Martin Deng 19/02/2012 11 Chemistry E T13P 8.2-5.3.1 perform a first-hand investigation to compare the properties of some common elements in their elemental state with the properties of the compound(s) of these elements (eg magnesium and oxygen) Chem.p1.53 Dot. pt.Pre.Chem. p 34 T13P: Comparison of properties in elemental and compound state T13P: Comparison of properties in elemental and compound state Introduction: The idea of this practical experiment is to understand properties of common elements in their elemental state and in their compound state. The processes that are to be used in this experiment are synthesis, oxidation and combustion. It also involves the changing of elements into a compound.
The supplies included: a pencil, a printout of the table of reactions, a toothpick, a sheet of white paper, a sheet of black paper, a paper towel, distilled water, a small amount of household cleaners (such as: Windex, vinegar, and stainless steel/granite cleaner), the goggles from LabPaq, 24-well plate, 96-well plate, a empty short stem pipet, and the bag labeled for the experiment from LabPaq that included: aqueous ammonia, bromethylmol blue, Copper (II) Sulfate, FDC blue dye #1, hydrochloric acid, lead (II) nitrate, phenolphthalein solution, potassium iodide, silver nitrate, sodium bicarbonate, sodium hydroxide, sodium hypochlorite, and starch solution 1% stabilized. The 24-well plate was used to hold the pipets of chemicals going to be used. The end of each of the pipets was cut off to allow use. Next, the table of reactions was labeled with the perspective well that would be used for each chemical reaction listed. The first chemical reaction was in well A-1, two drops of NaHCO3 (sodium bicarbonate) was added to the well followed by two drops of HCl (hydrochloric acid).
This is provable by the reaction that occurred with the two gases hydrogen and oxygen. Oxygen is found in the air, and the hydrogen was trapped by placing a test tube over the reacting test tube. When the mixture of the two gases was heated with the flaming wood splint, a reaction producing H2O occurred, and in the process released heat and light. Part C Was one of the products of this reaction a precipitate? How could you tell?
An Investigation to determine the reaction kinetics of the Iodine-Propanone reaction The Aim for this investigation to use the reaction between Iodine and Propanone, with an acid catalyst, to determine the reaction kinetics of each of the reactants and find out which order each of the reactants is and to develop a rate equation. This will be done by changing the concentrations of the reactants and reacting them in a colorimeter and measuring the colour change over time by measuring the percentage of light absorbed over a constant period of time. Equation- CH3COCH3(aq) + I2(aq) → CH3COCH2I(aq) + H+(aq) + I-(aq) Source- http://www.chemtopics.com/unit09/iodina.pdf This is a substitution reaction because a Hydrogen atom gets substituted for an Iodine atom. The role of the acid catalyst is to speed up the otherwise slow rate of reaction. Nuc: + R-LG → R-Nuc + LG: The electron pair (:) from the nucleophile (Nuc) attacks the substrate (R-LG) forming a new bond, while the leaving group (LG) departs with an electron pair.
Rate of Evaporation and Intermolecular Forces Laboratory Report General Chemistry Laboratory Bernard Determining the Rate of Evaporation and Intermolecular Forces. Introduction Evaporations occur when a liquid absorbs energy and changes to gas. The evaporation process occurs only at the surface of a liquid compared to the boiling process in which liquid also changes to gas at the bottom of the liquid where the additional heat source is located. Two types of organic compounds were encountered in this experiment- alkanes and alcohols. Alkanes composed of only carbon and hydrogen atoms are referred to as hydrocarbons.
* 100% key lime * 50% key lime * 25% key lime 3. This is the formula to produce different key lime concentrations. * M1V1 = M2V2 Preparing of Kirby-Bauer test Materials and apparatus * Broth cultures of P. anvenginosa, E coli, S. aurens and B. spizizenii * Sterile cotton swab * Forceps * Bunsen burner * Whatman filter paper (small piece after punch) * Key lime discs * Parafilm Procedure 1. Swirl the contents of the broth culture of P. anvenginosa until it is equally murky throughout. 2.
Section 3: The titration of an unknown concentration of HCl with the standard solution of NaOH. Section 4: Use the HCl solution titrate a commercial basic product and determine the quantity of active ingredient. -Section1: Preparation of a Standard Sodium Hydroxide Solution Materials 250-mL volumetric flask Weigh scale Weighing bottle, or watch glass for NaOH sample, Glass funnel Dropper pipette 100 ml beaker Deionized water NaOH solid Procedure 1. Weigh approximately 1 gram of NaOH in a weighing bottle. Record the actual mass (1.01 grams weighed) in the results table.
The Empirical Formula of an Oxide, Purpose: The purpose of this lab was to determine the empirical formula of magnesium oxide. To do this, we measured the weight of the magnesium before the reaction with oxygen, and then measure it after it had bonded with the oxygen. After the mass of the items were collected, the data was calculated in empirical formula. Background: The empirical formula of a compound is the whole number ratio of the elements in a compound. For example, the empirical formula of water is H2O meaning for every 1 O atom there are 2 H atoms.
The gases being observed in this lab are hydrogen (H2), oxygen (O2), and carbon dioxide (CO2). These gases will be generated while carrying processes that adhere to the following reactions: Hydrogen (H2) Mg + 2HCl ( MgCl2 + H2 or Zn + 2HCl ( ZnCl2 + H2 Oxygen (O2) 2H2O2 (Catalyst MnO2) (2H2O + O2 Carbon Dioxide (CO2) NaHCO5 + 2HCl ( NaCl + H2O + CO2 Materials Used: Materials provided by the student – Matches, toothpicks, tin foil pie tin, permanent fine tip marker, white vinegar, 3% Hydrogen peroxide, measuring spoons, drinking straw, tissue paper, Sodium bicarbonate Material from Labpaq – Safety googles, 5 – test tube in bubble pack, Well plate – 24, gas assembly (stopper with copper/plastic tubing), pipet – empty and short stem, 2 Alka Seltzer tablets, 4ml of 0.04% Bromothymol Blue in pipet,20ml of 2M Hydrochloric Acid in dropper bottle, 6ml of Limewater (Saturated Calcium Hydroxide) in pipet, 5 pieces of Manganese Metal, 3 wide-neck pipet bulbs, 5 pieces of mossy Zinc Procedure and Experiment Observations: |Data Table 1: Experiment Results | |Gas |Flame Reaction |Glowing Splint |Limewater
(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.