how would you state Ag2CrO4 acting as a cathode?

Ag2CrO4.

The cathode is where reduction occurs. Reduction is either of the following:
Ag+ + e ==> Ag(s)
CrO4^= + 3e +8H^+==> Cr^+3 + 4H2O

To determine how Ag2CrO4 would act as a cathode, first, we need to understand the composition and properties of Ag2CrO4. Ag2CrO4 is the chemical formula for silver chromate. It consists of two silver ions (Ag+) and one chromate ion (CrO4^2-).

To determine whether Ag2CrO4 would act as a cathode, we need to consider its reduction potential. The reduction potential is a measure of the tendency of a substance to gain electrons and undergo reduction at the cathode during a redox reaction.

We can refer to the standard reduction potential (E°) values table to find the reduction potential of Ag2CrO4. The more positive the reduction potential, the greater the substance's tendency to act as a cathode.

After referencing the table, we find that the reduction potential for silver chromate (Ag2CrO4) is +0.62 V. This positive value suggests that Ag2CrO4 has a tendency to be reduced (gain electrons) and thus can act as a cathode during a redox reaction.

In summary, when Ag2CrO4 is involved in a redox reaction, it has the potential to act as a cathode due to its positive reduction potential (+0.62 V).