5 3 dynamic equilibria

The equation for the production of ammonia that takes place in the Haber process is: N2 (g) + 3H2 (g) ⇌ 2NH3 (g)

True. The formation of ammonia is exothermic.

False. A catalyst does not affect the position of equilibrium, only the rate at which it is reached.

A higher pressure would increase the rate at which equilibrium is reached, as there are more successful collisions.

A higher temperature would increase the rate at which equilibrium is reached, as the particles have greater kinetic energy.

True. Cooling an exothermic reaction results in the equilibrium shifting in the exothermic direction to produce more heat and raise the temperature.

Iron is used as a catalyst in the Haber process

The conditions used in the Haber process are described as a compromise as, they are not ideal in terms of yield, but provide a balance between product yield, reaction rate, and production cost.

Nitrogen and hydrogen are extracted from:

Increasing pressure results in the equilibrium shifting to the side with the fewer gas molecules to decrease the gas pressure.

A fertiliser is a compound containing nutrients that is applied to soil or plants to promote growth and increase crop yields.

The three essential elements in fertilisers are nitrogen, phosphorus, and potassium.

The ammonium ion is NH4+.

Nitrate ions (NO3-) are a source of soluble nitrogen in fertilisers.

The formula of the phosphate ion is PO43-.

False. Most common potassium compounds dissolve in water to produce potassium ions (K+), which are a component of fertilisers.

The balanced symbol equation is: NH3 (aq) + HNO3 (aq) → NH4NO3 (aq)

Plants require nitrogen, potassium and phosphorus because:

The Haber process produces ammonia industrially.

Sulfuric acid is sprayed into a chamber of ammonia gas to form ammonium sulfate.

The steps used in the laboratory to form ammonium sulfate are: