Problem 1: Cell EMF Calculation (E°cell)

Q: Calculate the standard cell EMF for Fe|$Fe^{2+}$||$Ag^{+}$|Ag. E°($Fe^{2+}$/Fe) = −0.44 V, E°($Ag^{+}$/Ag) = +0.80 V.

Step 1: Identify cathode and anode.

• Cell notation: left = anode (Fe), right = cathode (Ag)
• Fe is oxidized (anode): Fe → $Fe^{2+}$ + 2$e^{-}$
• $Ag^{+}$ is reduced (cathode): $Ag^{+}$ + $e^{-}$ → Ag

Step 2: Apply formula. $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} = (+0.80) - (-0.44) = +1.24 \text{ V}$

Step 3: Verify sign. E°cell = +1.24 V > 0 → spontaneous galvanic cell. ✓