AchieveQ9

[Moselle Stieler 3A]

Hi,
I was never able to solve this problem on Achieve:
A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M
iron(II) ion solution and another electrode composed of silver in a 1.0 M
silver ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C.
Refer to the list of standard reduction potentials.
Can someone please break it down step by step? Thanks :)

[Hannah Fiel 2H]

Referring to the list of standard reduction potentials, you will find the following reduction potentials for the given elements in the reaction

Fe2+(aq) + 2e– → Fe(s), standard reduction potential= –0.44
Ag+(aq) + e– → Ag(s), standard reduction potential=0.8

Use this equation to calculate the standard reduction potential for the entire cell: E∘cell=E∘cathode−E∘anode

Determine which reaction occurs at the cathode and anode by looking at where reduction and oxidation occur respectively.

[YSH]

The higher the standard reduction potential, the better the oxidizing agent (more suited as an oxidizing agent) so in this case Ag would be the oxidizing agent and be reduced and Fe would be oxidized. So the E cathode would be 0.8 and E anode would be -0.44.
Hope this helps!