Exp 21 Reactivities of Some ALkyl Halides Summary: * The reactivities of several substrate types will be examined under both SN1 and SN2 reaction conditions in this experiment. * Sodium Iodide or Potassium Iodide in Acetone: A reagent composed of sodium iodide or potassium iodide dissolved in acetone is useful in classifying alkyl halides according to their reactivity in an SN2 reaction. * Silver Nitrate in Ethanol: A reagent composed of silver nitrate dissolved in ethanol is useful in classifying alkyl halides according to their reactivity in an SN1 reaction. Procedure: * Part A. Sodium Iodide in Acetone: * The Experiment: * Label ten test tubes from1 to 10.
Experiment#2 “Separating the Components of a Ternary Mixture” By Mohammad Bazargan Lab partners: Aaron Radtke, Kevin Campbell, Austin Gilchrist Instructor: Professor Mundell Section #: 12 Sep/14/2011 Abstract In this laboratory, we used physical and chemical properties to separate the components of a ternary (three substances) mixture. We also determine the percentage of each substance in the mixture. The percentages are the following,38.2% NaCl, 40.45% SiO2, and 72.84% CaCO3.The mentioned substances were all separated using methods such as filtration, evaporation and reaction with other chemicals which will be explained throughout this report. Intro Mixtures are \ physical combinations of two or more substances where each substance keeps its own chemical identity. Mixtures can be classified as either homogeneous or heterogeneous.
½ mark 10 Outline the reaction pathway to produce propanoic acid from propane. Write the chemical reactions (using chemical structures) indicating reactants and any special conditions. 2 marks 11 Name all the chemical species in Q10 using the IUPAC system. 1 mark 12 If you put the product formed in Q10 in a basic solution, what would the resulting ion look like? 1 mark 13a Indicate the chemical equation when your product from question 10 undergoes a
* Exercises on page 156 – 160 (4.19; 4.23; 4.37; 4.39; 4.49; 4.61; 4.68 ( Answers: a 7.18 g; b 0.0756 M); c 439 ml). Problems solved in class on Acid-Base-Titrations. Page 166 – 168; page 170 – 183; page 188 – 192; Page 212 – 215; page 234; page 235; page 237 – 243 (lanthanides and actinides excluded); page 259 – 270; page 276 – 279 * Energy, work, and heat calculations. Calorimetry. Exothermic and endothermic reactions.
Aim: To determine the presence of the cations Na+, K+, NH4+, Ag+, Cu2+ and Bi3+ in the solution under analysis. Procedure: Please refer to page 26-27 of CHM152/154/2252 Laboratory Manual. Results: Procedure No and Ion Test Reagent or Technique Evidence of Chemical Change Chemical(s) Responsible for Observation Equation(s) for Observed Reaction 1. Na+ Perform flame test by dipping a test loop in test solution and putting in Bunsen flame after cleaning the loop with HCl(aq) A brilliant yellow persistent flame occurs Presence of sodium in the test solution - 2. K+ Perform flame test by dipping a test loop in test solution and putting in Bunsen flame after cleaning the loop with HCl(aq).
