Learning Goal: I’m working on a chemistry question and need an explanation and answer to help me learn.
10.0 g of solid AgCl(s) is added to 1,000 L of pure water at 25 °C and 1 atm total pressure. Ignore activity corrections.
a) Calculate Gtot for the system in this state (state 1). Ignore the contribution of water to Gtot.
b) Some of the AgCl(s) dissolves to form Ag+ and Cl− such that [Ag+] = [Cl–] = 9.5 μM? Calculate Gtot for the system in this state (state 2). Ignore the contribution of water to Gtot. Which is the more thermodynamically stable state?
c) What is the standard molar Gibbs energy change of reaction for AgCl(s) dissolving to form Ag+ and Cl–?
d) What is ΔG̅r at conditions when [Ag+] = [Cl–] = 9.5 μM? Is further dissolution of AgCl(s) favorable (i.e. spontaneous) under these conditions?
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