Ammonium nitrate is a commonly used fertiliser - Scottish Highers Chemistry - Question 6 - 2023
Question 6
Ammonium nitrate is a commonly used fertiliser.
(a) (i)
Ammonium nitrate is made industrially by adding nitric acid, HNO₃, to ammonia, NH₃.
HNO₃(aq) + NH₃(g) ⇌ NH... show full transcript
Worked Solution & Example Answer:Ammonium nitrate is a commonly used fertiliser - Scottish Highers Chemistry - Question 6 - 2023
Step 1
Complete the diagram to show the shape of the enthalpy diagram for this reaction.
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Answer
The enthalpy diagram should show a curve that starts at the energy level of the reactants and rises up to a peak at the activation energy (X), then falls down to a lower energy level at the products. This represents an exothermic reaction where the products have lower potential energy than the reactants.
Step 2
State the term for the unstable arrangement of atoms formed at the point labeled X on the potential energy diagram above.
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Answer
Activated complex.
Step 3
Suggest a reason why the method shown in part (a)(ii) is the preferred industrial route.
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The method has 100% atom economy and produces only one product, making it more efficient and cost-effective than alternative methods.
Step 4
Suggest what is represented by the area under the curve in Graph 1.
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The area under the curve in Graph 1 represents the total number of molecules or particles in the gas mixture.
Step 5
Add a second curve to Graph 1 to show the distribution of kinetic energies at a higher temperature.
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The second curve should be displaced to the right of the original curve, indicating that at a higher temperature, there are more molecules with greater kinetic energy.
Step 6
Draw a line to show how a catalyst affects the activation energy, EⱣ.
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Draw a vertical line at a lower kinetic energy than the original EⱣ, indicating that a catalyst lowers the activation energy required for the reaction.
Step 7
State what is meant by the term dynamic equilibrium.
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Answer
Dynamic equilibrium occurs in a reversible reaction when the rate of the forward reaction equals the rate of the reverse reaction, and the concentrations of reactants and products remain constant.
Step 8
Explain how this will affect the production of ammonia.
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Removing ammonia continuously will shift the equilibrium to the right, according to Le Chatelier's principle, increasing the yield of ammonia produced.
Step 9
State another way that the manufacturing process maximises profit or minimises the impact on the environment.
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Recycling unreacted gases or using a catalyst can reduce costs and minimize environmental impact in the Haber process.
Step 10
Write the overall redox equation for the reaction taking place in the fuel cell.
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The overall redox equation is:
ightarrow N_2 + 6H_2O$$
Step 11
Identify the reducing agent in the reaction taking place in the fuel cell.
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Ammonia (NH₃) is the reducing agent in the reaction.
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