Iron ore: processes and History
Iron ore: processes and History Intro An ore also is a mixture of one or more minerals. We distinguish ore from rock in that a valuable and/or useful material can be mined or extracted from the ore. This material often is a metal. Iron ore, is mined for its iron content. Mining companies sell the ore to manufacturers who extract the iron and use it in producing iron and steel products. The portion of the ore that is not iron is considered a waste or by-product. Even though it is considered a waste of the iron process, the by-product may be useful in some other process. Firstly, iron is quite magnetic. Ores can be located by magnetic sensing akin to backyard metal detectors, and possibly even harvested, unoxidised iron at least, with simple electromagnets. Underground mining is achieved by sinking shafts to the appropriate levels and then driving horizontal tunnels, called adits, to reach the ore. Underground mining is, however, relatively expensive and is generally limited to rich ores. Iron compounds are used as a colourant in glasses, which look to have a tremendous importance in lunar construction, manufacturing, and export. Process: Over-view Smelting is a way of getting metals from the rocks in which they exist in their natural form. These rocks are often known as ores. These ores are heated to a high temperature in an oven or a kiln, so that the metal in them
An experiment to find the heat energy in different alcohols.
An experiment to find the heat energy in different alcohols. In this experiment I will be burning 6 different alcohols to heat up a beaker of water. I will be burning 6 alcohols, methanol, ethanol, propanol, butanol, pentanol and hexonal. The aim is to find out how much energy is produced when burning these 6 different alcohols. Water and carbon dioxide is formed when the alcohol reacts with oxygen in the air. The heat energy is given out when forming the bonds between the new water and carbon dioxide molecules. The specific heat capacity is the number of joules required to heat one gram of water by 1°C. I decided to choose water because it is safe and easily found. I will also need to ensure that I conduct the experiments safely. As these alcohols are very dangerous and highly flammable I will wear my safety goggles at all times. I will need to keep all lose items off clothing tucked in e.g. my tie tucked in to shirt. The lids on the alcohols must be kept on at all times to prevent evaporation of the alcohol or any spillage's. Apparatus · Beaker · Thermometer · Measuring cylinder · Weight scales · Gauze · Tripod . 6 different alcohols . Wood block . Heat mat . Matches The method that I will use is as follows: · Measure 100ml of water into a beaker. · Record the
Fuel cell technology.
INTRODUCTION A fuel cell by definition is an electric cell, which unlike storage cells can be continuously fed with the fuel so that the electrical power output is sustained indefinitely. It converts the hydrogen or hydrogen containing fuels directly into electrical energy plus heat through the electrochemical reaction of a hydrogen and oxygen into water. Fuel cells are one of the cleanest and most efficient technologies for generating electricity. A fuel cell produces electricity by means of an electrochemical reaction much like a battery. But there is an important difference. Rather than extracting the chemical reactants from the plates inside the cells, a fuel cell uses hydrogen fuel and oxygen extracted from the air to produce electricity. Unlike a battery, however, fuel cells never lose their charge. As long as there is a constant source of fuel - usually natural gas for the hydrogen and air for the oxygen - fuel cells will generate electricity. Since there is no combustion, there are none of the pollutants commonly produced by boilers and furnaces. For systems designed to consume hydrogen directly, the only products are electricity, water and heat. Fuel Cell Origins: In 1839, Sir William Grove, a British physicist, first discovered the principle of the fuel cell. Grove utilized four large cells, each containing hydrogen and oxygen, to produce electric power which
Find out the difference in energy that is given out by the alcohols Methanol, Ethanol, Propanol and Butanol when they are burned under a tin of water for 3 minutes.
