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Constructing Electrochemical Series Based on Potential
Difference Between…
Constructing Electrochemical Series Based on Potential
Difference Between Two Metals with Zinc Nitrate as Electrolyte
Procedure
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Both strip connected to the voltmeter by using the crocodile clip and dip into the beaker containing electrolyte
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Experiment is repeated with copper strip, magnesium strip, silver strip and aluminium strip
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Discussion
Electrochemical series is a series of chemical elements arranged in order of their standard electrode potentials.
The standard electrode potential will be arranged based on its reactivity.More reactive metal will on the top on the electrochemical series while low reactive
metal will be on the bottom of the electrochemical series.More reactive metal usually exist as reducing agent which will had the oxidation reaction at anode terminal.
When the reactivity increased,the electropositivity increased. In this experiment,simple voltaic cell was used.After the voltaic cell prepared,the redox reaction occur.
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Precaution:Prepare more solution before start the experiment and used different solution in each metallic pair
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Abstract
The aim of the experiment is to constructing electrochemical series based on potential difference between two metals with zinc nitrate as electrolyte.In this experiment,we investigated about how the
electrochemical series was formed based on voltage obtained on reaction between metallic pair in 0.1M zinc nitrate solution.Zinc electrode was set as standard in each metallic pair.
Zinc electrode was at negative terminal when react with Pb,Cu and Ag electrode.For the reaction with Al and Mg electrode,zinc electrode will be at negative terminal.The redox reaction will occur.
Electrode that exist as oxidizing agent will have reduction process on negative terminal(anode) while reducing agent will have oxidation process in positive terminal(cathode)
Al and Mg will be on top of electrochemical series but Mg,Pb,Cu and Ag will be low than zinc
In conclusion,the electrochemical series can be determined by obtain the voltage difference of each metal electrode with zinc electrode.If the voltage increased,the position of certain metal will be far from the zinc position in electrochemical series whether it was more electronegativity or more electropositivity.
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Conclusion
The electrochemical series can be constructed by using different pairs of metal in simple voltaic cell. The series that we got is, Al,Mg,Zn,Pb,Ag and Cu .
Introduction
By measuring the potentials of various electrodes versus standard hydrogen electrode (SHE), a series of standard electrode potential has been established. When the electrodes (metal and non-metal) in contact with their ions are arranged on the basis of the values of their standard reduction potential or standard oxidation potentials, the resulting series is called the electrochemical or electromotive of activity series of the elements.
The electrochemical series has its own characteristics. Firstly, the substances which are stronger reducing agents than hydrogen in the series and have negative values of standard reduction potential. Then,the metals on the top (having high negative values of standard reduction potential) have the tendency to lose electron readily. These are active metals. So,the activity metal decreases from top to bottom. After that, the non metals on the bottom (having high positive values of standard reduction potentials) have tendency to accept electrons readily. These are active non-metals. Does, the activity of non-metals increases from top to bottom
The construction experiment of simple voltaic cell consists of two metal plates immerse in an electrolyte.The metal which is higher in electrochemical series will become the negative terminal.The atom of the metal which is higher in electrochemical series will release electron to form negative ions.The electrons are then move to the other metal plate through the wire. The metal which is lower in electrochemical series will become the positive terminal. In positive terminal, the electrons will be released to the positive ions in the electrolyte
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