Problem: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2 (g) + 3H2 (g) ⇌ 2NH3 (g) the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are PN2 = 0.250 atm, PH2 = 0.400 atm, and PNH3 = 0.850 atm

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For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 

N2 (g) + 3H2 (g) ⇌ 2NH3 (g) 

the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are

 PN2 = 0.250 atm, PH2 = 0.400 atm, and PNH3 = 0.850 atm


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