The electrolysis of Sodium Sulfate (Na2SO4)
Electrolysis I. The electrolysis of Sodium Sulfate (Na2SO4) Data Collection The side of anode and cathode The color before electrolysis The changes during electrolysis Anode Colorless The color stays the same and there is bubble. Cathode Colorless The carbon produces purple color and there is bubble. Data analysis & Conclusion From the experiment, after the electrolysis of Na2SO4, the color of cathode side becomes purple and there is bubble. The same thing happens in the other side, which is anode, bubble is also formed. Reduction happens in cathode, whereas oxidation happens in anode. In cathode, hydrogen (H2) is formed and in anode, Oxygen (O2) is formed. The reaction is in the following: Cathode --> 2H2O + 2e- --> 2OH- + H2 Anode --> 2H2O --> 4H+ + O2 + 4e- In cathode, the product the reduction is OH-, which is base becomes purple after being added by phenolphthalein and in anode, the product of oxidation is H+ is acid. If acid is added by phenolphthalein, the solution will stay the same, which is colorless. In both sides, cathode and anode, there is bubble, which is produced by hydrogen. In conclusion, II. The electrolysis of Potassium Iodide (KI) Data collection The side of anode and cathode The changes during electrolysis The changes after adding phenolphthalein The changes after adding starch Anode The
To find out how current affects the rate of electrolysis
Electrolysis experiment. Aim: To find out how current affects the rate of electrolysis. Pre-test: Pre-test Apparatus: . Power Pack 2. Stop watch 3. 3 wires 4. Amp meter 5. A piece of Card 6. stop watch 7. Top pan balance Pre-test Method: . Check to see if all the apparatus work by forming a small circuit with a bulb 2. Collect apparatus and set them out like the diagram below. Ensure that the positive wire leads to the anode and the negative leads to the cathode. 3. Measure out 50 ml of copper sulphate 4. In to a small class beaker 5. Weigh cathode on top pan balance 6. Slide anode and cathode in to piece of card and place in electrolyte 7. Turn on the power pack 8. Time until two minutes 9. Weigh cathode make sure you do not scrape off any copper 0. Repeat three times 1. Repeat for each current Pre-test Findings: By doing this pre-test I have learnt that: * The analog amp meter is very unreliable it * To be very accurate I need to use a multi meter * To be careful not to scrape of copper when measuring weight * Make sure that the anode and the cathode do not touch during the experiment * Make sure wires and power packs are working before you start * To change the electrolyte after each experiment * To use a stop watch instead of a clock as it is more accurate * To use a variable resistor to get the exact current you need Research: There are
Suitability Test
Suitability Test Introduction My work is about a scenario where a building contractor that wishes to develop an area of land into new houses for families. The Environment Agency has been asked to check the land for contamination. My task is to decide which method of testing Ph values in soil is most suitable for an environmental scientist. The desirable characteristics should be: * Safe: So no one is harmed whilst using it. * Easy To Use: So its easier to carry out more than once * Accurate: So that the readings are reliable. * Light: So it is easy to carry around. * Portable: So that it is easy to transport around. * Durable: So it can last longer. * Small: So that it's easier to transport. * Cheap: So it saves money and is cost effective. * Energy Efficient: So it doesn't need a mains power supply. Evaluation RED= Poor ORANGE= Average GREEN= Good Cost Litmus U.I. Solution Soil Probe pH Probe About 3p £4.15 £6.95 £294.46 Accuracy Litmus U.I. Solution Soil Probe pH Probe Acid/Alkali 0.5 .0 0.01 Time for results Litmus U.I. Solution Soil Probe pH Probe 5 Minutes 5 Minutes Minute 5-10 Minutes Sensitivity Litmus U.I. Solution Soil Probe pH Probe Acid/Alkali -14 Full Range 4-7 Full Range - More Accurate Durability Litmus U.I. Solution Soil Probe pH Probe ***** *** **** **** Easy To Use Litmus U.I. Solution
The Age of the Earth
