Work ExperienceProject Daniell Cell Made By: Sharad Raghav Class XII-A Daniell cell generates an electric . A porous partition or a salt bridge separates the two half-cells from each other. In this process. Working: The half reactions can be viewed as a competition between two kinds of metal atoms for electrons. Zn electrode dissolves in the solution of ZnSO4 and reduces in size while Cu electrode grows in size due to the deposition of copper metal. Electrons are here so cathode is the positive electrode. One half-cell is zinc rod dipped in 1M ZnSO4 solution. The two electrodes are connected together externally by a metal wire through a voltmeter are produced here so anode is the negative electrode. Both the reactions take place simultaneously at both the half-cell s. Construction: Daniell cell consists of two half-cells.Daniell Cell with Construction and Working Daniell cell is the simplest voltaic or galvanic cell. it will show the voltage. The copper rod acts as cathode where reduction takes place. both the positive and negative ions move through the aqueous solutions via the salt bridge. If there is a voltmeter. It converts chemical energy into electrical energy spontaneously. In this case zinc atoms are more reactive and their tendency to lose electrons is greater than that of copper. The other half-cell is copper rod dipped in a solution of 1M CuSO4. electrons travel in the external circuit through the wire from the zinc anode to the copper cathode. In this cell. To complete the circuit. If a bulb is in the circuit. it will light up. a porous pot. THEORY Reduction potential of an electrode increases with increase in concentration of the electrolyte. AIM: To study the variation of cell potential in Zn|Zn 2+||Cu2+|Cu cell with change in concentration of electrolytes (CuSO4 and ZnSO4) at room temperature. sand paper. using higher concentration of Cu2+ and lower concentration of Zn2+ ions increase the Ecell of Zn|Zn2+||Cu2+|Cu .potential of 1.10 volt. connecting wires.016V . when the solutions in the half cells are both 1M.----------------------> M(s) In the zinc-copper electrochemical cell zinc electrode acts as anode while copper electrode acts as cathode. Ecell =Ecathode .057V 1. milli voltmeter.064V 1.0125M EMF of the Cell 1. copper strip. of CuSO4 solution 1M 0.Eanode Ecell increases if Ecathode increases and Eanode decreases. of ZnSO4 solution 1M 1M 1M 1M Conc. 1M ZnSO4 solution and 1M CuSO4 solution. zinc strip.025M 0. OBSERVATIONS: Conc.059/n log [M]/[Mn+] APPARATUS AND CHEMICALS 1 beaker. Thus.5M 0.040V 1. The relation between concentration of the electrolyte and the standard electrode potential is given in the form of the Nernst Equation: E=E0 . Mn+ (aq) + ne.0. 0125M 1M 1M 1M 1. .5M 0.072V 1.0.025M o.071V 1.073V CONCLUSION: EMF of the cell increases with decrease in concentration of the electrolyte around anode and increase in concentration of the electrolyte around the cathode.