Consider the following half reactions:
Zn2+(aq) + 2e- → Zn(s) Eo = -0.76V
Fe3+(aq) + 3e- → Fe(s) Eo = -0.036V
If these two metals were used to construct a galvanic cell:
Calculate Gibb's Free Energy (in kJ) for this electrochemical cell Report value to 3 sig figs
Identify the appropriate redox reaction represented by the following cell notation.
Fe(s) ∣ Fe2+(aq) II Cu2+(aq) ∣ Cu(s)
Group of answer choices
Cu(s) + Fe2+(aq) → Fe(s) + Cu2+(aq)
Fe(s) + Cu2+(aq) → Cu(s) + Fe2+(aq)
2 Fe(s) + Cu2+(aq) → Cu(s) + 2 Fe2+(aq)
2 Cu(s) + Fe2+(aq) → Fe(s) + 2 Cu2+(aq)
3 Fe(s) + 2 Cu2+(aq) → 2 Cu(s) + 3 Fe2+(aq)