the equilibrium constant Kc is 0.83 at 400 C for thefollowing reaction: 2NH 3 (g
ID: 682929 • Letter: T
Question
the equilibrium constant Kc is 0.83 at 400 C for thefollowing reaction: 2NH3 (g) N2 (g) + 3H2 (g) 14.6 g of ammonia is placed in a sealed 4.00 L flask. Theflask is then heated to 400 C. calculate the concentrations of allthe gases once the system reaches equilibrium. the equilibrium constant Kc is 0.83 at 400 C for thefollowing reaction: 2NH3 (g) N2 (g) + 3H2 (g) 14.6 g of ammonia is placed in a sealed 4.00 L flask. Theflask is then heated to 400 C. calculate the concentrations of allthe gases once the system reaches equilibrium.Explanation / Answer
Number of moles of Ammonia = 14.6 g / 17.031 g / mol = 0.8572 moles Initial concentration of Ammonia = 0.8572 moles / 4.00 L = 0.2143 M Kc = 0.83 2NH3 (g) N2 (g) + 3H2 (g) I(M) 0.2143 0 0 C(M) -2x +x +3x E(M) 0.2143 - 2x +x +3x Kc = [N2 ][H2]3 /[NH3 ]2 0.83 = ( x )(3x )3 /( 0.2143 - 2x)2 ( x )(3x )3 -0.83 ( 0.2143 -2x)2 = 0 On solving above equation we get x = 0.086 M At equilibrium : [NH3] = 0.2143 M - 2 * 0.086 M = 0.0423 M [N2] = 0.086M [H2 ] = 0.258M On solving above equation we get x = 0.086 M At equilibrium : [NH3] = 0.2143 M - 2 * 0.086 M = 0.0423 M [N2] = 0.086M [H2 ] = 0.258MRelated Questions
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