the Haber process. Flashcards
a mixture of chemicals are present in a closed system at dynamic equilibrium
A+B ⇌ C.
-describe what is happening when the mixture is at dynamic equilibrium.
-what is a closed system?
reversable reaction carried out in a closed container so the reactants and products can’t escape.
A+B ⇌ C.
in certain conditions the position of equilibrium lies to the right.
-explain what this means?
more of C than A+B.
Co₂ (g) + 3H₂ (g) ⇌ CH₃OH (g) + H₂O (g)
if the steam is removed from the equilibrium mixture what happens to the equilibrium yield of menthol?
-explain.
more menthol.
equilibrium position moves right to replace steam.
CH₄ (g) + H₂O (g) ⇌ CO (g) + 3H₂O(g) energy change: +200kj/mol.
-if the temp of equilibrium is increased what would happen to equilibrium yield of hydrogen?
-explain.
more hydrogen.
equilibrium moves to the right in an endothermic reaction to decrease the temp.
CH₄ (g) + H₂O (g) ⇌ CO (g) + 3H₂O(g) energy change: +200kj/mol.
if the pressure of this equilibrium was increased what would happen to the equilibrium yield of hydrogen?
-explain.
less hydrogen.
equilibrium moves left. less gas molecules to decrease pressure.
what can be made in this process?
ammonia.
what is the formula for ammonia?
nitrogen + hydrogen ⇄ ammonia.
N₂ (g) +3H₂ (g) ⇄ 2NH₃ (g)
what catalyst is used?
iron.
why is a catalyst used?
increase rate of reaction.
what happens to the percentage of ammonia as the pressure is increased?
increases.
what happens to the percentage of ammonia as the temperature is increased?
decreases.
why are unreacted gases recycled?
prevents waste.
more ammonia is made if the temperature is 350c. why don’t manufactures use this temperature to make ammonia?
slower rate of reaction.
more ammonia is made if the pressure is higher. why don’t manufactures use a higher pressure of 200 atmospheres?
difficult to contain, requires a lot of energy and very expensive.
what can ammonia be used to make?
fertiliser.
