Identification of an unknown organic compound
Identification of an unknown organic compound Aims: The aim of the identification experiment is to use a variety of tests to ultimately go to one functional group to identify an unknown organic compound. It could be one of the following: * Alkenes * Primary alcohol * Tertiary alcohol * Aldehyde * Ketones * Carboxylic acid * Ester * Phenol I will take each of the supplied functional groups and talk about them generally and identify a test which will be most suitable to identify whether that functional group is present in the unknown organic compound we are provided with. If tests need to be taken to see if oxygen, carbon dioxide or hydrogen gas has been given off, we will do the following: * Hydrogen - is present if we light a splint and put it in the test tube and it goes out with a squeaky pop. * Oxygen - is present if we light a wooden splint and blow it out and put it in the test tube and it rekindles. * Carbon dioxide - is present if when bubbled through lime water- it goes cloudy. During the experiment I will wear safety goggles, gloves and a laboratory coat throughout the whole experiment as some substances may cause irritant to the skin and be dangerous if in contact with skin and eyes. I will use 8 tests in total to identify the identity of the unknown organic compound. Alkenes Alkenes are unsaturated hydrocarbons and contain at least one double C=C
acid tabs
Chemistry Coursework, An investigation into the factors affecting the rate of reaction of indigestions tablets with acid. Planning, To start the investigation my partner and I discussed what affected rates of reaction. We managed to come up with 4 ideas: Surface area 2 Temperature 3 Concentration 4 Mixing of the substances (stirring) We decided to do 2 different preliminary experiment so we could chose which a certain variable to investigate and see what equipment was necessary to provide us with an accurate set of data. Our first Preliminary experiment was testing what affect heat had on the rate of reaction. We planned a basic experiment, We took a heatproof mat and placed a Bunsen burner on it. 2 We then put a tripod directly above the Bunsen burner on which we placed a conical flask with a bung and delivery tube tightly attached on. 3 We fed the delivery tube into a bowl of water. 4 Then a measuring cylinder was filled up with water, (to the very top) it was then turned upside down with a hand over the open hole letting no water out. It was the placed under (hole first). 5 The delivery tube was then placed inside of measuring cylinder (to collect any gas given off). 6 A timer was needed to time how long the experiment took. 7 The Conical flask was then filled up with 100cm3 of acid; this was then heated to the desired temperature (of which there was
Preparation of a crystalline derivative.
Preparation of a crystalline derivative. . Place 0.5 cm3 (10 drops) of the unknown liquid. (If the substance is solid dissolve 0.5g in a minimum amount of methanol.) Add 5 cm3 of the 2,4-dinitrophenylhydrazine solution and stir. 2. If precipitation does not occur, carefully add 1 cm3 of dilute sulphuric acid. 3. Using suction filtration apparatus as shown in diagram1, filter the precipitate. 4. Stop suction, either by lifting the funnel or by disconnecting the tubing, and soak the precipitate in about 1 cm3 of methanol. (Do not turn off the tap as you may get a "suck back" of water.) 5. Resume suction and dry the crystals by drawing air through them for a few minutes. 6. Recrystallize the solid using the following procedures. a. Transfer the crystals to a 150 cm3 beaker in a water bath. b. Dissolve the crystals in the minimum amount of hot ethanol. c. When the crystals have dissolved, cool the solution in an ice- water mixture until crystals re-appear. d. Filter the crystals as before. If necessary, rinse the beaker with the filtrate to complete the transfer. Wash the crystals with a few drops of cold ethanol. e. Press the crystals between filter paper to dry them thoroughly. Leave crystal in warm air until they are fully dry. Determination of the melting point of the derivative. . take a melting-point tube and push the open end through a pile of the derivative
Exploring physical properties of water (that have biological significance).
