The equilibrium reaction for the solubility of silver chloride at 25 °C is as follows: AgCI (s) Ag* (aq) + Cr (aq) If it is known that the free Gibbs energy of standard formation (AG) AgCl is -109.8 kj Ag is 77.1 kJ, and Cl is -131.3 kJ. Answer the following questions: a) What is the number of changes in the Gibbs free energy (AG) produced. b) Determine whether the reaction is spontaneous or non-spontaneous. c) If the Kp of AgCI is 1.8 x 10^-10, calculate the solubility of AgCl in units of gL.Known: (Ar Ag 107.9, Cl 35.5 gmol) %3!

The equilibrium reaction for the solubility of silver chloride at 25 °C is as follows: AgCI (s) Ag* (aq) + Cr (aq) If it is known that the free Gibbs energy of standard formation (AG) AgCl is -109.8 kj Ag is 77.1 kJ, and Cl is -131.3 kJ. Answer the following questions: a) What is the number of changes in the Gibbs free energy (AG) produced. b) Determine whether the reaction is spontaneous or non-spontaneous. c) If the Kp of AgCI is 1.8 x 10^-10, calculate the solubility of AgCl in units of gL.Known: (Ar Ag 107.9, Cl 35.5 gmol) %3!

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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