Answered: 1.calculate of the change in Gibbs'…

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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1.calculate of the change in Gibbs' free energy to the formation of the silver ion (Ag+(aq)) ∆°Gf

in the picture.

2. Calculate the equilibrium constant according to the concentrations of the next reaction at a temperature of
25 ° C: Ag+(aq) + 2NH3(aq) → Ag(NH3)2⁺ (aq)

3. Given the following electrochemical cell, constructed of a standard hydrogen electrode as the anode
And from half of Brom's cell:

Br2(l) + H2(g) + 2H2O(l)→2Br^-(aq)+ 2H3O+(aq)

Added silver ions until AgBr sinks on the cathode. the ionic concentration of ag+ reaches to 0.0600M and the ionic concentration of br- reaches to 8.5*10^-12. the cell voltage that has been measured at this point is 1.721V. calculate ∆°E

aq) +e → Ag,)
E°-0.7996V
AgBr(s) + e -→ Ags) + Br(aq)
E° 0.0713V
AGP (NH3(ag) ) =- 26.50 kJ/mol
AGr °( Ag ( NH:)2 (aq) ) = -17.12 kJ/mol

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