Chem 112 Assignment for Chapter 19 1. Calculate ΔS° values for the following reactions by using tabulated S° values from Appendix B (Petrucci text) a) N2H4 (g) + H2 (g) → 2NH3 (g) b) 2Al (s) + 3 Cl2 (g) → 2 AlCl3 (s) c) Mg(OH)2 (s) + 2 HCl (g) → MgCl2 (s) + 2 H2O (l) d) 2 CH4 (g) → C2H6 (g) + H2 (g) 2. Use data in your Appendix B to find ΔH° and ΔS° values at 25°C to calculate ΔG° where ΔG° = ΔH° - T ΔS° for each of the following reactions. a) Ni (s) + Cl2 (g) → NiCl2 (s) b) CaCO3 (s, calcite) → CaO (s) + CO2 (g) c) P4O10 (s) + 6 H2O (l) → 4 H3PO4 (aq) d) 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l) Note: the following values ΔHf° (kJ/mol) S° (J/K) Ni (s) 0 29.9 NiCl2
Title: Experiment 1: Qualitative Analysis of Common Anions Aims To qualitatively analysis common anions of SO42- , PO43-, CO32-, S2-, I-, Br-, Cl- and NO3-. Procedure Please refer to laboratory manual page 14 to 22. Results Procedure Number and Ion | Test Reagent or Technique | Evidence of Chemical Change | Chemical(s) Responsible for Observation | Equation(s) for Observed Reaction | * | Addition of NH3 Addition of Ba(NO3)2 | White precipitate | BaSO4(s), BaCO3(s), Ba3(PO4)2(s) | SO42-(aq) + Ba(NO3)2(aq) BaSO4(s)CO32-(aq) + Ba(NO3)2(aq) BaCO3(s)3(PO4)3-(aq) + 3Ba(NO3)2(aq) Ba3(PO4)2(s) | * | Separation of SO42-, PO43- & CO32- by centrifugation. | Colourless solution and white precipitate | BaSO4(s), BaCO3(s), Ba3(PO4)2(s) | - | * SO42- | Addition of HNO3Centrifugation | Colourless solution and white precipitate | BaSO4(s) | Ba2+(aq) + SO42-(aq) BaSO4(aq) | * PO43- | Addition of (NH4)6Mo7O24 Put in warm water | Yellow precipitate | (NH4)3PO4(MoO4)12(s) | Ba3(PO4)2(s) + 2H+(aq) 3Ba2+(aq) + 2HPO42- (aq)HPO42-(aq) + 12(NH4)2MoO4(aq) + 23H+(aq) (NH4)3PO4(MoO4)12(s) + 21NH4+(aq) + 12H2O(l) | * CO32- | Centrifuge mixtureAddition of HNO3Immediately insert a stirring rod | White precipitate | CaCO3(s) | CO3 2-(aq) + 2H+(aq) H2O(l) + CO2(g) CO3 2-(aq) + 2OH-(aq) CO3 2-(aq) + H2O(l)CO3 2-(aq) + Ca2+(aq) CaCO3(s) | * S2- | Addition of HNO3Addition of Cu(NO3)2Centrifugation | White precipitate and green solution | CuS (s) | Cu2+ (aq) + S2- (aq) CuS (s) | * I- | Addition of Fe(NO3)3Addition of toluene | Formation of purple layer | I2(toluene) | 2Fe3+ (aq) + 2I- (aq) 2Fe2+(aq) + I2(toluene) | * Br- | Addition of tolueneAddition of HNO3Addition of KMnO4 | Formation of brown layer | 5Br2(toluene) | 2MnO4- (aq) +10Br-(aq) +16H+(aq) 2Mn2+ (aq) + 5Br2(toluene) + 8H2O(l) | * Cl- | Addition of AgNO3 |
Chemistry Lab Report 1 Experiment 1: Qualitative Analysis of Common Anions Aim: To separate and identify the presence of the anions SO42-, PO43-, CO32-, Cl-, Br-, I-, S2-, NO3-. Procedure: Please refer to the lab manual from page 18 to 20. Results: Procedure Number and Ion Test Reagent or Technique Evidence of Chemical Change Chemical(s) Responsible for Observation Equation(s) for Observed Reaction ① NH3, Ba(NO3)2 White precipitate BaSO4 Ba2+(aq) + SO42-(aq) → BaSO4(s) Ba3(PO4)2 3BA2+(aq) + 2(PO4)3-(aq) → Ba3(PO4)2(s) BaCO3 Ba2+(aq) + CO32-(aq) → BaCO3(s) ② Centrifuge Transparent (supernatant) BaS Ba2+(aq) + S2-(aq) → BaS(aq) BaI2 