The Age of the Earth In 1654 it was calculated that the earth had formed on October 23, 4004 BC. James Ussher made this discovery from the Bible. Nowadays the age of the earth is determined to be at least 4.5 billion years old. People all over the world now disagree with Ussher's theory because of religious reasons and most Christians still believe that the Earth was created 4004BC. Almost all of our evidence towards the Earth's age comes from the examination of rocks. People who analyse new discoveries of fossils and meteorites can possibly lead us to knowing the age since we can examine carbon and radiocarbon dating. Fossils in sedimentary rocks and the weathering of most ancient craters prove to us that some of the eldest bits rocks date back to about 4.5 billion years old. There is evidence to prove that the earth had formed approximately 1 billion years ago by radiometric age dating of particular rocks, such as lead in uranium-rich minerals which had showed us that it was in excess of being a billion years old. However the oldest bits of minerals to be discovered are small crystals of zircon that was found at Jack Hills of Western Australia. The dating of these minerals were approximately 4.404 billion years old. The earth must have been as old as any formation on it and information such as this can easily be considered as proof of the earth's existence meaning that
Extraction Of Iron
Extraction Of Iron Iron, perhaps the most important element to all civilization is also one of earth's most abundant. Like the majority of metal ores, iron ores are not pure compounds. Rather, most iron ore compounds are polluted with sand, rock and silica. The process of extracting iron involves a number of steps. The first step to concentrate the iron ore and remove its contents of silica. To further remove any existing impurities, a complex process takes place in a blast furnace. The charge is where materials are placed into the blast furnace. These materials are: Ore, Limestone and Coke. A burst of hot, oxygen enriched air is blown into the air-blast nozzle located at the near bottom of the furnace. What follows are a number of oxidation and reduction type reactions which ultimately produce the metallic iron. One of these reactions is the coke being burnt. The heat generated by this reaction increases the bottom of the furnace to a temperature near 19000° C. This reaction is represented in a chemical equation: C(s) + O2(g) (r) CO2(g) + heat The carbon dioxide generated rises halfway up the furnace, where it reacts with the hotter coke. This causes the carbon dioxide to reduce into carbon monoxide. This reaction absorbs some heat and lowers the temperature of the upper part of the furnace to roughly 1300° C. CO2(g) + C(s) + heat (r) 2CO(g) This
Atmospheric pollutants in the lower atmosphere essay.
Atmospheric pollutants in the lower atmosphere The atmosphere becomes polluted by both natural processes and the activities of humans. Volcanoes can release toxic gases including sulfur dioxide. Lightning produces toxic nitrogen oxides and ozone. Let us examine some gases that pollute the lower atmosphere. Lower atmospheric pollutants often include particulates such as soot from forest fires and the exhaust from industry. Metal dusts and concrete dusts also are atmospheric pollutants, as are vapours from solvents used in industry and domestically. Carbon dioxide The concentration of carbon dioxide has shown a gradual increase during the twentieth century. The burning of fossil fuels such as coal and oil products has caused this gradual increase in carbon dioxide levels. This increase in carbon dioxide is one of the factors that scientists believe has added to global warming. This is sometimes referred to as the 'enhanced greenhouse effect'. Carbon dioxide absorbs infrared (IR) radiation that is re-radiated by the Earth's surface. This process is vital in ensuring that the Earth does not lose too much heat and become a cold, lifeless planet. Too much carbon dioxide, however, leads to higher heat retention with consequent changes to the abiotic and biotic environment. Carbon monoxide Carbon monoxide is a lower-atmospheric pollutant. Road traffic emissions account for up
How the concentration of brine affects the conduction of electricity.
