A student constructed a voltaic cell by combining Sn/Sn2+ and Zn/Zn2+ two half cells and measured a cell potential of 0.620 V. He then constructed a voltaic cell by combining Sn/Sn2+ and Ni/Ni2+ two half cells and measured a cell potential of 0.140 V. It is seen that the tin metal precipitated out of the solution in each above cell. Except for the reduction potential of Zn which is known as -0.763V, the reduction potentials of all the other two electrodes are unknown.  a. Calculate the reduction potential of Sn2+ (aq)+ 2e- ---> Sn(s).  b. Calculate the reduction potential of Ni2+(aq)+2e- ----> Ni(s) c. Write the cell reaction for the cell of Sn/Sn2+ and Zn/Zn2+

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.