Given that E°_red = -0.45 V for Fe²⁺/Fe at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Fe(s)∣ Fe²⁺(1.0 × 10^-5 M)∣∣ Fe²⁺(0.100 M)∣ Fe(s)

Question

Quizplus · Accepted Answer

The shorthand notation of the concentration cell is: Fe(s)|Fe²⁺(1.0x10-5 M)||Fe²⁺(0.100 M)|Fe(s) First, we need to find E° for the half-reaction Fe²⁺/Fe: E°_red = -0.45 V We know that the oxidation half-reaction is Fe(s) → Fe²⁺, so the reduction half-reaction is the reverse: Fe²⁺ → Fe(s). We can use the formula E°cell = E°cathode - E°anode to find E°cell for the concentration cell: E°cell = E°cathode - E°anode E°cell = E°Fe²⁺(0.100 M) - E°Fe²⁺(1.0x10-5 M) E°cell = 0 - (-0.45) = +0.45 V Next, we can use the Nernst equation to find E for the concentration cell: E = E°cell - (RT/nF)ln(Q) Q = [Fe²⁺(1.0x10-5 M)]/[Fe²⁺(0.100 M)] Q = 1.0x10-4 E = 0.45 - (0.0257/2)ln(1.0x10-4) E = +0.12 V Therefore, the answer is B: E° = 0.00 V and E = +0.12 V.

Given That E°red = -0

Given That E°_red = -0