The equilibrium constant at 427°C for the reaction N₂(g)+ 3H₂(g) 2NH₃(g)is K_p = 9.4 $\times$ 10^-5. Calculate the value of $\Delta$G° for the reaction under these conditions. A)-33 kJ/mol B)-54 kJ/mol C)54 kJ/mol D)33 kJ/mol E)1.3 J/mol

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The Answer of The equilibrium constant at 427°C for the reaction N₂(g)+ 3H₂(g) 2NH₃(g)is K_p = 9.4 $\times$ 10^-5. Calculate the value of $\Delta$G° for the reaction under these conditions. A)-33 kJ/mol B)-54 kJ/mol C)54 kJ/mol D)33 kJ/mol E)1.3 J/mol

The Equilibrium Constant at 427°C for the Reaction N2(g)+ 3H2(g) ×\times×

The Equilibrium Constant at 427°C for the Reaction N₂(g)+ 3H₂(g) $\times$