Calculate the equilibrium constant at 500 K for the following reaction given the data below. N₂(g) + 3H₂(g) 2NH₃(g) K_c(298 K) = 6.1 *10⁵ $\Delta$ G (NH₃,g) = -16.5 kJ/mol $\Delta$ H (NH₃,g) = -46.1 kJ/mol

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The Answer of Calculate the equilibrium constant at 500 K for the following reaction given the data below. N₂(g) + 3H₂(g) 2NH₃(g) K_c(298 K) = 6.1 *10⁵ $\Delta$ G (NH₃,g) = -16.5 kJ/mol $\Delta$ H (NH₃,g) = -46.1 kJ/mol

Calculate the Equilibrium Constant at 500 K for the Following Δ\DeltaΔ

Calculate the Equilibrium Constant at 500 K for the Following $\Delta$