[mr cool]

Are my answers correct?

First Question...

  N_2(g)  +  3H_2(g) 2NH _3(g)  its got the same balanced equation for all 4 questions by the way

[H₂]₀ = 2.0 x 10^-3 M
[N₂]₀ = 1.0 x 10^-5 M                               [1.0 x 10^-3]²                  = 1 x 10 ^-6  = 1.25 x 10 -7  which means the reaction needs to go ------->
[NH3]₀ = 1.0 x 10^-3 M                       [2.0 x 10^-3]³[1.0 x 10^-5]          8 x 10 ^-14
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Second Question

[H₂]₀ = 3.54 x 10^-1 M
[N₂]₀ = 1.50 x 10^-5 M              [2.00 x 10] ²                 = 1.18 x 10^-4  Rxn goes ----->
[NH3]₀ = 2.0 x 10^-4 M      [1.50 x 10^-5][3.54 x 10^-1]³


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#3

[H₂]₀ = 1.0 x 10^-2 M
[N₂]₀ = 5.0 M                                          = [1.0 x 10^-4]²                   = 2 x 10^-2
[NH3]₀ = 1.0 x 10^-4 M                               [5.0][1.0 x 10^-2]³                  Rxn goes -------> to balance

[Borek]

You have to be more precise about the data and the question, as they are presented now I have no idea what is going on.

[mr cool]

You have to be more precise about the data and the question, as they are presented now I have no idea what is going on.

Description on the homework....  For each of the following conditions of the Haver-Bosch process, determine if the scenario is at equilibrium OR which direction the reaction will proceed to each equilibrium.  If the concentrations are taken at 500 ^oC where the reaction has an equilibrium constant of 6.02 x 10^-2