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(c) Ammonia reacts with oxygen at high temperatures in the presence of a suitable catalyst to form nitric oxide, NO.
[tex]\[
4 NH_3(g) + 5 O_2(g) \rightarrow 4 NO(g) + 6 H_2O(g)
\][/tex]

(i) Explain how this chemical equation shows ammonia acting as a reducing agent.
[tex]\[\qquad \][/tex]
[1]

(ii) Suggest a suitable catalyst for the reaction from the list of metals. Give a reason for your answer.
- aluminium
- calcium
- platinum
- potassium
- sodium

Suitable catalyst: [tex]\[\qquad \][/tex]
Reason: [tex]\[\qquad \][/tex]
[2]

Sagot :

GinnyAnswer
Let's break down the problem step-by-step:

(i) Explain how this chemical equation shows ammonia acting as a reducing agent.

The given chemical reaction is:
[tex]\[ 4 \text{NH}_3(\text{g}) + 5 \text{O}_2(\text{g}) \rightarrow 4 \text{NO}(\text{g}) + 6 \text{H}_2\text{O}(\text{g}) \][/tex]

In this reaction, ammonia ([tex]\(\text{NH}_3\)[/tex]) is transforming into nitric oxide ([tex]\(\text{NO}\)[/tex]).

- As [tex]\(\text{NH}_3\)[/tex] is converted to [tex]\(\text{NO}\)[/tex], it loses hydrogen atoms and gains oxygen atoms.
- Losing hydrogen atoms and gaining oxygen atoms indicates that ammonia is being oxidized.
- Oxidation is the process where a substance loses electrons.
- In a redox (reduction-oxidation) reaction, the substance that is oxidized acts as a reducing agent, as it donates electrons to another substance.

Therefore, ammonia ([tex]\(\text{NH}_3\)[/tex]) acts as a reducing agent in this reaction because it donates electrons (gets oxidized) in the process.

(ii) Suggest a suitable catalyst for the reaction from the list of metals. Give a reason for your answer:

List of metals: aluminium, calcium, platinum, potassium, sodium

Suitable catalyst: Platinum

Reason: Platinum is highly efficient and stable in various chemical environments. It is commonly used as a catalyst in chemical reactions due to its ability to increase the reaction rate without being consumed in the process. Its high efficiency and stability make it a suitable choice for facilitating the reaction between ammonia and oxygen to produce nitric oxide and water.
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