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Chemistry lab report Experiment 32 Voltaic Cell Measurements Tutankhamen Yearly Partner Zamia Behaves General Chemistry II lab Instructor Irrationals Babushka Nazarene University Introduction Most of the chemical reactions can be classified as redo reactions, which include two half reactions, oxidation and reduction respectively. To measure the tendency for a reader reaction to occur, special apparatus called voltaic cell can be used. It is made by connecting a voltmeter between two electrodes, which are immersed in to the two different solutions separated by porous barrier.

This airier allows flow of ions, so that the voltage or potential can be measured. In a closer look of such reactions, it can be determined that the sum of the potentials of oxidation and reduction is actually the voltage of the whole voltaic cell. For convenience negative electrode of the voltaic cell is considered to be that where oxidation occurs – anode, and it is connected to the negative pole of electrode. The picture bellow is a schematic diagram of the voltaic cell which we will study. However this also makes trouble in calculating individual potentials of reduction or oxidation.

Cable clips I Glass crucible I Wash bottle I Safety goggles I Lab coat I Discussion In Part A all of the seven cells were made up well and the cell potential of each of them were accurately measured. It was investigated that the highest potential was when iron and zinc electrode systems were connected. The cell potential was equal to 1. 51 V. Since standard potential of oxidation of zinc is 0. IV and the same potential but now for reduction of the zinc is 0. IV, the total Cell must be about 1. 51 V. Actual result that we got is also 1. IV, which tells us that our experiment was conducted very accurately. However, there might be some errors, and in combined effect they could result in some inaccuracy. For instance we could not properly wash the beaker and particularly crucible with porous bottom, where the ions from the previous cell could be found. For avoiding such mistake it is better to use each time clear crucible, however this would result in insufficient founding for other more important experiments, so to wash all the equipments better next time.

In contrast the smallest value we obtained during he lab was when we connected copper and potassium iodide. The total cell potential was recorded as 0. IV. Fortunately, even smallest result was correct. According to the table of half reactions, the strength of oxidation of cupper is 0. IV, and as mentioned before potential of the reduction strength of did is 0. 51 V. Theoretically the total potential must be approximately O. IV, just like as we got. Conclusion Overall, this experiment was provided without any significant complications and this laboratory work was very useful in understanding the voltaic cell.

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