Electrochemical Cell Lab Report

Introduction:
This lab is destined to calculate the cell potential of different electrochemical cell. Electrochemical cells is very useful in everyday life. Thanks to them, we have batteries that powers our mobile phones, laptops and so on.. Electrochemical Cells are devices in which chemical energy released during a chemical reaction is converted into electrical energy . A typical cell might consist of two half cells. Each half-cell consists of cathode, electrode where reduction(gain of electrons) is happened, or anode in which oxidation(loss of electrons) is happened, and electrolyte, a solution containing the corresponding cation(metal) of the half-reaction. The electrode of the half-cells are connected by a wire along which the electrons flow. And two solutions are separated by a salt bridge. As long as electrode is dipped in its electrolyte, potential difference is developed at the metal solution interface. The potential difference between the two electrodes in a galvanic cell is called a cell potential or emf of the cell. Thus magnitude of the potential depends on the nature of metals

In experiment 3, iron electrode is defined as cathode, because the more positive (or less negative) the reduction potential, the greater is the tendency for the reduction to occur. So in third experiment, Fe2+ has a greater tendency to be reduced than Zn2+. Moreover, Zn has a greater tendency to be oxidized than Fe. Due to the in the anode is negative electrode in which oxidation reaction is occur, Zn electrode is defined as anode. However, in forth experiment iron act as anode, because the value of E0 of iron is more negative than E0 of copper. The standard reduction potentials are -0.44V for iron and +0.34 V for copper. After the cathod and anode was defined, the cell potential in experiment 2&3&4 was measured. There was some inconsistencies with theoretical value of the cell