Robbie Morgan Alcohols Coursework Aim: The aim of this work is to find out the difference in energy that is given out by the alcohols Methanol, Ethanol, Propanol and Butanol when they are burned under a tin of water for 3 minutes. Plan: The first thing I need to do is to collect and correctly set up the apparatus. Here is a diagram of how I plan to do this: Here is the list of apparatus I am going to use: Stand, boss and clamp Spirit burner Metal can Thermometer Electronic scales Heat proof mat Matches I am going to use four different spirit burners each with a different alcohol in it. I am going to choose ones that look as if they have roughly the same amount of fuel in them to make the test fairer. I am using a metal can because it conducts heat better than a glass beaker and therefore it will give me a more accurate result. I will measure the temperature of the water to the nearest 0.5 of a degree because this is the smallest I can accurately measure with my naked eye on the thermometer available to me. I will use a stop clock to time 3 minutes for each experiment and I will also use the same amount of water each time (120 ml). In my preliminary work I discovered that 120 ml is the best amount because if you have less than that the water boils and if you have more it doesn't get hot enough to record a difference between the alcohols in the 3 minutes. In order
Science Coursework:Methanol & Ethanol
Aim: To observe temperature change in ethanol and methanol and predict which of the two fuels has the highest temperature while burning for 10mins. Introduction: I'm going to burn methanol and ethanol to find out which one of the fuels will have the highest temperature. Methanol and Ethanol are both types of alcohols. Methanol is a clear colourless liquid which is made from fossil fuels and natural gases. Ethanol is made from grains and is renewable. Prediction: I think methanol will have a higher temperature than ethanol because Fair test: The test was fair because the amount of water and temperature for both experiments were the same. The height of the flame was also the same and we timed each experiment for 10 minutes. We used the same equipment for both experiment. Safety: To make the experiment safe we tied back long hair, put on our goggles and cleared the space in front of us. Equipment: The equipment we used were: beehive stands, tripod, gauze mat, timer, thermometer, beaker, goggles and heat proof mat Method: 50ml of water at room temperature was poured into the beaker. The beaker was placed on a tripod which was on a gauze mat. The fuel was then lit and we used a thermometer to measure the temperature every minute. The experiment was repeated three times. Both fuels were used. We recorded the data in two tables; one for ethanol and another for methanol. We
To compare the given values of the molar heat of combustion
AIM: The aims of my experiment are to compare the given values of the molar heat of combustion with my experimental values, and to predict the theoretical value of heptanol. PREDICTION: I predict that my experimental values will be lower than the given values. This is because heat will be lost in unnecessarily obtaining the results. This will be by sound and light energy given off, incomplete combustion (complete combustion occurs when there are lots of oxygen atoms available when the fuel burns, and then you get carbon dioxide, as a carbon atom bonds with two oxygen atoms; a limited supply of oxygen results in carbon monoxide being produced), and also conduction, convection and radiation of heat through the air, and draughts speeding the process up. Water will be evaporated, meaning that there is a lower volume of water, causing the remaining water to absorb more heat energy, which will affect the results. To combat this, I will stir the water with the mercury thermometer immediately after the experiment, thus spreading the heat energy around the water. The beaker will also be heated, diverting some of the heat energy away from the water. I also predict that the heavier one mole of the alcohol is, the greater the molar heat of combustion will be. This is because the heavier the mole, the more bonds there are, and the more heat energy is required to break them, resulting in
Do larger molecules produce more heat?
Do larger molecules produce more heat? The first four members of the alcohols - OH (hydroxyl) group have been used for heating. They are: methanol, ethanol, propanol and butanol, respectively. Each member of the series has an extra HCH than the member before it. The aim of the experiment was to test the statement: "Do larger molecules produce more heat?" My hypothesis is that alcohols with larger molecules will produce more heat. The following equipment was set up to carry out the experiment: tin beaker, thermometer, matches, ring clamp, retort stand, electronic scale, ruler, 100ml measuring cylinder and methanol, ethanol, propanol and butanol burners. Method: . Use the measuring cylinder to measure 100ml of water and pour it into the metal beaker. 2. Place the thermometer into the beaker and record the temperature. 3. Weigh and record the weight of the methanol burner (with cap on). 4. Attach the ring clamp (with beaker) onto the retort stand. 5. Place the burner directly beneath the beaker. 6. Light the burner. 7. Adjust the ring clamp so that the distance between the flame and the base of the beaker is 3cm. 8. Heat the water until its temperature rises by about 30°C. 9. Put the cap back on the burner to extinguish the flame. 0. Weigh the alcohol burner again with the cap on, and record the result. 1. Repeat the experiment with the other 3
Investigating the combustion of varying alcohols.
