• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

To determine the value of Faraday constant (quantity of electricity per mole) by using electrolysis of Copper.

Extracts from this document...


1) Title: QN1 A Quantitative study of electrolysis 2) Aim/Objective: To determine the value of Faraday constant (quantity of electricity per mole) by using electrolysis of Copper. 3) Results: Before electrolysis: Weight of cathode = 2.164 g Weight of anode = 2.502 g After electrolysis: Weight of cathode = 2.237 g Weight of anode = 2.435 g Time of electrolysis = 20 minutes = 1200 seconds Ammeter reading = 0.19A 4) Calculation/interpretation: The equation of the electrolysis reaction at the cathode: Cu2+(aq.) + 2e- � Cu(s.) Gain in weight of cathode = 2.237g - 2.164g = 0.073 g Loss in weight of anode = 2.520 - 2.435g = 0.085 g No. of moles of loss in cupper anode = 0.085 / 63.5 = 0.00134 mol Quantity of electricity required = 0.00134 mol * 2 = 0.00268 mol Quantity of electricity supplied = 1200 * 0.19 = 228C Faraday Constant = quantity of electricity / no. ...read more.


ions might not be very soluble at that moment. After that, the copper electrodes were rinsed with propanone and heated under a Bunsen flame. Since propanone can remove grease or oil, this treatment could leash off the sebum which we have left on the electrodes when transferring them. Of course, when rinsing them by propanone, a pairs of forceps was used. After rinsing, the copper electrodes were warmed high on a Bunsen flame to evaporate propanone more quickly. However, they should be placed high above the Bunsen flame because propanone is flammable and a Bunsen flame can oxidize the copper plate, forming copper (II) oxide on their surface, which will finally lead to a heavier weight and smaller Faraday Constant. The value of the Faraday Constant was calculated to be smaller than the literature one (96500 Cmol-1) due to a number of errors. For instance, it was inevitable that the electricity supply was not exactly 0.19A in the time interval 20 minutes. ...read more.


This can explain why the gain in weight of the cathode and the loss in weight in the anode were not the same. So if the gain in weight of the cathode was taken into consideration, the calculated value of the Faraday Constant would be larger. After finding out the value of the Faraday Constant, the thickness of the metal plating can also be calculated. According to the formulae Density = Mass / Volume and Volume = Thickness * Surface Area, since the density of copper (8920kgm3), the surface area, the mass of copper formed are all known, the thickness of the plating can be known. It is actually calculated by: Mass / Density / Surface area. Such electrolysis process performed in this experiment is useful in electro-plating. It can plate a certain object by placing it on the cathode, and the metal to be plated onto the object will be put on the anode. 6) Conclusion: The Faraday constant was calculated to be 161000 C mol-1. ?? ?? ?? ?? Yu Wing Yee 6A(30) - 1 - ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Changing Materials - The Earth and its Atmosphere section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Changing Materials - The Earth and its Atmosphere essays

  1. The Electrolysis Of Copper (ii) Sulphate Solution Using Copper Electrodes

    - 2electrons --> Cu2+ (aq) 193000C 64g So; 193000C deposits 64g 300Y Coulombs deposits 64 x 300Y / 193000 =19200Y / 193000 = Y x 19200 / 193000 With a current of 0.35A: Mass deposited = 0.35 x 19200 / 193000 = 0.0348g With a current of 0.60A: Mass deposited

  2. Investigate the factors that affect the mass of Copper deposited on the Copper Cathode ...

    During the experiment the current seemed to be fluctuating quite frequently, especially when using higher currents and although most times the current was adjusted back to its previous amount using the ammeter as soon as possible, at times the experiment was left unattended for a minute or two and the current could have fluctuated then.

  1. An experiment to show how electroplating using copper electrodes.

    The method and the equation I have mentioned early on in background knowledge can calculate the actual mass change. The prediction I have predicted has come out to be exactly the same as the experiments, which is that the change in mass will be proportional to the change in current.

  2. Investigating how the amount of copper affects the mass of the cathode

    The rheostat allowed me to choose the size of the current of my choice and also stay at the same position throughout the experiment. I also decided to change the size of the current that was applied and start it from at least 0.5 amps because previously I noticed that

  1. Investigating one of the factors that affects the mass of copper deposited when copper ...

    Each electron that goes round the circuit has a tiny charge. A current of 1 ampere flowing for 1 second carries a charge of 1 coulomb. To find the charge of any current we can use the formula: charge = current x time.

  2. The Electrolysis Of Copper Sulphate Solution Using Copper Electrodes

    For the 0.40A reading, the anode difference is 0.07A, a much greater difference, and the cathode variation was smaller, at 0.02A. The 0.60A anode difference was only 0.01A, and the cathode was the same. The 0.80A anode and cathode variation were also 0.01A.

  1. Investigation into Electrolysis

    solution onto the cathode, variables will affect the amount of plated metal produced. Variables including the reactivity of the metal involved, the concentration of the solution and the surface area of the metal in contact with solution affect the amount of plated metal.

  2. Electrolytic wastewater treatment apparatus

    electrolytic oxidation cell that incorporates stainless steel electrodes, and wherein the stability and lifetime of the anode are enhanced by incorporation of metal chips. [0003] 2. Description of the Related Art [0004] Industrial wastewater streams may be contaminated by various substances that render their discharge into waterways or municipal waste treatment systems problematic or illegal.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work