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Chemistry?
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species.
For the reaction
2NO(g)+O2(g)↽−−⇀2NO2(g)
the standard change in Gibbs free energy is Δ𝐺°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are 𝑃NO=0.150 atm , 𝑃O2=0.350 atm , and 𝑃NO2=0.900 atm ?
Δ𝐺=
TOOLS
x10y
kJ/mol
1 Answer
- hcbiochemLv 75 days ago
ΔG = Δ𝐺° + RT ln (PNO2)^2 / (PNO)^2 PO2
Δ𝐺 = -72.6 kJ/mol + (8.314 J/molK) (298K) ln (0.900)^2 / (0.150)^2 (0.350)
Δ𝐺 = -61.1 kJ/mol