Question

ered 1.00 EXPERIMENT 2: The molarity of the Cu2+ and Zn2+ solutions used in the setup of the electrochemical cell was 1 M. Explain why the voltage was not equal to the standard reduction potential for the Cu Zn redox reaction at all times during the experiment

Answer 1

Note: Electrochemical can never have negative electrode potential otherwise the reaction taking place will not be spontaneous and cell will not work. Anode and cathode in electrochemical cells are dependentbon their standard reduction potentials which are constant for a particular specie.

= Molarity of cyht and 2n2+ solutions in on electrochemical all reaction for Eulen llicro chemical ull, following reactions take place In Zn2+ +2e- Cupt thé - cu 2+ € - HOV Net reaction = Zn + 2+ i + 2027 Standard electro de potential do not remains same because when reaction starts in all, concentration of Cult decreases and 2n2t increases which changes the potential continuously. Eault = €cu - 0.0591 log Element Hov 2 O [ Cupt] The above equation shows dependence of fell on concentration of com. So with change in concentration of solutions, electrode potential changes,