The flow diagram shows how ammonium nitrate is manufactured from raw materials in the Ostwald process and subsequent neutralization:
Ammonia, Air, Water→Nitrogen monoxide→Nitrogen dioxide→Nitric acid→Ammonium nitrate \text{Ammonia, Air, Water} \rightarrow \text{Nitrogen monoxide} \rightarrow \text{Nitrogen dioxide} \rightarrow \text{Nitric acid} \rightarrow \text{Ammonium nitrate} Ammonia, Air, Water→Nitrogen monoxide→Nitrogen dioxide→Nitric acid→Ammonium nitrateThe nitrogen monoxide needed can be formed by burning ammonia gas in oxygen.
Balance the equation for this reaction:
…NH3+…O2→…NO+…H2O \dots\text{NH}_3 + \dots\text{O}_2 \rightarrow \dots\text{NO} + \dots\text{H}_2\text{O} …NH3+…O2→…NO+…H2OThe equation for the catalytic oxidation of nitrogen monoxide to nitrogen dioxide (Reaction 2) is:
2NO(g)+O2(g)⇌2NO2(g)ΔH=−114 kJ/mol 2\text{NO(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)} \quad \Delta H = -114\text{ kJ/mol} 2NO(g)+O2(g)⇌2NO2(g)ΔH=−114 kJ/molAssuming that this reaction reaches equilibrium, explain what happens to the yield of nitrogen dioxide if the reaction is carried out at a higher pressure but at the same temperature.
Assuming that this reaction reaches equilibrium, explain what happens to the yield of nitrogen dioxide if the reaction is carried out at a higher temperature but at the same pressure.
Reaction 2 can be represented on an energy profile. Explain how the energy level of the products compares to the reactants and how the enthalpy change (ΔH\Delta HΔH) is shown on an energy profile diagram for this reaction.
Reaction 2 is carried out using a platinum-rhodium catalyst. State the effect, if any, of using a catalyst on the enthalpy change for the reaction.
Explain how a catalyst increases the rate of a reaction.
The equations for some of the other reactions used in this manufacturing process are:
Explain which two of these are redox reactions.
A manufacturer produces a batch of 270 kg270\text{ kg}270 kg of dinitrogen pentoxide (N2O5\text{N}_2\text{O}_5N2O5). Calculate the maximum mass of nitric acid (HNO3\text{HNO}_3HNO3) that can be made from this mass of dinitrogen pentoxide, using the overall reaction:
N2O5+H2O→2HNO3 \text{N}_2\text{O}_5 + \text{H}_2\text{O} \rightarrow 2\text{HNO}_3 N2O5+H2O→2HNO3(Relative atomic masses: H=1\text{H} = 1H=1, N=14\text{N} = 14N=14, O=16\text{O} = 16O=16). Give a unit for your answer.
