Verification Of Faradays First Law Of Electrolysis

Verification Of Faradays First Law Of Electrolysis My research question How can Beers law be used to verify Faradays First law of electrolysis and to determine Avogadros number and Faradays constant by electrolysis of 1.000 mol dm-3 copper sulfate (CuSO4) solution using graphite electrodes? is an indirect question to the investigation. I was always interested in verifying laws and learning about interdependence between laws. I was so keen in finding how that how the nature of one law depends upon another law as chemistry a whole subject depends upon multiple concepts. So I took this opportunity to show how one law can be proved using another law. Here in my research I have shown how Beers law can be used to verify Faradays First law of electrolysis and I have also used Beers law to determine Avogadros number. This research clearly indicates that there is interdependency between laws. In the verification of Faradays First law of electrolysis of CuSO4, we generally focus on mass of Cu deposited, but not much on color. My focus was that how to use this phenomenon / property of change in intensity to calculate mass indirectly. The same concept of absorbance in Beers law applies while determining Avogadros number. I did the experiments to verify Faradays First law of electrolysis and to determine Avogadros number in indirect manner. Indirect methods have often helped scientists to get their results better and we also have good examples for Back titration and chromatography. So with the same expectation in mind, I came with such a topic for my research. Slight modification in the experiments can really help. I did use graphite electrodes because they are cheap, it is therefore widely used in electrolysis rather than platinum as it is costly. The disadvantage for graphite electrodes is, it flakes off and therefore mass readings of Cu deposited over graphite electrode are highly unreliable. So as the result is highly unreliable, we might not get the accurate readings of the mass of Cu deposited at cathode. But if we use the colorimeter technique to find out the deposition, the mass of graphite lose in the electrolysis process is not affected. I mainly focused upon the absorbance value by the diff erence of color. Once while performing an experiment on electrolysis during my school days, I was using graphite electrodes and I noticed that graphite particles were flaking off the electrodes in electrolyte solution during the experiment. The amounts of carbon particles lost from graphite were very less and so was neglected but later I thought that it might be affecting the result in some or the other way as in the experiment we were supposed to weigh the electrodes to find out the amount of Copper deposited on the cathode. I used to think that if graphite electrodes are themselves losing some mass, then how the electrode can give accurate readings or a reliable result. The copper deposit over cathode is not strongly attached to the cathode thus there are chances that copper deposited on cathode may be lost by mishandling of the electrode before taking direct mass reading; this made me think about an alternative method which would be more accurate as well as reliable, where in the electrodes will n ot have to be removed from the experimental set-up at all! 2. THEORY I would like to start by mention something about electromagnetic spectrum as my experiment deals with Beers law which can be obtained through absorbance value. Absorbance in the colorimeter is found by setting a particular wavelength and there is different wavelength for different objects, similarly there is a particular wavelength absorbed by CuSO4. Electromagnetic radiations have frequencies and all the possible frequencies are covered in the range known as electromagnetic spectrum. The property of characteristic distribution of electromagnetic radiation emitted or absorbed by any specific object is the electromagnetic spectrum of that object. Electromagnetic spectrum has its range from low frequencies which are used for modern radio to the high frequency like gamma radiation. It covers wavelength from thousand kilometers to small fraction. The limit for the long wavelength is the universe itself and shortest wavelength is near to the Plank length even if the principal states the s pectrum is infinite and continuous which is truly acceptable. In the Vernier colorimeter we have option to select the wavelength from range 430nm, 470nm, 565nm and 635nm. According to the user guide for Vernier colorimeter CuSO4 will yield a good Beers law curve at 635nm. Therefore it says that the wavelength absorbed by CuSO4 lies in the range 635nm and I had used 635nm range throughout the experiment for finding the absorbance of CuSO4. In the study of light we have the Beer-Lambert law which is also known as Beers law and the law is related to the absorption of light to the properties of the material from which the light passes. Electrolysis is a process to separate bonded elements and compounds .The methodology followed is by passing an electric current through