In the haber process for the preparation of NH3 which is given by the equilibruim?
N_2_(g)+3H_2_(g) <---> 2NH_3_(g)...... delta H= -92.38kJ
State the conditions of concentrations and temperture that will favor production of NH_3_?

Please help! would it be high tempertures? or am I wrong? please explain why cause I'm lost!

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  1. First, most everyone here recognizes that subscripts are a problem so we write it as
    N2(g) + 3H2(g( ==> 2NH3(g) + heat
    and keep in mind that numbers before the element are coefficients and numbers after the element are subscripts.
    This problem is one on Le Chatelier's Principle.
    To favor the production of NH3, we want the reaction to go to the right as much as possible. So we increase (N2) and/or (H2), decrease (NH3) as it is produced, and keep temperature low. Increasing pressure favors production of NH3 also.
    Note: Remember Le Chatelier's Principle says that a reaction at equilibrium will try to UNDO what we do to it. So increasing temperature, as you suggest, would try to use up the added heat so the reaction would shift to the left (look at my equation above to see that) and that will DECREASE NH3. See also that adding N2 and/or H2 will try to use up the added N2 and H2 and that means more NH3 production. For pressure, the reaction shifts to the side with fewer mole when increasing P. There are 4 moles of gas on the left and 2 on the right so increasing P moves to more NH3 by shifting to the right. A rather long explanation and somewhat repetitious in spots but I hope this helps.

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  2. how to find reagents need to dissolve a chemical in a system? If I have a equilibrium equation would I use the chemical on the product side or reactant side to dissolve a compound.

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  3. You may be referring to the SbCl3 post which I answered just a second ago.

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