Q.Give one method for industrial preparation and one for laboratory preparation of CO and CO2 each.

Carbon monoxide (CO)

1. Industrial preparation — producer gas. Air is passed over red-hot coke/carbon. Carbon first burns to CO$_2$, which is then reduced by more hot carbon to CO; the nitrogen from air remains as a diluent, giving "producer gas" (a mixture of CO and N$_2$), used as an industrial fuel:

2. Laboratory preparation. Formic acid (HCOOH) is dehydrated by heating with concentrated sulphuric acid, which removes water and leaves CO gas:

Carbon dioxide (CO$_2$)

3. Industrial preparation — calcination of limestone. Heating limestone (calcium carbonate) strongly in a lime kiln decomposes it to quicklime (calcium oxide) and CO$_2$ gas — this is also the basis of large-scale cement manufacture: $\text{CaCO}_3 \xrightarrow{\Delta} \text{CaO} + \text{CO}_2$ …

Recall the standard named preparations from the textbook: industrial CO via the producer-gas process (partial combustion of coke in air), laboratory CO via acid-catalysed dehydration of formic acid; industrial CO$_2$ via limekiln calcination of limestone, laboratory CO$_2$ via …

• Confusing producer gas (CO + N$_2$, from limited-air combustion of carbon) with water gas (CO + H$_2$, from steam over hot carbon) — both are valid industrial CO routes, but they must not be conflated in the same equation.
• Forgetting the dehydrating agent (conc. H$_2$SO$_4$) and heating condition in the laboratory preparation of CO from formic acid. …