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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Question
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
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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F792dc78a-e43b-409d-8062-d1e272a5b889%2F0c81b007-0d1b-4b57-881c-af545ed64a2c%2F53xqxhe_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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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