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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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thunter609 thunter609
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A month ago

The equilibrium constant for the reaction image 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? (R = 8.314 J/K • mol)



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ΔG = 69.1 kJ/mol, nonspontaneous



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ΔG = –69.1 kJ/mol, spontaneous



▸

ΔG = 97.5 kJ/mol, spontaneous



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ΔG = 40.6 kJ/mol, nonspontaneous



▸

ΔG = –97.5 kJ/mol, nonspontaneous

Textbook 
Chemistry: Atoms First

Chemistry: Atoms First


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finley07finley07
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