1. Determine ∆S for the phase change of 1.78 moles of naphthalene from solid to liquid at 80.3°C. (∆H = 18.8 kJ/mol) 2.

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1. Determine ∆S for the phase change of 1.78 moles of
naphthalene from solid to liquid at 80.3°C. (∆H = 18.8 kJ/mol)
2. Consider the reaction: ICl(g) + Cl₂(g) → ICl₃(s). The
∆G° of the reaction is -17.09 kJ/mol. Calculate the ∆G, in kJ/mol,
for the reaction at 298 K if the partial pressure of ICl(g) is
0.0400 atm and the partial pressure of Cl₂(g) is 0.00100 atm.
3. For a reaction where ∆H° = +573 kJ/mol and ∆S° = +1.64
kJ/mol･K, at what temperature, in K, does X(l) → X(g) occur
spontaneously?
4. Determine the equilibrium constant for a reaction at
260.0 K if ∆G° =38.70 kJ/mol. (R = 8.314 J/mol ･ K)
5. What is K for a reaction if ∆G° =-336.0 kJ/mol at 25.0
°C? (R = 8.314 J/mol ･ K)