Biology --> Water By: Tahira Jamani Date: September 8th 2004 Investigation: Exploring physical properties of water (that have biological significance) Task: Design, then execute, a lab protocol to investigate water properties Research question: Is water co-hesive/ ad-hesive? Hypothesis: If we test water's co-hesion and ad-hesion on various papers, it will vary. For example, if we place water on wax paper, it will not be absorbed and thus helps to prove that it is not very ad-hesive as it will stay in a ball and will easily roll off. Also, the water will be easily broken if we were to try separating it using a metal stick, and this will show weak co-hesive forces. However on the other hand, if we test toilet paper, the water will be absorbed more easily and thus helps to prove that it is more ad-hesive to the paper as it will not be able to roll off. Furthermore, the water will not be able to split, and this will show strong co-hesive forces. All in all, it can be said that the stronger the ad-hesion, the stronger the co-hesion, and vice versa. We are hoping to see the weight of all the various papers increase, which will indicate that they have absorbed water and thus imply that the ad-hesion is great. Variables: Controlled variables: * Temperature (23o) * Amount of water on each paper (2 droplets) * Amount of paper used (6x6 cm) * Amount of time
TEST FOR CARBOHYDRATES
Aim To investigate the presence of simple sugars, non-reducing sugars, starch, proteins and fats in the food substances. Introduction Foods contain basic units. To determine which molecules are present in food, we have devised various tests to detect whether there is sugar, starch, protein, or lipid. These tests rely on the specific chemical; properties of the compound being tested. Method To perform the test, the below materials were needed: Materials * 12 boiling tubes * Dropper * Beaker * Unknown liquids A,B and C * Benedict's solution (blue) * Hydrochloric acid * Iodine solution (brown) * Sodium hydroxide * Copper sulphate (blue) * Ethanol Each student pair received three unknown samples dissolved in a solution of water. The below tests were performed in addition to any other physical observations we could make such as: colour, odour, clear or opaque, texture etc. Our results were recorded in a data table. Benedict's test - for simple (reducing sugar): A small amount of each unknown liquids was taken in three separate boiling tubes. To each of them Benedict's solution was added. All three tubes were heated gently for 2 minutes in the waterbath. A colour change from blue to orange was searched and the result was noted in the table. Iodine test - for starch: A small amount of each unknown liquids was taken in three separate boiling tubes. To each of them
An investigation to find out the factors affecting the rate of reaction of Hydrochloric acid with Sodium Thiosulphate.
An investigation to find out the factors affecting the rate of reaction of Hydrochloric acid with Sodium Thiosulphate. Aim: I am going to discover how the concentration influences the rate of reaction of Hydrochloric acid and Sodium Thiosulphate. There are four factors that influences the rates of reaction, they are: > Concentration(for gases it is pressure) > Temperature > Surface Area(Size of particles) The rate of reaction is owed to the collision theory. For a reaction to take place, particles must collide with great strength. If they do not collide with great strength, the reaction will not take place. Consequently, the rate of reaction is dependant on the collision of the particles. Method: . Set up the apparatus. 2. On a piece of paper, draw a dark cross. 3. Put 25ml of Sodium Thiosulphate. This is known as 1 Mole. 4. Place the beaker on top of the piece of paper, with the cross marked on it. 5. Check the temperature using a thermometer. 6. Add the Hydrochloric Acid to the Sodium Thiosulphate. As soon as the Hydrochloric acid touches the Sodium Thiosulphate start the time, using the stopwatch to see how long it takes until the cross is no longer visible. 7. Repeat this, however this time use 25ml of Sodium Thiosulphate and 5ml of water. 8. Keep repeating this; however change the concentration to 0.6M, 0.4M and 0.5M. 9. Repeat these processes three
Investigate the enthalpy values for the reaction between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride.
Investigate the enthalpy values for the reaction between Calcium Carbonate and Calcium Oxide with Hydrogen Chloride. H3 CaCO3 (s) CaO (s) + CO2 H1 HCl H2 HCl CaCl2 (aq) Results Variables of CaCO3 Mass of CaCO3 + weighing bottle 3.302 g Mass of empty weighing bottle 0.831 g Mass of CaC03 used 2.471 g Temperature of acid initially 8 C Temperature of solution after mixing 21 C Temperature change during reaction 3 C Variables of Temperature Mass of CaO + weighing bottle 2.362 g Mass of empty weighing bottle 0.936 g Mass of CaO used .426 g Temperature of acid initially 7 C Temperature of solution after mixing 27 C Temperature change during reaction 0 C Calculations * Heat Capacity x Temperature Change x Volume 1000 * Mass of Reactant Moles Ar * H1 for the reaction between CaCO3 + HCl 4.2 x 3 x 50 630_ 0.63 1000 1000 2.471 0.025 Ca ? 40 x 1 = 40 100 C ? 12 x 1 = 12 O ? 16 x 3 = 48 = 100 0.63_ 25.2 0.025 H1 = ?25.2 Kj mol H2 for the reaction between CaO + HCl 4.2 x 10 50 1890 2.1 1000 1000 .426 0.025 Ca ? 40 x 1 = 40 56 O ? 16 x 1 = 16 ? = 56 2.1 _ 84 0.025 H2 = ?84 Kj mol Due to the fact that I am using Hess' Law in
Investigating the Concentration of Hydrochloric Acid on the Rate of Reaction.
