Question

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,

Answer 1

The equilibrium constant, Keq, can be calculated using the Nernst equation and the given standard reduction potentials. The standard reduction potentials for the half-reactions in the given equation are Eo (I2/I-) = +0.53 and Eo (Br2/Br-) = +1.07. To calculate Keq, we can use these values in the Nernst equation and solve for lnKeq.

Step-by-step explanation:

The equilibrium constant, Keq, can be calculated using the Nernst equation and the given standard reduction potentials. The Nernst equation is Ecell = (0.0257/n) lnKeq, where Ecell is the cell potential, n is the number of electrons transferred in the balanced equation, and lnKeq is the natural logarithm of the equilibrium constant. The standard reduction potentials for the half-reactions in the given equation are Eo (I2/I-) = +0.53 and Eo (Br2/Br-) = +1.07.

To calculate Eocell, we can use the given Eo values and plug them into the Nernst equation. Since the reaction involves the transfer of two electrons, n = 2. Plugging in the Eo values:

Eocell = (0.0257/2) lnKeq

0.53 + 1.07 = (0.0257/2) lnKeq

1.6 = 0.01285 lnKeq

lnKeq = 124.27

Now, we can find Keq by taking the inverse natural logarithm of lnKeq:

Keq = e^lnKeq = e^124.27 = 3.75 x 10^53