The Haber reaction for the manufacture of ammonia is N2 + 3H2 ---> 2NH3. Which of the followng are true?

A) Reaction rate = - D[N2]/Dt.


B) The reaction is first order in N2.


C) Disappearance rate of H2=3 (Disappearance rate of N2).


D) Disappearance rate of N2=3 (Disappearance rate of H2).


E) D[H2]/Dt will have a positive value.


F) The reaction is not an elementary reaction.


G) The activation energy is positive.The Haber reaction for the manufacture of ammonia is N2 + 3H2 ---%26gt; 2NH3. Which of the followng are true?
you can't really answer rate questions without a table to show how varying the concentration will affect rate. However, I do know that E is false and I don't know what you would define as an elementary process, but it can be quite complex in the sense that you must apply a great deal of heat and pressure in order to break the N2 bonds. Adding heat alone would shift the equilibrium to the left since the process is exothermic which is why you need to add pressure: to shift it back to the right. Because you must add heat and pressure to this process, the activation energy is positive.