University:
Emporia State University
Course:
CH 126 | Chemistry Ii
Academic year:

2023
Views:

214

Pages:

1
Author:

Jerry Crosby

Chem II HW Set 24 1. Use the Nernst equation to predict the spontaneity of the redox reaction shown below. Co(s)+Fe2+(aq,1.94M)⟶Co2+(aq, 0.15M)+Fe(s) 2. The standard potential () of a voltaic cell based on the Zn/Cu2+ ion reaction: Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s) is 1.104 V. What is the value of at 25°C when [Cu2+] = 0.100 M and [Zn2+] = 1.90 M? 3. a) 2 Fe³⁺(aq) + 3 Cu(s) ⇌ 2 Fe(s) + 3 Cu²⁺(aq) E°cell = 0.771 – 0.34 = 0.431V ΔG° = -nEF = -249523 J/mol K = e100.1 = 5.212 x 1043 Spontaneous reaction b) Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) E°cell = 0.7996 – 0.34 = 0.4596V ΔG° = -nEF = -88702.8 J/mol K = e35.78 = 3.475 x 1015 Spontaneous reaction c) Mn(s)+Ni2+(aq)⟶Mn2+(aq)+Ni(s) E°cell = -0.257 – (-1.185) = 0.928V ΔG° = -nEF = -179104 J/mol K = e72.25 = 2.396 x 1031 Spontaneous reaction d) 3Cd(s)+2Al3+(aq)⟶3Cd2+(aq)+2Al(s) E°cell = (-1.662)– (-0.403) = -1.259V ΔG° = -nEF = 728961 J/mol K = e-294 = 0 Non-spontaneous reaction

Chemistry II HW Set 24

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