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Carbon and hydrogen are detected by heating the compound with ____________ during quantitative analysis.
- a)Carbon dioxide
- b)Copper (II) oxide
- c)Magnesium oxide
- d)Sulphur dioxide
Correct answer is option 'B'. Can you explain this answer?
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Carbon and hydrogen are detected by heating the compound with ________...
Introduction
In quantitative analysis, specifically for determining the amounts of carbon and hydrogen in organic compounds, the choice of reagents is crucial.
Why Copper (II) Oxide?
- Reactivity: Copper (II) oxide (CuO) is a strong oxidizing agent. When heated with an organic compound, it effectively reacts with carbon and hydrogen present in the sample.
- Combustion Process: The process involves the complete combustion of the organic compound:
- Carbon is oxidized to carbon dioxide (CO2).
- Hydrogen is oxidized to water (H2O).
Formation of Products
- Quantification: The amounts of CO2 and H2O produced can be measured:
- The mass of CO2 formed indicates the amount of carbon in the original sample.
- The mass of water formed indicates the amount of hydrogen.
Advantages of Using Copper (II) Oxide
- Efficiency: CuO ensures complete combustion, which is essential for accurate quantitative analysis.
- Controlled Reaction: The reaction can be controlled well, minimizing side reactions that could impact results.
Other Options Considered
- Carbon Dioxide (a): This is a product of combustion, not a reagent.
- Magnesium Oxide (c): While it can oxidize, it is less effective than CuO for this specific analysis.
- Sulfur Dioxide (d): This is not an oxidizing agent and does not facilitate the combustion of carbon and hydrogen.
Conclusion
In quantitative analysis, copper (II) oxide is the preferred reagent for detecting carbon and hydrogen due to its strong oxidizing properties and the reliability of the combustion process it facilitates.
In quantitative analysis, specifically for determining the amounts of carbon and hydrogen in organic compounds, the choice of reagents is crucial.
Why Copper (II) Oxide?
- Reactivity: Copper (II) oxide (CuO) is a strong oxidizing agent. When heated with an organic compound, it effectively reacts with carbon and hydrogen present in the sample.
- Combustion Process: The process involves the complete combustion of the organic compound:
- Carbon is oxidized to carbon dioxide (CO2).
- Hydrogen is oxidized to water (H2O).
Formation of Products
- Quantification: The amounts of CO2 and H2O produced can be measured:
- The mass of CO2 formed indicates the amount of carbon in the original sample.
- The mass of water formed indicates the amount of hydrogen.
Advantages of Using Copper (II) Oxide
- Efficiency: CuO ensures complete combustion, which is essential for accurate quantitative analysis.
- Controlled Reaction: The reaction can be controlled well, minimizing side reactions that could impact results.
Other Options Considered
- Carbon Dioxide (a): This is a product of combustion, not a reagent.
- Magnesium Oxide (c): While it can oxidize, it is less effective than CuO for this specific analysis.
- Sulfur Dioxide (d): This is not an oxidizing agent and does not facilitate the combustion of carbon and hydrogen.
Conclusion
In quantitative analysis, copper (II) oxide is the preferred reagent for detecting carbon and hydrogen due to its strong oxidizing properties and the reliability of the combustion process it facilitates.
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Community Answer
Carbon and hydrogen are detected by heating the compound with ________...
During quantitative analysis, a known quantity of the organic compound is burned in the presence of excess of oxygen and copper (II) oxide. The carbon present in the compound is oxidized to carbon dioxide and the hydrogen is transformed to water.
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Carbon and hydrogen are detected by heating the compound with ____________ during quantitative analysis.a)Carbon dioxideb)Copper (II) oxidec)Magnesium oxided)Sulphur dioxideCorrect answer is option 'B'. Can you explain this answer?
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