Oxides of Carbon - CO and CO2 - UNSOLVED PRACTICE SET
Chapter: p-Block Elements Groups 13 and 14 | Topic: Oxides of Carbon CO and CO2
OXIDES OF CARBON - CO AND CO2 - UNSOLVED PRACTICE SET
Topic: Oxides of Carbon CO and CO2
Multiple Choice Questions
Q1. Carbon monoxide (CO) is prepared in the laboratory by:
- Heating calcium carbonate
- Dehydration of formic acid with concentrated H₂SO₄
- Passing CO₂ over heated carbon
- Heating oxalic acid
Q2. Carbon dioxide (CO₂) is a gas at room temperature, while silicon dioxide (SiO₂) is a solid because:
- CO₂ has a higher molecular mass
- CO₂ exists as discrete molecules with weak intermolecular forces
- CO₂ has stronger covalent bonds
- CO₂ is more polar
Q3. Carbon monoxide is poisonous because it:
- Reacts with oxygen in the blood
- Forms a stable complex with haemoglobin, preventing oxygen transport
- Dissolves in blood plasma
- Destroys red blood cells
Q4. When CO₂ is passed through lime water, it first turns milky and then clear on excess CO₂. This is because:
- CaCO₃ is formed first, then soluble Ca(HCO₃)₂
- Ca(OH)₂ is formed first, then CaCO₃
- Ca(HCO₃)₂ is formed first, then CaCO₃
- No reaction occurs with excess CO₂
Q5. Carbon monoxide acts as a reducing agent in the extraction of iron because:
- It oxidises iron oxide to iron
- It reduces iron oxide to iron, getting oxidised to CO₂
- It acts as a catalyst
- It provides heat for the reaction
Q6. Dry ice is:
- Frozen water
- Solid carbon dioxide
- Solid carbon monoxide
- A mixture of CO₂ and water
Short Answer Questions
Q7. Write balanced chemical equations for the laboratory preparation of:
(a) Carbon monoxide from oxalic acid
(b) Carbon dioxide from calcium carbonate
Q8. Why is carbon monoxide called a "reducing agent"? Give one industrial application where CO is used as a reducing agent.
Q9. Explain the structure of carbon monoxide (CO) molecule. How does it form a coordinate bond with haemoglobin?
Q10. Why does CO₂ not support combustion, yet magnesium continues to burn in CO₂? Write the relevant chemical equation.
Q11. Your family uses a gas geyser for heating water during Delhi winters. The instruction manual warns about ensuring proper ventilation. Explain the chemical reason behind this warning.
Q12. How does carbon dioxide help in fire extinguishers? Why is it more effective than water for electrical fires?
Long Answer Questions
Q13. Compare the properties and structures of carbon monoxide (CO) and carbon dioxide (CO₂):
(a) Molecular structure and bond lengths
(b) Physical state and solubility in water
(c) Nature as acidic oxide (CO₂) vs. neutral oxide (CO)
(d) Reducing nature of CO vs. oxidising nature of CO₂
(e) Reaction with haemoglobin (CO) vs. photosynthesis (CO₂)
Write balanced chemical equations for relevant reactions.
Q14. Discuss the environmental impact of carbon dioxide and carbon monoxide:
(a) The role of CO₂ as a greenhouse gas and its contribution to global warming
(b) Sources of CO₂ emissions in India (thermal power plants, vehicles, industries)
(c) The dangers of CO poisoning and why it is called a "silent killer"
(d) Measures to reduce CO and CO₂ emissions in Indian cities
Q15. Carbon dioxide has both harmful and beneficial effects on our planet. Discuss:
(a) The role of CO₂ in photosynthesis and why it is essential for life
(b) How CO₂ is used in the food industry (carbonated drinks, fire extinguishers, refrigeration)
(c) The process of carbon capture and storage (CCS) being explored in India
(d) Why India's pledge at COP26 to achieve net-zero emissions by 2070 requires managing CO₂ levels
Numerical / Application-Based Problems
Q16. In the extraction of iron in a blast furnace, the reduction of Fe₂O₃ occurs mainly through carbon monoxide:
Fe₂O₃ + 3CO → 2Fe + 3CO₂
(a) Calculate the mass of CO required to reduce 160 kg of Fe₂O₃ completely.
(b) Calculate the mass of iron produced and the volume of CO₂ evolved at STP.
(c) If the blast furnace operates at 80% efficiency, calculate the actual mass of CO needed.
[Given: Atomic masses: Fe = 56, C = 12, O = 16; Molar volume at STP = 22.4 L]
Q17. A car in a closed garage produces carbon monoxide. The garage has a volume of 50 m³ (50,000 L). The car engine produces CO at a rate of 0.5 L per minute at STP.
(a) Calculate the concentration of CO in ppm (parts per million) after 30 minutes. Assume uniform mixing.
(b) The lethal concentration of CO is about 1600 ppm. Calculate how long it would take to reach this concentration.
(c) Why is CO particularly dangerous compared to other poisonous gases?
Q18. In a photosynthesis experiment, a plant is exposed to 44 g of CO₂.
(a) Write the balanced equation for photosynthesis.
(b) Calculate the mass of glucose (C₆H₁₂O₆) produced if all the CO₂ is utilised.
(c) Calculate the volume of O₂ released at STP during this process.
[Given: Atomic masses: C = 12, H = 1, O = 16; Molar volume at STP = 22.4 L]