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H2O(S)  = H2O(L) We already know that the Gibbs energy change of the reaction is 0 J/mol reaction at 0 oC and 1 bar.  Calculate the Gibbs energy change of the reaction at 1.18 oC and 1 bar. ΔrG = _________ J/mol. 3 sig. fig.  The following data are copied from the appendix of the textbook and assuming constants in the temperature region: Smo (ice) = 37.99 J K-1 mol-1          Smo (water liquid) = 69.91 J K-1 mol-1

H2O(S)  = H2O(L) We already know that the Gibbs energy change of the reaction is 0 J/mol reaction at 0 oC and 1 bar.  Calculate the Gibbs energy change of the reaction at 1.18 oC and 1 bar. ΔrG = _________ J/mol. 3 sig. fig.  The following data are copied from the appendix of the textbook and assuming constants in the temperature region: Smo (ice) = 37.99 J K-1 mol-1          Smo (water liquid) = 69.91 J K-1 mol-1

Chemistry
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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H2O(S)  = H2O(L)

We already know that the Gibbs energy change of the reaction is 0 J/mol reaction at 0 oC and 1 bar. 

Calculate the Gibbs energy change of the reaction at 1.18 oC and 1 bar. ΔrG = _________ J/mol. 3 sig. fig. 

The following data are copied from the appendix of the textbook and assuming constants in the temperature region:

Smo (ice) = 37.99 J K-1 mol-1         

Smo (water liquid) = 69.91 J K-1 mol-1 

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