Note the correct spelling of Celsius.
I have rewritten the equation to show the heat better, like this,
N2(g)+3H2(g)⇌2NH3(g) + heat
Here are the answer choices:
a.adding more catalyst
b.increasing the pressure to 400atm
c.increasing the temperature to1000degree celcius
d.using air rather than nitrogen
a. adding catalyst doesn't change the equilibrium.
b. There are 4 mols gas on the left and 2 mols gas on the right so increasing pressure will shift the equilibrium to the right so as to occupy a smaller volume and that produces more product which is what you want..
c. Increasing T will shift the equilibrium to the left. You don't want that.
d. Decreasing amount of N2 shifts the equilibrium to the left. You don't want that.
Make sure you understand all of this.
Ammonia is manufactured on a large scale by the Haber's process. .In a particular plant,conditions of 400degreeC and 250atm in the presence of an iron catalyst are used.
N2(g)+3H2(g)⇌2NH3(g) deltaH=-92Kjmol^-1
What would contribute most to increasing the equilibrium yield of ammonia?
a.adding more catalyst
b.increasing the pressure to 400atm
c.increasing the temperature to1000degree celcius
d.using air rather than nitrogen
1 answer
1 answer