1-What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag+ concentration is 8.50×10-4 M and the Al3+ concentration is 1.48 M ? 3Ag+(aq) + Al(s)3Ag(s) + Al3+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: True or False
1-What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag+ concentration is 8.50×10-4 M and the Al3+ concentration is 1.48 M ? 3Ag+(aq) + Al(s)3Ag(s) + Al3+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: True or False
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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1-What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag+ concentration is 8.50×10-4 M and the Al3+ concentration is 1.48 M ?
3Ag+(aq) + Al(s)3Ag(s) + Al3+(aq)
Answer: V
The cell reaction as written above is spontaneous for the concentrations given: True or False
2-
-
Consider the following reaction at 298K.
2 H+(aq) + Ni (s) H2(g) + Ni2+(aq)
Which of the following statements are correct?
Choose all that apply.
n = 5 mol electrons
The reaction is product-favored.
K < 1
delta Go < 0
Eocell < 0
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