At equilibrium a mixture of n2, h2, nh3 gas at 500◦c is determined to consist of 0.551 mol/l of n2, 0.400 mol/l of h2, and 0.184 mol/l of nh3. what is the equilibrium constant for the reaction

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The balanced equation for the reaction is N₂(g) + 3H₂(g) ⇄ 2NH₃(g) The equilibrium constant, k for the reaction can be written as k = [NH₃(g)]² / [N₂(g)][H₂(g)]³ The given concentration are at equilibrium state. Hence, we can use those directly for the calculation. [NH₃(g)] = 0.184 mol/L [N₂(g)] = 0.551 mol/L [H₂(g)] = 0.400 mol/L By applying the formula, k = ( 0.184 mol/L)² / ((0.551 mol/L) x (0.400 mol/L)³) k = 0.960 mol⁻² L² Hence, the equilibrium constant for the reaction at 500 °C is 0.960 mol⁻² L²


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