Question

1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol

Which of the following is true?

ΔG = -44.8 kJ/mol and the process will not be spontaneous

ΔG = +39.4 kJ/mol and the process will be spontaneous

ΔG = -44.8 kJ/mol and the process will be spontaneous

ΔG = -19.1 kJ/mol and the process will not be spontaneous

ΔG = +39.4 kJ/mol and the process will not be spontaneous

2. Consider a process with ∆H = -89.8 kJ and ∆S = -151 J/K. At what temperature will this process be at equilibrium?

450

760

595

234

378

3. What does the standard change in Gibbs free energy (ΔG° ) of a reaction tell us about the equilbrium constant (K) for that reaction under standard conditions?

A negative ΔGº indicates that reactant formation is favored, and K will be less than 1.

There is no significant relationship between ΔG° and K

A negative ΔG° indicates that product formation is favored, and K will be greater than 1.

4.What is ΔS_surr (in J/K) if ΔH_sys is -27.2 kJ and T is 379 K?

5. Which of the following processes have a ΔS that is positive? More then one answer

2 N₂O₅ (g) → 4 NO₂ (g) + O₂ (g)

CO₂ (s) → CO₂ (g)

H₂O (l) → H₂O(s)

N₂ (g) → N₂ (l)

Al (s) → Al (l)

Answer 1

Answer 2