Question

The Haber process is used to make ammonia, N2(g) + 3H2(g) = 2NH3(g) a) Write down the condition for equilibrium for this reaction in terms of the concentrations of reactants and products. At 298 K, this reaction has AH° = -46 kJ mol"', and AS° = -100 J K-mol?. Assume that AH° and ASº are independent of temperature. At what temperature does AGº vanish, i.e. AG° = 0? (c) Under practical industrial conditions the equilibrium constant for this reaction is: Kc = 0.08 M2. The concentrations at equilibrium of N2(g) and H2(g) are, respectively, 0.821 M and 0.663 M. What is the concentration of NH3(g)? (d) Are there more microstates available to the atoms of the reactants (i.e. 1 mol N2(g) and 3 mol of H2(g)) or to the atoms in the products (i.e. 2 mol of NH3(g))? You may assume the volume does not change for this part only. Explain your reasoning.

only do part (c) **please explain how to solve M^-2

Answer 1

The equilibrium constant for the given reaction is given by Kc = [NH3]^2 /[N2][H2]^3

M^-2 represents unit of NC, no need to solve it.

0.08 = [NH3]^2 /(0.821*(0.663)^3)

The concentration of NH3 is 0.138 M