An electrochemical (galvanic) cell consists of a pure cadmium electrode immersed in a solution of cadmium (II) nitrate. This is connected via a salt bridge (containing sodium nitrate) to a half-cell containing a graphite electrode immersed in an acidified dichromate solution in which chromium ions are also present. 3.1.1 Identify the half-reactions and then write down the fully balanced cell reaction, showing all phases. 3.1.2 Calculate the standard potential for this cell and use your answer to determine the value of /\rG 0 (in kJ) for the system at 25 3.1.3 Consider this same cell, with a standard cadmium half-cell, and in the other compartment the dichromate ion concentration is 0.950 M, [h3o+] =7.14x10^-3 M and the concentration of chromium ions is 0.696 M. Determine the potential of the cell under these conditions. 3.1.4 Comparing your answer in question 3.1.3 with the standard cell potential, comment on the change in spontaneity of the cell reaction under the non-standard conditions.
3.1 An
3.1.1 Identify the half-reactions and then write down the fully balanced cell reaction, showing all phases.
3.1.2 Calculate the standard potential for this cell and use your answer to determine the value of /\rG 0 (in kJ) for the system at 25
3.1.3 Consider this same cell, with a standard cadmium half-cell, and in the other compartment the dichromate ion concentration is 0.950 M, [h3o+] =7.14x10^-3 M and the concentration of chromium ions is 0.696 M.
Determine the potential of the cell under these conditions.
3.1.4 Comparing your answer in question 3.1.3 with the standard cell potential, comment on the change in spontaneity of the cell reaction under the non-standard conditions.
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