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Author Question: The equilibrium constant for the reaction AgBr(s) Ag+(aq) + Br (aq) is the solubility product ... (Read 83 times)

acwiles

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Question 1

The equilibrium constant at 427°C for the reaction N2(g) + 3H2(g) 2NH3(g) is Kp = 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, Ksp = 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


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Marked as best answer by acwiles on Nov 5, 2023

gyvette

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acwiles

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Reply 2 on: Nov 5, 2023
Excellent


TheNamesImani

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Reply 3 on: Yesterday
Thanks for the timely response, appreciate it

 

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