Consider the Voltaic Cell Based on the Following Reaction:
$\rightarrow$

Consider the voltaic cell based on the following reaction:
Zn(s) + Ni^{2 +}(aq) $\rightarrow$ Zn^{2 +}(aq) + Ni(s)
Two students are assigned to measure the standard cell potential at 25°C.Student 1 claims that both solutions of ions have to be at exactly 1.00 M concentration, but student 2 is sure that the measurement will be the same if the concentrations of the two solutions are equal, but not necessarily
1) 00 M.What do you think?

A) Student 1 is right because, by definition, standard cell potentials must be measured at concentrations of 1.00 M.
B) Student 1 is right because she understands the Nernst equation and what it describes.
C) Student 2 is right because she understands the Nernst equation and what it describes.
D) Student 2 is right because cell potentials do not depend on the concentration.
E) Both are right because cell potentials do not depend on the concentration.