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Calculate the standard entropy, Δ?∘rxn, of the reaction at 25.0 ∘ C using the table of thermodynamic properties. C2H4(g)+H2O(l)⟶C2H5OH(l) C2H4(g)= 219.3 H2O(l)= 70.0 C2H5OH(l)= 160.7 Calculate the standard Gibbs free energy of the reaction, Δ?∘rxn. The standard enthalpy of the reaction, Δ?∘rxn, is −44.2 kJ⋅mol−1. C2H4(g)= 68.4 H2O(l)= -237.1 C2H5OH(l)= -166.6

Calculate the standard entropy, Δ?∘rxn, of the reaction at 25.0 ∘ C using the table of thermodynamic properties. C2H4(g)+H2O(l)⟶C2H5OH(l) C2H4(g)= 219.3 H2O(l)= 70.0 C2H5OH(l)= 160.7 Calculate the standard Gibbs free energy of the reaction, Δ?∘rxn. The standard enthalpy of the reaction, Δ?∘rxn, is −44.2 kJ⋅mol−1. C2H4(g)= 68.4 H2O(l)= -237.1 C2H5OH(l)= -166.6

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
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Calculate the standard entropy, Δ?∘rxn, of the reaction at 25.0 ∘ C using the table of thermodynamic properties.

C2H4(g)+H2O(l)⟶C2H5OH(l)

C2H4(g)= 219.3

H2O(l)= 70.0

C2H5OH(l)= 160.7

Calculate the standard Gibbs free energy of the reaction, Δ?∘rxn. The standard enthalpy of the reaction, Δ?∘rxn, is −44.2 kJ⋅mol−1.

C2H4(g)= 68.4

H2O(l)= -237.1

C2H5OH(l)= -166.6

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