Investigating the combustion of varying alcohols Aim To find the different rates for the combustion of alcohol. The aim is to find out how much energy is produced when burning these alcohols. Prediction As the alcohol burns, the temperature of the water will increase and the weight of the alcohol will decrease. This is due to evaporation that takes place because of the heat. Alcohols react with oxygen in the air to form water and carbon dioxide. The reaction that is involved in burning alcohols is exothermic because heat is given out. From this reason the reactant energy is higher than that of the product. I predict that the more bonds there are holding the carbon, oxygen and hydrogen atoms together; more energy will be required to break them apart. For example Ethanol has the formula C H OH. In this formula you have five C-H bonds, one C-C bond, one C-O bond and one O-H bond. To separate these types of bonds you require a certain amount of energy. Type of Bond Energy Required (joules) C-H 410 C-O 360 O-H 510 C-C 350 O=O 496 C=O 740 To separate C-H bond you need to apply 410 joules of energy. There are five such bonds in ethanol so you multiply 410 by five to get 2050 joules. You do these calculations for all the other types of bonds that make up ethanol, add them all together and you get 3270 joules. All of the other alcohols can be broken up in this
Aircraft power plant
Aircraft power plant Introduction For this assignment I have been asked to design my own aircraft power plant, which is a sub or super sonic jet engine. I will include all the individual components that are incorporated in the system, stating reasons why I have selected them. I will also state which fuel tanks I would use where they will be placed and why I have place them there, how they are constructed and any protective treatments that I may choose to apply. I will be describing the type of fuel that will be used in the system and why it will be used. Work plan Monday Start assignment in rough Complete by Tuesday Completed Monday Tuesday Check assignment and start to word process Complete by Wednesday Completed Monday Wednesday Finish word processing check and print Complete by Friday Completed Monday Intake Compressor Combustion Turbine Exhaust = High pressure air = Hot gases Dave Janney Page 1 5/2/2007 Description of components Supersonic convergent / divergent (intake) - allows the correct amount of air to enter the compressor. Designed similar to a venturi tube. The throat is designed not to let air in at speeds above mach 1 even when the aircraft is travelling at speeds well above mach 1. If this type of intake was not used and air was allowed to enter the intake at speeds above mach1 the compressor becomes overloaded and
To find out which of these four alcohols: ethanol butanol propanol pentanol is the best fuel to use and also which, uses the least amount of fuel to boil a certain amount of water.
CHEMISTRY COURSEWORK GCSE Different Fuels Investigation: To investigate different alcohols. Aim: To find out which of these four alcohols: 1-ethanol 1-butanol 1-propanol 1-pentanol is the best fuel to use and also which, uses the least amount of fuel to boil a certain amount of water. Background: I looked through books and encyclopaedias to find out more about these alcohols, so that I can base my prediction on this. I found out that: ) Propanol: - is an isomeric alcohol which means it is an isomer which means that propanol can be made up of 2 or more compounds but having the same molecular formula but different structural formula. Propanol is also a by-product of the synthesis of methanol from carbon monoxide and hydrogen. Its molecular formula is CH3 CH2 CH2OH or in simple terms C3H7OH. Propanol is a colourless, flammable, fragrant liquid and it is also fairly toxic. 2) Pentanol: - is an organic compound, its molecular formula is CH5H11OH. The term is commonly applied to mixtures and compounds, which are used as solvents for resins and oily materials. It is a colourless liquid, slightly soluble in water and it has a penetrating odour. 3) Butanol: - is an organic compound, its molecular structure is very similar to the other alcohols, its molecular structure is C4H9OH. Butanol is a solvent for lacquers, resins, abd other coatings and components of hydraulic break
