Discover a wealth of knowledge at Westonci.ca, where experts provide answers to your most pressing questions. Get detailed and precise answers to your questions from a dedicated community of experts on our Q&A platform. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently.
Sagot :
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.
(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.
We hope our answers were helpful. Return anytime for more information and answers to any other questions you may have. We hope our answers were useful. Return anytime for more information and answers to any other questions you have. We're glad you chose Westonci.ca. Revisit us for updated answers from our knowledgeable team.