bonded elements and compounds. Electric current is passed through a conductor called as electrode. Electrodes are found in various forms like wires, plates, and rods. Electrodes are mainly constructed of metal, such as copper, silver, lead, or zinc. Electrodes can also be made up of nonmetal substance, such as carbon. There are commonly used Graphite electrodes which are made up of carbon. In my experiments as I have used graphite electrodes, I am indirectly using nonmetal substance having carbon. Inert electrodes do not take part in the chemical reactions for Examples, Graphite and Platinum electrodes. Active electrodes take part in chemical reactions where the anode itself produces metal ions which get discharged at the cathode for Example, Copper electrodes. I noticed that graphite rod was losing carbon particles on stirring, thats the reason why direct method to find mass of copper deposited was not adopted by me. The electrodes which I used for the experiments were Inert electrodes and I used graphite electrodes because platinum electrodes were not available and they were costly. An electrode passes current between a metallic part and a nonmetallic part of an electrical circuit. Most frequently, conductors that are metallic carry electrical current. In other circuits, however, current is passed through a nonmetallic conductor. In an electrochemical cell, an electrode is called either an anode or a cathode. An anode is an electrode at which current leaves the cell and oxidation takes place. For example, an anode is the positive electrode in a storage battery. Faradays 1st Law of Electrolysis states that, The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electricity transferred at that electrode. Quantity of electricity refers to the quantity of electrical charge, typically measured in coulomb. Throughout the investigation I had rounded off few of the readings to get correct significant figures. Using a colorimeter: This method is only useful if one of the reactants or products is coloured. It is a more satisfactory method than titration for two reasons: firstly, no sampling is needed, and secondly, a reading can be taken almost instantaneously. So quite rapid reactions can be followed, especially if the colorimeter is interfaced to a data logger or computer which can plot a graph of concentration versus time as the reaction proceeds. A colorimeter consists of a light source with filters to select a suitable colour (i.e. set of wavelengths) of light which is absorbed by the sample. The light passes through the sample onto a detector whose output goes to a meter or a recording device. The colorimeter usually needs to be calibrated and even I calibrated the Vernier colorimeter with distilled water before conducting the experiments. Calibration is done to establish the relationship between its readings and the concentration of the copper sulfate used. 3. INVESTIGATION My investigation was divided into three main sections, starting with verification of Faradays First law of electrolysis, secondly to determine Avogadros number and finally in determining Faradays constant. I had predicted that the results of investigating Faradays First law by direct method and indirect method will give almost the same result and I was successful in getting that. But according to my assumptions, more accurate readings can be obtained by the indirect method of colorimeter using Beers law technique. It is also useful to determine Avogadros number and Faradays Constant as the result which I got through the Beers law technique was almost near to the true value of Avogadros number and Faradays constant. 3.1 APPARATUS AND MATERIALS Beakers (250 cm3 ÃÆ'- 1) Volumetric flask (100 cm3 ÃÆ'- 5 and 1000 cm3 ÃÆ'- 1) Measuring Cylinder (100 cm3 ÃÆ'- 1) Digital Weighing Balance Graphite electrodes Copper sulfate (CuSO4) Ammeter (0-500mA) Rheostat (0-500 à ¢Ã¢â‚¬Å¾Ã‚ ¦) DC variable voltage source (0 12 V) Vernier labquest colorimeter Cuvette 3.2 CIRCUIT DIAGRAM OF EXPERIMENTAL SET UP The above shown diagram represents the electric circuit diagram of the entire experimental setup. A DC variable voltage source (0-12 V) was used as a battery. Rheostat was use to control the current coming from the battery because I was recording the Ammeter readings and I wanted the readings on the Ammeter to be constant throughout the experiment. I used Rheostat because the Ammeter reading was fluctuating and not remaining constant. The positive terminal of the battery was connected to the one end of Rheostat and the negative terminal of the battery was connected to the cathode. The connections were made in series as it was suppose to be for this experiment. The experimental set up was not disturbed during the electrolysis. During the investigation, there goes a chemical reaction within the experimental setup for the electrolysis of copper sulfate. Below are shown the reactions using graphite anode inert electrode. At cathode: Cu2+ + 2e- à ¢Ã¢â‚¬  Ã¢â‚¬â„¢ Cu At anode: OH1- 1e- à ¢Ã¢â‚¬  Ã¢â‚¬â„¢ OH x 2 [2OH à ¢Ã¢â‚¬  Ã¢â‚¬â„¢ H2O + [O] ] 4OH à ¢Ã¢â‚¬  Ã¢â‚¬â„¢ 2H2O + O2 Product at anode: Oxygen