# What is #K_(eq)# for the reaction #N_2 + 3H_2 rightleftharpoons 2NH_3# if the equilibrium concentrations are #[NH_3] = 3 M#, #[N_2] = 2 M#, and #[H_2] = 1 M#?

##### 1 Answer

Apr 6, 2017

Use the definition of

#K_(eq) = (["products"]^(d,e,f, . . . ))/(["reactants"]^(a,b,c,. . . ))#

#= (["NH"_3]_(eq)^2)/(["H"_2]_(eq)^3["N"_2]_(eq))#

Just make sure you remember to use stoichiometric coefficients correctly.

Now, plug in your concentrations and evaluate. Are they or are they not already equilibrium concentrations?