For the reaction
C2H6(g)+H2(g)↽−−⇀2CH4(g)
the standard change in Gibbs free energy is Δ????°=−32.8 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ????C2H6=0.100 atm , ????H2=0.450 atm , and ????CH4=0.700 atm ?
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species.?
2020-08-04 9:10 am
回答 (1)
2020-08-04 10:07 am
C₂H₆(g) + H₂(g) ⇌ 2CH₄(g)
ΔG
= ΔG° + RT ln{????CH₄²/(????C₂H₆ × ????H₂)}
= -32.8 + (8.314 × 10⁻³) × 298 × ln{0.700²/(0.100 × 0.450) kJ/mol
= -26.9 kJ/mol
ΔG
= ΔG° + RT ln{????CH₄²/(????C₂H₆ × ????H₂)}
= -32.8 + (8.314 × 10⁻³) × 298 × ln{0.700²/(0.100 × 0.450) kJ/mol
= -26.9 kJ/mol
收錄日期: 2021-04-18 18:36:38
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20200804011046AAR94za