The equilibrium constant at 427^$\circ$C for the reaction N₂(g) + 3H₂(g) $\leftrightharpoons$ 2NH₃(g) is K_p = 9.4 * 10^-5. Calculate the value of $\Delta$G^$\circ$ 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^$\circ$C for the reaction N₂(g) + 3H₂(g) $\leftrightharpoons$ 2NH₃(g) is K_p = 9.4 * 10^-5. Calculate the value of $\Delta$G^$\circ$ 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 ∘\circ∘ C for the Reaction N2(g) + 3H2(g)

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