The Haber-Bosch process is used to convert nitrogen and hydrogen into ammonia.
Which raw material is the standard industrial source of the hydrogen?
Gases used and produced in these chemical industries undergo several reversible reactions.
Reaction 1:
N2(g)+3H2(g)⇌2NH3(g)ΔH=−92 kJ mol−1 \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) \quad \Delta H = -92 \text{ kJ mol}^{-1} N2(g)+3H2(g)⇌2NH3(g)ΔH=−92 kJ mol−1Reaction 2:
N2(g)+O2(g)⇌2NO(g)ΔH=+180 kJ mol−1 \text{N}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{NO}(\text{g}) \quad \Delta H = +180 \text{ kJ mol}^{-1} N2(g)+O2(g)⇌2NO(g)ΔH=+180 kJ mol−1Predict what will happen to the equilibrium position in Reaction 1 when the pressure is increased. Give a reason for your prediction. Prediction: Reason:
Predict what will happen to the equilibrium position in Reaction 2 when the temperature is increased. Give a reason for your prediction. Prediction: Reason:
Predict what will happen to the rate of Reaction 1 when the pressure and temperature are increased. Effect of increased pressure: Effect of increased temperature:
Some of the ammonia is made into nitrogen-rich fertilizers such as ammonium sulfate.
The equation for the formation of ammonium sulfate is:
2NH3+H2SO4→(NH4)2SO4 2\text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow (\text{NH}_4)_2\text{SO}_4 2NH3+H2SO4→(NH4)2SO4A manufacturer makes a batch of 66 kg of ammonium sulfate.
Calculate the amount, in moles, of (NH4)2SO4(\text{NH}_4)_2\text{SO}_4(NH4)2SO4 in 66 kg of ammonium sulfate. Amount of (NH4)2SO4(\text{NH}_4)_2\text{SO}_4(NH4)2SO4: _________ mol\text{mol}mol
Deduce the amount, in moles, of ammonia needed to make this amount of ammonium sulfate. Amount of ammonia: _________ mol\text{mol}mol
Calculate the mass, in kg, of ammonia needed. Mass of ammonia: _________ kg\text{kg}kg
Multi-nutrient fertilizers are often labelled with an NPK rating. Suggest the names of two elements, other than nitrogen, represented by these letters that are essential for plant growth.
