discuss the application of Le chatelier principle by Haber's process
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Le chatelier principle :
If a system of equilibrium is subjected to the change of pressure, temperature or concentration ,the system is shifted In such a way that to nullify the effect of change
Haber's process :
In this process nitrogen and hydrogen combines together to form ammonia
ex: N2+ 3 H2«- - - - -» 2 NH3 +92.1KJ
Effect of concentration :
If the concentration of N2,H2 or both Increases or conc of the NH3 decreases then the forward reaction takes place more favourably and yields higher amount of ammonia
Effect of temperature :
The formation of ammonia is exothermic reaction low temperature favours the forward reaction. But at low temperature the reaction is too slow. But at low temperature the reaction.Therefore an optimum temperature is chosen in Haber process
Effect of pressure :
In the forward reaction 1 volume of N2 and 3 Volumes of H2 to form 2 volumes of NH3 . There is decrease in volume of the forward reaction. according to le -chatelier principle increase of pressure favours the forward reaction where there is a decrease in volume. So higher the pressure are used in the manufacture of ammonia by Haber process
Optimum conditions :
Pressure :200 atm
temperature : 725-775 k
catalyst : Fe (powered)
Promoter : Mo or (K2O+ Al2O3)
Answer:
Le Chatelier's principle can be used to predict the behavior of a system due to changes in pressure, temperature, or concentration. Le Chatelier's principle implies that the addition of heat to a reaction will favor the endothermic direction of a reaction as this reduces the amount of heat produced in the system.A worked example using Le Chatelier's principle to predict how concentrations will shift for different perturbations. Example includes changing reaction vessel volume, changing amount of solid product, adding inert gas, and adding a catalyst.