The equilibrium constant at 427°C for the reactionN 2 (g)+ 3H 2 (g) 2NH 3 (g)is K p = 9.4 × 10 -5 . Calculate the value of $\Delta$G° for the reaction at this temperature.

The Answer of The equilibrium constant at 427°C for the reactionN 2 (g)+ 3H 2 (g) 2NH 3 (g)is K p = 9.4 × 10 -5 . Calculate the value of $\Delta$G° for the reaction at this temperature.

The equilibrium constant at 427°C for the reactionN 2 (g)+ 3H 2 (g) 2NH 3 (g)is K p = 9.4 × 10 -5 . Calculate the value of $\Delta$G° for the reaction at this temperature.

The Answer of The equilibrium constant at 427°C for the reactionN 2 (g)+ 3H 2 (g) 2NH 3 (g)is K p = 9.4 × 10 -5 . Calculate the value of $\Delta$G° for the reaction at this temperature.

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The Equilibrium Constant at 427°C for the ReactionN₂(g)+ 3H₂(g) $\Delta$ G° for the Reaction at This Temperature

Question 60

Multiple Choice

The equilibrium constant at 427°C for the reactionN₂(g) + 3H₂(g) $The equilibrium constant at 427°C for the reactionN2(g) + 3H2(g) 2NH3(g) is Kp = 9.4 × 10-5. Calculate the value of \Delta G° for the reaction at this temperature. A) 56 kJ/mol B) -56 kJ/mol C) -33 kJ/mol D) 33 kJ/mol E) 1.3 J/mol$ 2NH₃(g) is K_p = 9.4 × 10^-5. Calculate the value of $\Delta$ G° for the reaction at this temperature.