Chemistry Coursework Investigating the Concentration of Hydrochloric Acid on the Rate of Reaction In this coursework I am going to investigate the rate of reaction and how this is increased or decreased by the concentration of acid I will use. My aim in this experiment is to find the concentration of acid which will produce the fastest reaction. When carrying out my experiment I will use the following equipment: measuring cylinder conical flask clamp stand plastic beaker thistle funnel ice-cream tub The chemical reaction which occurs in this experiment will be: Calcium + Hydrochloric Calcium + Water + Carbon Carbonate Acid Chloride Dioxide CaCo (s) + 2HCl (aq) CaCl (aq) + H O + CO I will perform several experiments using the previous apparatus to see which concentration of hydrochloric acid will yield the most carbon dioxide. Apparatus Set Up Method To carry out my experiment I will set up my apparatus as I have previously shown. I will also need: * Three measuring cylinders - a large on which is to be used in the experiment and two smaller ones to measure the acid and water in. * 5 grams of Calcium Carbonate - measured out using a top pan balance. Firstly I will set up the above apparatus and
To plan an experiment to investigate the effect of concentration on the initial rate of reaction between Calcium Carbonate and Hydrochloric Acid.
AIM: To plan an experiment to investigate the effect of concentration on the initial rate of reaction between Calcium Carbonate and Hydrochloric Acid. Carbonate + Acid --> Chemical Salt + Water + Carbon Dioxide Calcium Carbonate + Hydrochloric Acid --> Calcium Chloride + Water + Carbon Dioxide CaCO3(s) + 2HCl(aq) --> CaCl2(aq) + H2O(l) + CO2(g) reactants products Rate of reaction is how much reactant (i.e. marble chips) is converted to product per unit of time. We can't work out the rate of reaction from a chemical equation. Equations can only tell us how much product we can get. They don't say how quickly it is made. We can only find the rate by actually doing experiments. During a reaction we can measure how much reactant is used up in a certain time. On the other hand, we can also measure how much product is formed in a certain time. In order to investigate this I am going to do several experiments in which I vary the concentration of the Hydrochloric acid. Each experiment I do will last 2 minutes and I will take readings every 10 seconds. I shall use the data I collect to make graphs to enable me to compare and evaluate my data fully. I will then attempt to link my results with the statement that: as we increase the concentration, the rate of reaction increases. To do this I will make an educated evaluation using both the theory I have learnt in the
An Investigation to Explore Rates of Reaction
GCSE Chemistry Coursework An Investigation to Explore Rates of Reaction Daisy Roberts Background information: The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a chemical reaction. If the reactants take only a short time to change into the products, that reaction is a fast reaction and the speed or the rate of the reaction is high. If a reaction takes a long time to changing the reactants into the products, it is a slow reaction and the speed or rate of that reaction is slow. The minimum energy needed for a reaction to occur is called the activation energy. The kinetic theory: The kinetic theory of matter states that matter is made up of small particles that are constantly in motion. The higher the temperature the faster they move. In a solid, the particles are closer together and attract one and other strongly. In a liquid the particles are further apart with weaker forces of attraction, and in gases there is almost no force of attraction between particles. Each of these states have different factors that would increase a reaction. The collision theory: The collision theory states that particles have to collide hard enough with each other in order to react. The rate of reaction simply depends on how often and how hard the reacting particles collide with each other. Factors affecting the rate of reaction: According
