Question

Consider the following reaction at 298K.
I2 (s) + 2 Fe2+ (aq) 2 I- (aq) + 2 Fe3+ (aq)

Which of the following statements are correct?

Choose all that apply.
ΔGo > 0
K < 1
The reaction is product-favored.
n = 2 mol electrons
Eocell > 0


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Answer 1

$$E_{cell}^0 = E_{Red}^0 - E_{Ox}^0$$

$I_2(s) + 2e^- \rightarrow 2I^-$ $E_{Red}^0 = 0.54 V$

$(Fe^{2+} \rightarrow Fe^{3+} +1e^-)\times2$ $E_{Ox}^0=-0.77 V$

$$E_{cell}^0= 0.54+(-0.77)= -0.23 V$$

$$\Delta G_0= -nFE_{cell}^0= -2\times 96485.309\times (-0.23)= 44383\frac{J}{mol}$$

$$\Delta G = -RTlnK$$

$$44383= -8.314\times 8.314lnK$$

$$K= e^{-\frac{44383}{8.314\times298}}= 1.66\times10^{-8}$$

Right answers are:

$\Delta G_0>0$

$K<1$