gas 3.3 PREPARATION OF SOLUTION Preparation of 1 dm-3 of reagents: The salt which I used in preparation of solutions was Copper sulfate pentahydrate, we commonly call it as copper sulfate. The molar mass of CuSO4.5H2O is 249.68 gmol-1. Therefore, to prepare a 1.000 molar of CuSO4 solution, I took 124.84 g of CuSO4 weighing upon a digital balance and then I diluted 124.84 g of CuSO4 in 500cm3 of distilled water. I had used distilled water to dilute the chemicals and to clean the apparatus rather using tap water because distilled water is more pure and using tap water can affect the result as it can indirectly react with the chemicals used for the experiments. It was very difficult to dissolve CuSO4 by using glass rod. Therefore, I had used magnetic stirrer to dissolve the crystals of Copper sulfate in distilled water. It was very time consuming in dissolving CuSO4 in distilled water but within few minutes the 500cm3 solution of 1.000 molar of CuSO4 was ready. From that 500cm3 of 1.000 molar of CuSO4, I prepared different 100cm3 solutions of concentration 0.8 molar, 0.6 molar, 0.4 molar and 0.2 molar. The volumes of Copper sulfate and Water in the different molar solutions are given in the below table: Concentration ( ±0.001 mol dm-3) Volume of CuSO4 ( ± 0.05 cm3) Volume of H2O ( ± 0.05 cm3) 1.0 mol dm-3 100 cm3 00 cm3 0.8 mol dm-3 80 cm3 20 cm3 0.6 mol dm-3 60 cm3 40 cm3 0.4 mol dm-3 40 cm3 60 cm3 0.2 mol dm-3 20 cm3 80 cm3 3.4 VERIFICATION OF BEERS LAW Beer in 1852 studied the effect of absorption of light on the concentration of solutions and found a similar relationship. Beers law states that when a parallel beam of monochromatic light enters an absorbing medium, the rate of decrease of intensity of the light with concentration is directly proportional to the intensity of radiation. Alternative statements can be expressed thus: When a parallel beam of monochromatic light passes through an absorbing medium, the intensity of transmitted radiation decreases exponentially as the concentration of the absorbing species increases arithmetically. Successive layers of equal concentration and thickness absorb equal fraction of incidental radiation. The readings for my Beers law experiments are as follows: Concentration ( ±0.001mol dm-3) Transmittance (%T) Absorbance ( ±0.001) 0.0 100.04 0.000 0.2 25.92 0.586 0.4 8.17 1.088 0.6 3.02 1.520 0.8 1.33 1.875 1.0 0.97 2.015 The graph which was obtained for Beers law: The graph was taken from vernier colorimeter using logger pro software to get the accurate readings for the absorbance of CuSO4. Here I observed a curve in graph and I felt that this abnormal for Beers law but later when I searched the reason for this, I got satisfactory answer as I was not gone wrong. Beers law is true for dilute solutions and therefore it is sure to obtain a straight line graph for dilute solutions. In the cases of highly concentrated solutions we get a curve which flatters if extended further due to the high concentration. This is the same case with my Beers law graph because the solution of CuSO4 was much concentrated. Deviations from Beer Lamberts Law: According to Beer-Lamberts law, absorbance A is directly proportional to concentration c. Thus, a graph of Absorbance v/s concentration should give a straight line passing through the origin. Often we find that the graph is not linear, and deviations occur. If the straight line curves upwards or downwards it indicates positive or negative deviations respectively from Beer Lamberts law. Deviations from Beer-Lamberts law a : no deviation; law is valid b : positive deviation c : negative deviation I got negative deviation for my Beers law graph. Negative deviation is shown in the above graph with option c. The Negative deviation in the graph was expected as the CuSO4 solution was highly concentrated. Deviations fromBeer-Lamberts law can be of three types: Real deviations: which are fundamental in nature. Instrumental deviations: which arise as a consequence of the manner in which the absorbance measurement is made. Chemical deviations: which arise as a result of chemical changes associated with concentration changes. The deviation which I got in my Beers law graph was Real Deviations and such deviation occurs due to Effect of concentration. The Beer-Lamberts law is valid for dilute solutions only. If the concentration of the solution is more than 0.01 M, Beer-Lamberts law does not strictly hold well, and deviations occur. At higher concentration, the molecules of the absorbing species come closer to one another, and due to this, charge distribution of neighboring molecules is affected. This results in an alteration in the ability of the species to absorb a particular wavelength of radiation. The extent of interaction depends on the concentration of the solution and therefore deviations are observed in concentrated solutions. The molar absorptivity à Ã‚ · depends on the refractive index of the solution. If the solution is too concentrated it refractive index changes and thus à Ã‚ · changes. This causes deviations from Beer-Lamberts law. This effect is negligible in concentrations