Determine ΔG° for a cell that utilizes the following reaction: Cl2(g) + 2Br–(aq) → 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 1.075 volts. Group of answer choices

The ΔG° for a cell is 55000 J

The equation for the reaction is given as:

In the reaction, the reduction of chlorine takes place at the cathode;

i.e.

The oxidation of Bromine takes place at the anode;

i.e.

The Cell potential can be calculated as:

∴

The ΔG° for a cell can be determined by using the expression;

where;

Learn more about Faraday's Law here:

link

∆G°= -55005J or -55KJ

Explanation:

The first step is to determine E°cell= E°cathode - E°anode

2Cl-(aq)/Cl2(g) system is the cathode while 2Br-(aq)/Br2(g) is the anode

E°cell= 1.360-1.075

E°cell= 0.285V

From

∆G°= -nFE°cell

n= 2 from the balanced reaction equation, two electrons were transferred.

F= 96500

E°cell=0.285V

∆G°= -(2×96500×0.285)

∆G°= -55005J or -55KJ

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .