Calculate the value of the free energy change, ΔG, for the reaction below at 225.0ºC when the pressures of H₂ (g) = 5.00 atm, I₂ (g) = 5.00 atm, and HI (g) = 0.0750 atm. H₂ (g) + I₂ (g) → 2 HI (g) ΔGº=-15.92 kJ ΔHº=-9.48 kJ
Calculate the value of the free energy change, ΔG, for the reaction below at 225.0ºC when the pressures of H₂ (g) = 5.00 atm, I₂ (g) = 5.00 atm, and HI (g) = 0.0750 atm. H₂ (g) + I₂ (g) → 2 HI (g) ΔGº=-15.92 kJ ΔHº=-9.48 kJ
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter16: Thermodynamics
Section: Chapter Questions
Problem 45E: Consider the following reaction at 298 K: N2O4(g)2NO2(g)KP=0.142 What is the standard free energy...
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Calculate the value of the free energy change, ΔG, for the reaction below at 225.0ºC when the pressures of H₂ (g) = 5.00 atm, I₂ (g) = 5.00 atm, and HI (g) = 0.0750 atm.
H₂ (g) + I₂ (g) → 2 HI (g)
ΔGº=-15.92 kJ
ΔHº=-9.48 kJ
ΔSº=21.79 J/K
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