Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br- (aq) + I2(s) <--> Br2(l) + 2I- (aq)

Eocell = (0.0257/n) lnKeq, Calculate Eocell from Use this equation to calculate K value.

Eo (I2/I-) = +0.53, Eo (Br2/Br-) = +1.07,

Explanation:

The given chemical reaction is:

The relation between Eo cell and Keq is shown below:

The value of Eo cell is:

Br- undergoes oxidation and I2 undergoes reduction.

Reduction takes place at cathode.

Oxidation takes place at anode.

Hence,

F=96485 C/mol

n=2 mol

R=8.314 J.K-1.mol-1

T=298K

Substitute all these values in the above formula:

Keq=6.13x10^33

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm