In the haber process, it is true the higher the pressure , the more favourable the foward reaction is?
Answer:
It's true that the higher the pressure, the higher the yield of ammonia. However, if it was carried out at a high pressure, it would take absolutely ages for the reaction to reach a dynamic equilibrium. Initially, there would be a high yield of ammonia but after a while, that would decrease dramatically until the dynamic equilibrium was reached.
Haber reaction:
3H2(g) + N2(g) ---> 2NH3(g)
Now Le Chatelier's principle states that the the position of equilibrium will shift in favour of the reaction which counteracts any change to the system. So if we increase the pressure, the system will act to decrease it, so the reaction which produces fewer gas molecules (in this case the forward one) increases.
So yes, increase in pressure does favour the forward reaction.
Here ya go...
"increasing the pressure causes the equilibrium position to move to the right"
http://www.ausetute.com.au/haberpro.html...
Hope I have helped...
Ron.
Haber's reaction:
N2 + 3H2 = 2NH3
total no of moles of reactants = 3+1= 4
total no of moles of product = 2
there's a contraction of vol in the forward rxn (Δn= -2)
=> according to La chatelier's principle the forward rxn is favored by high pressure.
=> higher the pressure, the more favorable the forward reaction is,
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