The total Oxidation State of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge. 3. Group 1 metals have an Oxidation State of +1 and group 2 an Oxidation State of +2 4. The Oxidation State of fluorine is -1, when in compounds 5. Hydrogen generally has an Oxidation State of +1 in compounds 6. Oxygen generally has an Oxidation State of -2 in compounds 7. In binary metal compounds, group 17 elements have an Oxidation State of -1, group 16 of -2, and group 15 of -3. (Note: The sum of the oxidation states is equal...
Words: 2601 - Pages: 11
...Unit 7 Unit 8 Study Guide 1. Which of the following statements is incorrect? A) Ionic bonding results from the transfer of electrons from one atom to another. B) Dipole moments result from the unequal distribution of electrons in a molecule. C) The electrons in a polar bond are found nearer to the more electronegative element. D) A molecule with very polar bonds can be nonpolar. E) Linear molecules cannot have a net dipole moment. 2. Atoms having greatly differing electronegativities are expected to form: A) no bonds B) polar covalent bonds C) nonpolar covalent bonds D) ionic bonds E) covalent bonds 3. Choose the compound with the most ionic bond. A) LiCl B) KF C) NaCl D) LiF E) KCl 4. Atoms with very similar electronegativity values are expected to form A) no bonds. B) covalent bonds. C) triple bonds. D) ionic bonds. E) none of these 5. Which of the following bonds is least polar? A) C—O B) H—C C) S—Cl D) Br—Br E) They are all nonpolar. 6. For the elements Rb, F, and O, the order of increasing electronegativity is: A) Rb < F < O B) Rb < O < F C) O < F < Rb D) F < Rb < O E) None of these 7. For the elements Cs, F, and Cl, the order of increasing electronegativity is: A) F < Cl < Cs B) Cs < Cl < F C) Cl < Cs < F D) F < Cs...
Words: 3943 - Pages: 16
...------------------------------------------------- Reagent index[edit] A[edit] Chemical name | Chemical formula | Common name | Source and description | Acetic acid | CH3COOH + H2O | 5% Solution: White vinegar | Grocery store; "white vinegar"—5% or "cleaning vinegar"—10%Photography supply store; "Indicator Stop Bath"—89% (with Bromocresol Purple dye) or "Glacial Acetic Acid" 99.5–100% | Acetone | CH3COCH3 | Acetone | General; "nail polish remover"Discount store; Onyx, Cutex. Boating supply; "fiberglass cleaner" Hardware store; "Acetone"While composition varies from product to product, paint removers have more acetone per volume than regular nail polish remover, and industrial grade (rather than consumer grade) paint removers used by professionals + sold in bulk will contain more acetone still. Some stores sell pure acetone as well.[2] | Acetylene gas | C2H2 | Ethyne | Hardware store or Welding supply; "acetylene"By reaction of calcium carbide and water. | Acetylsalicylic acid | C9H8O4 | Aspirin | Pharmacy; "Aspirin" | Aluminium | Al | Aluminium | General; "aluminium foil"Fine art store; "metallic pigment"—powdered aluminiumFiberglass supply shop; powdered aluminium as a filler material.Refined from mined aluminum ore, or bauxite.Often coated with wax to reduce flammability. | Aluminium hydroxide | Al(OH)3 | alumina hydrate | General; "antacid tablets"—blended with magnesium hydroxideAntacid Tablets; Alu-cap, Amphojel, Dialume—100%Fine art supply: "thickening agent"...
Words: 6510 - Pages: 27