The equilibrium constant for the reaction AgBr(s) Ag+(aq) + Br ...

[acwiles]

Question 1

The equilibrium constant at 427°C for the reaction N₂(g) + 3H₂(g) 2NH₃(g) is K_p = 9.4 × 10^–5.  Calculate the value of ΔG° for the reaction under these conditions.
◦ –33 kJ/mol
◦ –54 kJ/mol
◦ 54 kJ/mol
◦ 33 kJ/mol
◦ 1.3 J/mol

Question 2

The equilibrium constant for the reaction AgBr(s) Ag⁺(aq) + Br^– (aq) is the solubility product constant, K_sp = 7.7 × 10^–13 at 25°C.  Calculate ΔG for the reaction when [Ag⁺] = 1.0 × 10^–2 M and [Br^–] = 1.0 × 10^–3 M.  Is the reaction spontaneous or nonspontaneous at these concentrations?
◦ ΔG = 69.1 kJ/mol, nonspontaneous
◦ ΔG = –69.1 kJ/mol, spontaneous
◦ ΔG = 97.5 kJ/mol, spontaneous
◦ ΔG = 40.6 kJ/mol, nonspontaneous
◦ ΔG = –97.5 kJ/mol, nonspontaneous

[gyvette]

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[acwiles]

TYSM

[kalskdjl1212]

Thanks for the timely response, appreciate it