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A chemistry student needs to calculate the equilibrium constant (Kc) for the reaction below at a certain temperature: N2(g) + 3H2(g) ⇌ 2NH3(g)Given the initial concentrations of N2, H2, and NH3 are 0.25 M, 0.1 M, and 0.1 M respectively, what is the value of Kc for this reaction at the given temperature?

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To calculate the equilibrium constant  Kc  for the reaction, we first need to determine the changes in the concentrations of the reactants and products at equilibrium. Let's denote the change in concentration as x.At equilibrium, the concentration of N2 will decrease by x, the concentration of H2 will decrease by 3x, and the concentration of NH3 will increase by 2x.N2: 0.25 - xH2: 0.1 - 3xNH3: 0.1 + 2xNow, we can write the expression for Kc:Kc = [NH3]^2 /  [N2] * [H2]^3 Plug in the equilibrium concentrations:Kc = [ 0.1 + 2x ^2] /  [ 0.25 - x  *  0.1 - 3x ^3] Unfortunately, we cannot solve for Kc without more information, such as the equilibrium concentrations or the temperature and the standard Gibbs free energy change  G  of the reaction. If you have any of these additional pieces of information, we can proceed to calculate Kc.

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