The redox reaction is 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) Calculate the following for the reaction at 298.0 K .A) The standard Gibbs free energy change of the reaction @ 298.0 K B) The equilibrium constant for the reaction C) The standard cell potential
The redox reaction is 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) Calculate the following for the reaction at 298.0 K .A) The standard Gibbs free energy change of the reaction @ 298.0 K B) The equilibrium constant for the reaction C) The standard cell potential
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 24E: For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is...
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2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq)
Calculate the following for the reaction at 298.0 K
.A) The standard Gibbs free energy change of the reaction @ 298.0 K
B) The equilibrium constant for the reaction
C) The standard cell potential
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this aprt of calculation seems wrong
ΔG° = -RTln(K)
=>-3.9 × 10^5 J/Mol. = - 8.314 J/K .Mol × 298K ln (K)
By Solving K = 9.77× 10^68
I think it is
(-3.9 × 10^5 J/Mol) = (- 8.314 J/K Mol × 298K x ln(K)
ln (K)= (-3.9 × 10^5 J/Mol) / (-8.314 J/K Mol × 298)
ln (K)= 157.4
K = e^157.4
K = 2.3 x 10^68
are you right or me
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by Bartleby ExpertFollow-up Question
2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) how di you get this reaction , i provided a different one
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