Are humans to blame for Global warming or is it a natural phenomenon?

Contents page . Introduction (page 3) 2. Scientific background (page 4-5) 3. Arguments for global warming being caused by humanity (page 6) 4. Arguments for global warming being caused natural phenomenon (page 7) 5. Conclusion (page 8) 6. Bibliography (page 9) Introduction The question I have chosen to answer is 'Are humans to blame for Global warming or is it a natural phenomenon?' I have chosen this question because this question raises numerous arguments that need to be addressed and solved. Global warming is a matter that is featured in my everyday life such as newspapers, books, news, etc. the main issue is the debate on whether global warming is man-made or the cause of a natural phenomenon such as the sunspot theory. In this case study I will be assessing and evaluating the evidence which I have collected in order for me to find out the true cause of the worldwide epidemic that is global warming. Research that I have done shows that global temperatures are trending upwards. So can assume that global warming is in effect however we have yet to find a definite decision as to who is the cause of global warming. Many people may argue that global warming is an idea theorised by 'tree-huggers' but reports have shown evidence that may shed some light on what global-warming actually is and the so-called 'greenhouse effect' The illustration above shows the

  • Word count: 2095
  • Level: GCSE
  • Subject: Science
Access this essay

Importance of electrolysis in our daily lives

Importance of electrolysis in our daily lives INTRODUCTION In 1800, two Englishmen, William Nicholson and Anthony Carlisle, used an electric current to decompose water into its element, hydrogen and oxygen. This is an example of electrolysis. Electrolysis is the process of using electricity to break down or decompose a compound. It has a few main components - a battery, electrodes and an electrolyte. There are many applications of electrolysis. Electroplating is one of the main areas where electrolysis is implemented. ELECTROPLATING It is the coating of one metal over the other which is called electroplating. It is done for few reasons to benefit us: . Resistance to corrosion and increased life span 2. Provision of insulation 3. Better appearance for e.g. chrome, nickel or silver can produce a mirror like finish Resistance to corrosion and increased life span: A coat of one less valuable metal on a more valuable metal can be very beneficial. For example if zinc is electroplated on iron then it would protect iron from getting corroded and would ensure proper usage. Provision of insulation: Insulating materials can be electroplated for safety of living organisms. Plastic for example can be electroplated on copper or aluminum for protection from shocks. Better appearance: this one of the most common method used for everyday life coating. Electroplating of silver,

  • Word count: 2082
  • Level: GCSE
  • Subject: Science
Access this essay

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

  • Ranking:
  • Word count: 388
  • Level: GCSE
  • Subject: Science
Access this essay

Using Simple cells to find an order of reactivity in metals

Using Simple cells to find an order of reactivity in metals In electrochemical cells a chemical reaction occurs in the "cell" causing an electrical current to be generated. The electrochemical cell is made by dipping two metals into a solution which allows electricity to pass through it. In this experiment a solution containing ammonium chloride is used. The Aim The aim of this science assessed practice is to use my data to confirm the position of the metals in the reactivity series. Apparatus Voltmeter 2 leads with crocodile clips Beaker (approximately 100cm3) Emery paper Ammonium chloride solution Strips of the following metals: Zinc Copper Magnesium Lead Tin Aluminium Nickel Procedure . Clean the metals with emery paper. 2. Half fill the beaker with ammonium chloride solution. 3. Connect two wires to the voltmeter. 4. Using crocodile clips connect a piece of one metal to wire and a different metal to the other wire. 5. Dip the two pieces of metal into the solution and record the HIGHEST reading given in the table 1. 6. Repeat steps 1-5 testing all the metals as indicated in the results table 1 (N.B. If the voltmeter reads a negative value make a note of the sign.) DIAGRAM OF APPARATUS Fair Test I measured the voltage and sign the positive or negative value in order to find the reactivity series. The only variable in this practice is the type of

  • Word count: 1236
  • Level: GCSE
  • Subject: Science
Access this essay

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

  • Ranking:
  • Word count: 2125
  • Level: GCSE
  • Subject: Science
Access this essay

Life's Essential Elements: Chlorine & Iodine.

Life's Essential Elements: Chlorine & Iodine Chlorine and iodine, both halogens, have important uses in everyday life particularly in industries. Their uses are described on pages 6-8. Both these elements had been discovered around 200 years ago and have been used ever since however methods of obtaining these elements have changed throughout the years. Extracting Chlorine Several processes can be used to obtain chlorine the main one being electrolysis of sodium chloride solution known as brine, a method used by chlor-alkali industries. Electrolysis can be achieved using three types of electrolytic cells namely the diaphragm cell, mercury cell and membrane cell. `The main difference in these technologies lies in the manner by which the chlorine gas and the sodium hydroxide are prevented from mixing with each other.'^(1) [image002.jpg] [image004.jpg] [image006.jpg] In diaphragm cells brine flows through the separator (made of asbestos/polymer modified asbestos composite) to the cathode compartment. In membrane cells the separator is an ion exchange membrane however mercury cells contain no diaphragm or membrane, instead the mercury itself acts as a separator. All modern cells use anodes made of titanium coated with `an electrocatalytic layer of mixed oxides' and are known as DSAs (dimensionally stable anodes) however the cathode material varies for each.