Electrolysis Investigation Aim: How the concentration of brine affects the conduction of electricity Background Information: Electrolysis: Metals that are more reactive than carbon are extracted by electrolysis. Electrolysis is the break down of a substance by electricity. Electrolysis only occurs in when an ionic substance is molten or is in solution. A substance that can be electrolysed is called an electrolyte. Electrolytes are made up of ions. Electrolytes need to be molten or in solution, so that the ions present are free to move. Ionic compounds have high melting points, so it is often easier to electrolyse the solution of the ionic compound. When the electrodes are connected to a source of direct current one, called the cathode, becomes negatively (-) charged while the other, called the anode, becomes positively (+) charged. The positive ions in the electrolyte will move toward the cathode and the negatively charged ions toward the anode. This migration of ions through the electrolyte constitutes the electric current in that part of the circuit. The migration of electrons into the anode, through the wiring and an electric generator, and then back to the cathode constitutes the current in the external circuit. Concentration: The concentration of a mixture also effects the rate of reaction. An increase in concentration means there are more particles. More
How the Concentration of Sodium Thiosulphate affects the Rate of Reaction
Rate of Reaction Coursework By Bonnie Kingett Contents Aim....................................................................................................................2 Introduction.......................................................................................................2 Preliminary Plan................................................................................................2 Preliminary Results...........................................................................................3 Safety................................................................................................................4 Fair Test............................................................................................................4 Method..............................................................................................................5 Results..............................................................................................................5 Conclusion........................................................................................................7 Evaluation.........................................................................................................8 Aim: The aim of our investigation was to find out how the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid is affected by varying the
Notes on the uses of limestone and its products
Indirect Uses of Limestone: Lime: * Manufacture * Thermal decomposition is used. * When calcium carbonate is heated strongly, it slowly disassociates into calcium oxide and carbon dioxide. * This reaction takes place in a lime kiln. * It is a reversible direction depending on the pressure and temperature. CaCO3(s) --> CaO(s) + CO2(g) (reversible) * Uses of lime(CaO): * Used as a drying agent. * To manufacture soda glass(ny heating it with sdium carbonate) * Alos used to make slaked lime. (Ca(OH)2) Slaked lime(Calcium hydroxide) * Manufacture * Made by adding an equal amount of water to calcium oxide. * This reaction is carefully monitored. * Thius control is needed as it is a highly exothermic reaction. CaO(s) + H20(l) --> Ca(OH)2(s) * Uses * Cheap industrial alkali. * Used to reduce soil acidity * Used in the manufacture of white wash. * Used in glass manufacture and water purification. * Limestone, a weak soln. of slaked lime is used to test for carbon diocide gas. * Calcium Hydroxide is mixed with sand to give mortar. * When mixed with water, it forms a strongly bonded material, in order to hold the bricks. * To remove acidic flue gases such as so2, produced when sulphur compounds in fossil fuels burn; the removal of so2 from flue gases is called desulphurization. * Test fpr CO2 * Limewater turns milky in presence of
Aerosols in Atmosphere - Environmental and Economical Impact.
Eni Ballauri 9A Chemistry Aerosols in Atmosphere Environmental and Economical Impact We have heard that greenhouse gases, mainly carbon dioxide, are leading to global warming. But, another factor has been identified that affects Earth's atmosphere; aerosols. Aerosols are small particles or droplets in the atmosphere. Aerosol particles may be created by wind blowing over dusty regions, and also by the conversion into tiny particles of some of the gases emitted by plants and volcanoes. Some aerosols remain in air only a few days, so they don't have much time to travel away. But nevertheless, they affect our surrounding environment at the local and global levels. It is also recognised as a health problem, especially in regard to respiratory illness. Atmospheric aerosols influence climate. They reflect the sunlight back to space, in a way that provides the gradual cooling of planet Earth. A professor in CU-Boulder's Laboratory for Atmospheric and Space Physics, Toon, who has studied similar modification of clouds over the ocean and their effects, said that aerosol cloud may even cancel out greenhouse warming. During winter, in polar regions, polar stratospheric clouds form. This provides sites for chemical reactions to take place. These reactions can lead reaction of reactive chlorine, which destroys the ozone. Contrary, because of loosing the ozone layer, Earth will lose
