Discuss the favourable conditions of concentration, pressure, and temperature on the Haber's process, in manufacture of ammonia.
N2(g) + 3H2(g) --> 2NH3(g); AH = -92.5KJ
in between Kp and Kc.
Answers
concentration of NH3 increase the concentration of product so the reaction which shift towards reactant side means backward reaction so for increasing then production of NH3 we have to decrease the concentration of reactants affect which means N2 and H2
if you are talking about pressure we need high pressure cause if you use high pressure the reaction was shifted towards the lower moles side which means towards product side so production of NH3 will enhanced pressure of 200 to 300 atmosphere is required
low temperature is required for it because it is an exothermic reaction as temperature decreases reaction will move towards products side means forward reaction but it low temperature the reaction is so we need optimum temperature of 725 to 775 Kelvin
if you like the answer plz make me brainliest this is my own and correct answer