Ba2+(aq) + 2I-(aq) → BaI2(aq) BaBr2 Ba2+(aq) + 2Br-(aq) → BaBr2(aq) BaCl2 Ba2+(aq) + 2Cl-(aq) → BaCl2(aq) ③ SO42- HNO3, Centrifuge White precipitate (does not dissolve) BaSO4 Ba2+(aq) + SO42-(aq) → BaSO4(s) ④ PO43- (NH4)6Mo7O24 Yellow Precipitate formed (NH4)3PO4(MoO3)12 3Ba2+(aq) + 2(PO4)3-(aq) → Ba3(PO4)2(s) Ba3(PO4)2(s) + 2H+(aq) → 3Ba2+(aq) + 2HPO42-(aq) HPO42-(aq) + 12(NH4)2MoO4(aq) + 23H+(aq) → (NH4)3PO4(MoO3)12(s) + 21NH4+(aq) + 12H2O(l) ⑤CO32- HNO3, Ca(OH)2 No milky solution CaCO3 CO32-(aq) + 2H+(aq) → H2O(l) + CO2(g) CO2(g) + 2OH-(aq) → CO32-(aq) + H2O(l) CO32-(aq) + H2O(l) + Ca2+(aq) → CaCO3(s) ⑥ S2- HNO3, Cu(NO3)2 Green solution, Grey precipitate CuS Cu2+(aq) + S2-(aq) → CuS(s) ⑦ I- Fe(NO3)2, toluene Purple layer formed I2 2Fe3+(aq) + 2I-(aq) → 2Fe2+(aq) + I2(toluene) ⑧Br- HNO3, KMnO4 Brown bromine gas formed Br2 2MnO4-(aq) + 10Br-(aq) + 16H+(aq) → 2Mn2+(aq) + 5Br2(toluene) + 8H2O(l) ⑨ Cl- AgNO3 White precipitate formed AgCl Ag+(aq) + Cl-(aq) → AgCl(s) ⑩ NH3 Pricipitae dissolved AgCl dissolves AgCl(s) + 2NH3(aq) ⇋ [Ag(NH3)2]+(aq) + Cl-(aq) ⑪ NaOH, Ag2SO4, centrifuge Black precipitate formed Insoluble salt such as AgBr or AgI which will
Name: Razlan bin Mohamed Fitri Partner's Name: Vinod MenonExperiment 1: Qualitative Analysis of Common AnionsAim: To investigate the qualitative analysis of common anions.Procedure: Refer to lab manual page 18-20.Results: Procedure Number and Ion | Test Reagent or Technique | Evidence of Chemical Change | Chemical(s) Responsible for Observation | Equation(s) for Observed Reaction | 1) | Addition of 6M NH3 and 0.3M Ba(NO3)2 | Whole solution is precipitated | Ammonia,NH3 and Barium Nitrate, Ba(NO3)2 | | 2) | Centrifuging | Only precipitate left | | | 3) SO4 ²ˉ | Addition of 6M HNO3 and centrifuging | White precipitate undisolved | Barium sulphate, BaSO4 and Nitric acid, HNO3 | | 4) PO4 ³ˉ | Addition of 0.2M (NH4)6Mo7O24 and heating | Yellow precipitate is formed | Barium phosphate, Ba3(PO4) and Ammonium heptamolybdate, (NH4)6Mo7O24 | | 5) CO3 ²ˉ | Repeat Part A and addition of 6M HNO3 and insertion of stirring rod dipped in saturated Ca(OH)2 | Milky solution seen | Barium carbonate, BaCO3 and Calcium hydroxide, Ca(OH)2 | | 6) S ²ˉ | Addition of 6M HNO3 and 1M Cu(NO3)2 and centrifuging | Blackish green precipitate formed | Nitric acid, HNO3 and Copper (II) nitrate, Cu(NO3)2 | | 7) I ˉ | Addition of 0.2M Fe(NO3)2 and toluene | Purple color seen in toluene layer | Iron (III) nitrate, Fe(NO3)2 and toluene | | 8) Br ˉ | Addition of 6M HNO3 and 0.1M KMnO4 | Brown bromine seen in the toluene layer | Nitric acid, HNO3 and Potassium permanganate, KMnO4 | | 9) Cl ˉ | Addition of 0.01M AgNO3 | White precipitate formed | Silver nitrate, AgNO3 | | 10) | Addition of 6M NH3 | White precipitate dissolves at first, then turns black( which
Methodology A survey was employed to find out the attitude towards chemistry and its prediction on achievement in chemistry. The attitude was measured using two scales of measurement namely Likert and Guttman. The selected topics in chemistry were periodic table (PT); chemical bonding (CB) and organic chemistry (OC).