Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.859 M and [Ni2 ] = 0.0190 M. Standard reduction potentials can be found here.
Cr+Ni(2+) ->Cr(2+) + Ni
Ecell = Eocell - (0.0592/n)log[(Cr^2+)/(Ni^2+)]
and you get Eocell by adding the OXIDATION for Cr to the REDUCTION of Ni^2+. I would do it here but the values in your text won't agree with the values in my OLD text.
3548h-869
To calculate the cell potential for the given reaction, we need to use the Nernst equation. The Nernst equation relates the cell potential to the concentrations of the species involved in the reaction.
The Nernst equation is given as follows:
E(cell) = E°(cell) - (0.0592/n) * log(Q)
Where:
E(cell) is the cell potential
E°(cell) is the standard cell potential
n is the number of electrons transferred in the reaction
Q is the reaction quotient, which is given by the concentrations of the reactants and products raised to their stoichiometric coefficients.
First, let's find the standard reduction potentials for the species involved in the reaction. You mentioned they can be found elsewhere. Do you have the values for them?