Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s) + Fe(s)
For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Question

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Quizplus · Accepted Answer

The Gibbs free energy change (ΔG°) for a reaction can be calculated using the formula ΔG° = -nFE°cell, where n is the number of moles of electrons transferred in the reaction, F is the Faraday constant (96485 C/mol), and E°cell is the standard cell potential. In this reaction, 2 moles of electrons are transferred (from the oxidation of 2Na to Na+), and E°cell is given as 2.35 V. Thus, ΔG° = -2 * 96485 * 2.35 = -453,189 J or -453 kJ. The negative sign indicates that the reaction is spontaneous under standard conditions at 200°C.

Consider the Nonaqueous Cell Reaction 2Na(l) + FeCl2(s) ⇄ 2NaCl(s)

Consider the Nonaqueous Cell Reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s)