Electrochemistry Lab Report

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Electrochemistry is the study of reactions in which charged particles (ions or electrons) appear in two phases of matter, such as the metallic phase (the electrode) or aqueous phase (the electrolyte). (Lower 2004) These reactions involve the transfer of electric charges between the electrodes and the electrolyte. These cells have two electrodes which are named the anode and the cathode. The anode is the electrode where oxidation occurs and the cathode is the electrode where reduction occurs (Electrochemical cells 2014). Oxidation always occurs simultaneously to reduction and the process of this electron transfer is named a redox reaction (A.Olivier 2010). In this experiment, the metals that I will use as electrodes are zinc, magnesium, copper and lead. The electrolytes…show more content…
The salt bridge that was used was KNO3 which is potassium nitrate. Potential difference is the work done per unit charge and it is measured in Volts. To measure this it is required that you connect the two half cells to a voltmeter and record the voltmeter reading. The cells must be left in the aqueous solution until there is a voltmeter reading. INVESTIGATIVE QUESTION Is the effectiveness of a half cell determined by the cell potential of that half cell? HYPOTHESIS It is predicted that the Zinc and Magnesium electrode will be the most effective half cell because they are the strongest reducing agents on the standard reduction potential table. AIM The aim of this experiment is to identify which half cell reaction will produce the most effective electrochemical cell PLANNED MEAUSREMENTS Independent variable: Zinc half cell Dependant variable: Cell potential, Voltage Controlled variable: Voltmeter, Salt Bridge, 4 different half cells APPARATUS • Voltmeter • 4 half cells :  Zn/ZnSO4 (aq)  Cu/CuSO4 (aq)  Fe/FeSO4

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