  • Word count: 1202
  • Level: GCSE
  • Subject: Science
Access this essay

Investigate the factors that affect the mass of Copper deposited on the Copper Cathode during the Electrolysis of Copper (11) Sulphate Solution using Copper Electrodes.

An Experiment to investigate the factors that affect the mass of Copper deposited on the Copper Cathode during the Electrolysis of Copper (11) Sulphate Solution using Copper Electrodes Background Information Electrolysis is the decomposition of a molten or aqueous compound by electricity. Electrolysis occurs only in liquids called electrolytes. Electrolytes are compounds, which conduct electricity when molten or dissolved in water, but not when they are in a solid state as the oppositely charged ions are held together by strong ionic bonds in a giant lattice and this means electricity cannot pass through it and the ions are unable to move. If electrolytes are molten or dissolved in water their ions are free to move, and the movement of ions in liquids is key in electrolysis. Electrolysis takes place in an electrolyte cell. The diagram below shows the apparatus used in the electrolysis of molten or aqueous ionic compounds. The electrodes (anode and cathode) are known as conducting rods. Normally they are made out of platinum or graphite as these substances are chemically unreactive and will not interfere with the experiment. They are inert electrodes. However in this experiment we are using copper electrodes. Copper electrodes are active electrodes and these metal electrodes take part in electrolysis. Copper electrodes are used in industry to obtain pure copper. The

  • Word count: 5567
  • Level: GCSE
  • Subject: Science
Access this essay

What Affects The Rate of Electrolysis Of Copper Chloride Solution?

What Affects The Rate of Electrolysis Of Copper Chloride Solution? Introduction We are going to find out what things affect the rate of Electrolysis and to find this out we will use Copper chloride salt dissolved in water to form a solution. The salt is dissolved in water because chemical compounds when in a molten state or when dissolved in water exist in the form of ions that are capable of movement, meaning their molecules become dissociated into positively and negatively charged components, which have the property of conducting an electric current. A compound that conducts when molten or in solution is called an electrolyte. When some substances dissolve they change slightly, their atoms are no longer neutral, neither positive nor negative. The negative atoms lose their electrons so the atoms become positive. These particles are no longer known as atoms but ions. The positive ions are called anode. The negative ions are called cathode. These electrons only dissolve in water. Because they have enough room to move this then lets the reaction take place. Equation CuCl2 Cu+2 + 2Cl-1 If a pair of electrodes is placed in a solution and a source of direct current is connected between them, the positive ions in the solution move towards the negative electrode (cathode), and the negative ions move towards the positive electrode (anode). On reaching the electrodes, the ions

  • Word count: 1355
  • Level: GCSE
  • Subject: Science
Access this essay

Investigating displacement reactions to find out the order of reactivity of some metals.

Aim Investigating displacement reactions to find out the order of reactivity of some metals. I will find this out by comparing temperature rise caused by different metals during displacement reactions in a salt solution. Prediction I predict that the reactivity series for these three metals (Zinc, Magnesium, Iron) will look like this: Magnesium Zinc Iron I also think the following: Magnesium will have the most vigorous reaction and the temperature change for this metal will be the most. Zinc will have a vigorous reaction with the solution but it will not be as vigorous as the reaction Magnesium will have. Iron will have the least vigorous reaction, as it is closest to Copper in the reactivity series (when compared with Zinc and Magnesium). Therefore the displacement reaction will occur between Iron and the Copper Sulphate solution but it will not be as significant as the displacement reaction Zinc and Magnesium will have with the Copper Sulphate solution. I believe that the most energy will be released by Magnesium. Magnesium as you can see by the use of the reactivity series is above the other metals I am investigating (Zinc and Iron), meaning it has the ability to loose it's electrons most easily and displace the copper from the solution and make it a pure metal. The equation for this will be: Mg + CuSO4 MgSO4 + Cu I also believe that the reactions

  • Word count: 2819
  • Level: GCSE
  • Subject: Science
Access this essay

Effect of increasing charge on mass of copper deposited during electrolysis.

Effect of increasing charge on mass of copper deposited during electrolysis Aim: It is known that by passing a constant electric current through an aqueous copper sulphate solution that the passage of ions through this solution results in copper atoms being dissolved into the solution from the anode while positive copper ions (cations) are being discharged at the cathode. The experiment I will carry out is aimed to monitor the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. Plan Diagram Method My apparatus for this experiment will be: * A Power Pack * 2 Copper electrodes * An ammeter * Wire, with clips * A beaker I will pour the Copper Sulphate solution into a small beaker. I will then weigh the electrodes and record their masses. I will then place the electrodes into the beaker containing Copper Sulphate solution. I will then connect the electrodes to the power pack and the ammeter. A steady current will be made (3 Amps) and the experiment will be stopped at definite times (i.e. 5,10,15,20,25 minutes). At these times the current will be switched off and both electrodes will be removed from the solution. They will then be dried by dipping into propanone (a highly volatile liquid which readily evaporates) Variables The factors that my effect the

  • Word count: 918
  • Level: GCSE
  • Subject: Science
Access this essay