16.4 Exercise 27

Determine ΔGº for the following reactions.

(a) Antimony pentachloride decomposes at 448 °C. The reaction is:
$\text{SbCl}_{5} \left(g\right) \rightarrow \text{SbCl}_{3} \left(g\right) + \text{Cl}_{2} \left(g\right)$

An equilibrium mixture in a 5.00 L flask at 448 °C contains 3.85 g of SbCl₅, 9.14 g of SbCl₃, and 2.84 g of Cl₂.

(b) Chlorine molecules dissociate according to this reaction:
$\text{Cl}_{2} \left(g\right) \rightarrow 2 \text{Cl} \left(g\right)$

1.00% of Cl₂ molecules dissociate at 975 K and a pressure of 1.00 atm.