wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Calculate
ΔG0 and the equilibrium constant for the formation of NO2 from NO and O2 at 298K
NO+1/2O2NO2, where
ΔfG0(NO2)=52.0kJ/mol,ΔfG0(NO)=87.0kJ/mol,ΔfG0(O2)=0kJ/mol

Open in App
Solution

NO+12O2NO2
ΔGoreaction=ΔGo(Products)ΔGo(reactants)
ΔGoreaction=ΔGo(NO2)[ΔGo(NO)+12ΔGo(O2)]
ΔGoreaction=(52.0)(87.0)12×0
ΔGoreaction=35 kJ/mol
For equilibrium,
ΔGoreaction=RTlnKeq
35×103=8.314×298×lnKeq
lnKeq=14.1267×103
Keq=1.014
Therefore, the equilibrium constant is 1.014

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Le Chateliers Principle
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon