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

Electrochemical Cell

Extracts from this document...

Introduction

IB Chemistry HL Yr. 2 Ms. Rachel 28th Feb, 10 Introduction To investigate the effect of change in temperature of the solutions on the voltage of an electrochemical cell. How does increase in temperature of the electrolytes in en electrochemical cell affect the voltage? An electrochemical cell produces electrical energy from chemical energy, where the chemical energy comes from the reactions in the cell. An electrochemical cell consists of two half-cells. Each half-cell consists of an electrode, and an electrolyte (salt solution). A salt bridge is used that connects the two solutions in the containers to allow flow of ions so there is no charge build up in either solution. Charge build-up would shift the equilibrium and the reaction would cease. When the two half cells, consisting of a metal electrode and a conducting solution are connected with an external wire, the strongest oxidizing agent will undergo a reduction in one half cell and the strongest reducing agent will undergo an oxidation in the other half cell. ...read more.

Middle

Materials required * Copper strip, 6cm x 1cm * Zinc strip, 6cm x 1cm * CuSO4 solution, 0.99M � 0.01M * ZnSO4 solution, 0.99M � 0.01M * KNO3 solution, 1.99M � 0.01M * Distilled water, 300mL � 1mL * Beakers (3), 250mL � 50mL * Graduated cylinder (100mL � 1mL) * Digital Voltmeter with crocodile wires * Hot plate * Thermometers (2), � 1�C * Paper strips, 10cm x 1cm * Magnetic stirrer * Rubber gloves * Apron * Safety Goggles Method Method to prepare solutions 1. Concentration required (CuSO4): 0.99M AMU of CuSO4: 159.61 So, 1.00M of CuSO4 has 159.61g of CuSO4 Hence 0.99M has: 159.61 x 0.99 = 158.01g � 0.01g Mix 158.01g � 0.01g of CuSO4 in 100mL of distilled water. Use a magnetic stirrer if necessary ==> Use 100mL � 1mL of 0.99M � 0.01M of CuSO4 solution. 2. Concentration required (ZnSO4): 0.99M AMU of ZnSO4: 161.44 So, 1.00M of CuSO4 has 161.44g of ZnSO4 Hence 0.99M has: 161.44 x 0.99 = 159.83g � 0.01g Mix 159.83g � 0.01g of ZnSO4 in 100mL of distilled water. ...read more.

Conclusion

Raw Data Table Volume of each electrolyte (mL � 1mL) Length of salt bridge (cm � 0.01 cm) Length of each electrode (cm � 0.01 cm) 100 16.00 6.00 Temperature (�C) Voltage (V) � 0.001 V Trial 1 Trial 2 Trial 3 23 1.028 1.029 1.028 30 1.036 1.038 1.039 40 1.048 1.050 1.048 50 1.057 1.059 1.057 60 1.069 1.067 1.067 70 1.073 1.073 1.070 80 1.076 1.074 1.075 90 1.081 1.079 1.078 Processed Data Temperature (�C) � 1 �C Average Voltage (V) 23 1.028 � 0.001 30 1.038 � 0.002 40 1.049 � 0.001 50 1.057 � 0.001 60 1.068 � 0.001 70 1.072 � 0.002 80 1.075 � 0.001 90 1.079 � 0.002 Data Processing Note: For the sample calculation below, data point 2 has been used (30�C � 1 �C). Average Voltage = Trial 1 + Trial 2 + Trial 3 3 = 1.036 + 1.038 + 1.039 3 = 1.0376 = 1.038 V Uncertainty of Average Voltage = Highest trial value - Lowest trial value 2 = 1.039 - 1.036 2 = 0.0015 = 0.002 V = 1.038 V � 0.002 V Graph Conclusion Evaluation Self Improvements ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry 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 International Baccalaureate Chemistry essays

  1. Design Lab-Voltaic Cell

    Record the Voltage in the data table. 5. Detach the voltmeter, wipe clean the electrodes. 6. Now place Zn into the copper solution and Cu into the zinc solution. 7. Attach Voltmeter, negative to Cu, and negative to Zn.

  2. Electrochemical cells - investigate the effect of the temperature change of the anode electrolyte ...

    of 3 Zinc metal, then clean them until they appear metallic shine, then put Zn strip into the solution of ZnSO4 and Mg strip into the solution of MgSO4. 3. Use the clamps to stable the Zn and mg, keep their immersion depth are the same.

  1. Investigating the effect of ion concentration in electrolytes on the potential difference in a ...

    Repeat steps 1~5 for the following concentrations (mol dm-3): 0.16, 0.12, 0.8 and 0.04. Make the desired concentration by adding appropriate volume of distilled water to the electrolytes. Use the equation, Mole 1 x Volume 1 = Mole 2 x Volume 2 to calculate the volume of distilled water and electrolyte needed 6.

  2. Esterification Equilibrium

    Moles of ethanol; calculating uncertainty 0.017 � 4.4x10-4 mol of ethanol was present. Moles of water are 0.212�0.0009mol. Mixture 6 and 7; Both of the mixture has 1ml of ethanoic acid, hence the amount in moles of ethanoic acid present in the original mixture is; Moles of ethanoic acid; calculating

  1. Effect of Concentration on Electrochemical Cell Potential Using Nernst Equation

    Hypothesis: An equal concentration of the solutions will result a cell potential equal to the standard because the logarithm of the reaction quotient will be 0. Variables and Controls Independent Variable: Concentration of copper and zinc nitrate Dependent Variable: Voltage of half electrodes Constant Variables: * Room Temperature (24.5�C)

  2. How duration affects the rate of electrolysis in a Voltaic Cell

    After that we cut out some filter paper and dip that into our spectator ion (potassium nitrate) in order to build a salt bridge. The salt bridge will primarily complete the circuit, allow flow of ions and maintain electrical neutrality.

  1. Chemistry Extended Essay - Viscosity of Xanthan Gum solutions

    The diagram shows a simplified view of the cell. At the cathode, copper(II) ions are deposited as copper. At the anode, copper goes into solution as copper(II) ions. For every copper ion that is deposited at the cathode, in principle another one goes into solution at the anode.

  2. Group 4

    Otherwise, the high internal pressure of the airbag would create a surface as hard as stone, a device that wouldn't result useful to the passenger or driver. Evaluation: The kinetic theory of gases assumes that gases are ideal, thus that there are no interactions between molecules, and the size of

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