electrochemistry question

Question

Given the following data

Ce⁴⁺(aq) + e^–  → Ce³⁺(aq)  E° =+1.61V

Hg²⁺(aq) + 2 e^– →  Hg(l) E° = +0.855

Calculate the standard potential in Volts of the galvanic cell that could be built based on the two half reactions above. Enter only numerical answer, do not enter units. 

Answer 1

Assuming these are reduction potentials, the E_cathode - E_anode = E_cell

Cathode is where reduction takes place, so it would be Ce and anode would be Hg. Thus...

E_cell = 1.61 V - 0855 V = 0.76 V