Determine $\Delta$G° for a cell that utilizes the following reaction: Cl₂(g)+ 2Br^-(aq)$\to$2Cl^-(aq)+ Br₂(l) The standard reduction for the chlorine gas is 1.360 volts and the standard reduction for the bromine liquid is about 1.078 volts.

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The cell potential (E°cell) is calculated by subtracting the standard reduction potential of the anode (bromine) from the cathode (chlorine): E°cell = 1.360 V - 1.078 V = 0.282 V. The Gibbs free energy change (ΔG°) is calculated using the formula ΔG° = -nFE°cell, where n = 2 (moles of electrons transferred) and F = 96485 C/mol. ΔG° = -2 * 96485 * 0.282 = -54.4 kJ.

Determine Δ\DeltaΔ G° for a Cell That Utilizes the Following Reaction: Cl2(g)

Determine $\Delta$ G° for a Cell That Utilizes the Following Reaction: Cl₂(g)