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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) = 2NH₂(g) the standard change in Gibbs free energy is AG° = -69.0 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.250 atm, PH₂ = 0.200 atm, and PNH, = 0.900 atm? AG= kJ/mol 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) ⇒ 2 NH3(g) the standard change in Gibbs free energy is AG° = -69.0 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.400 atm, and PNH₂ = 0.800 atm? AG= kJ/mol