Identigying Anode/Cathode when just given species names and concentrations

[Grace Ramey 2K]

The following items are obtained from the stockroom for the construction of a galvanic cell: two 250-mL beakers and a salt bridge, a voltmeter with attached wires and clips, 200 mL of 0.0080 M CrCl3 (aq), 200 mL of 0.12 M CuSO4 (aq), a piece of copper wire, and a chrome-plated piece of metal.

The question asks for a drawing of the galvanic cell. My question is, how do you determine which solution+metal combination will be the cathode, and which will be the anode (e.g. the combination involving chromium or the combination involving copper)? Do we need more information or are we supposed to be able to tell which is which just given the names and concentrations of the species?

Thank you for your help!

[Abel Thomas 2C]

I think for these types of problems we will be given a sheet of half-reactions. The larger the cell potential is for the specific half reaction, the more likely it is to be reduced. Thus, we can say that this half-reaction occurs at the cathode. Therefore, the other half-reaction will occur at the anode.

[Gianna Apoderado 1B]

Given the species, you can generally predict which reaction will be the reduction and oxidation from a given list of reactions and their standard reduction potentials. The more positive E^o, the stronger the oxidizing agent is, and the more likely that the species will be reduced.

[Riya Pathare 2E]

A galvanic cell will produce a current generally so the voltage must be positive. Thus if we are given reduction potentials we want to flip the half reaction that will produce a positive voltage when added. The anode will be the oxidation, the one you flip and the cathode will be the reduction which is the half reaction that you keep as the reduction potential form.

[Nate O 2L]

To answer the second part of your question, you shouldn't need to know any additional info besides the information already given.