would you use co2 or co to obtain iron from iron 3 oxide?

Answer 1

You can use Carbon or Carbon monoxide to obtain Iron from Iron(III) oxide. It is possible, but with carbon dioxide, I don't think it's possible.

From the manufacture of Iron, the 3rd step in the blast furnace is carbon monoxide acting as a reducing agent, reduces Iron(III) oxide forming Iron oxide.
Equation ==> CO(g) + Fe2O3(s) ---> FeO(s) + CO2(g)

Iron can also be obtained from Iron(III) oxide by heating Iron(III) oxide with carbon. Carbon being more reactive will displace Iron from its oxide.
Equation ==> 2Fe2O3(g) + 3C(s) --> 4Fe(s) + 3CO2

I hope this helps =]

Answer 2

The previous poster is right, carbon monoxide.

Carbon monoxide is a reducing agent (which means that it can be oxidized). When you are getting iron from iron(III) oxide the oxygen atoms associated with the oxide have to go somewhere and that somewhere is converting CO to CO2.

CO2 is already fully oxidized and will not accept more oxygen (readily).

A more effective reducing agent would be pure carbon (usually supplied as coke in an iron/steel mill) because it can be oxidized even more than CO.

Hope the explanation was useful!

Answer 3

Hi,

Carbon dioxide is a chemical compound composed two oxygen atoms covalently bonded to a single carbon atom. It is a gas at standard temperature and pressure and exists in Earth's atmosphere as a gas. It is currently at a globally averaged concentration of approximately 385 ppm by volume in the Earth's atmosphere, although this varies both by location and time. Carbon dioxide's chemical formula is CO2.

In general, it is exhaled by animals and utilized by plants during photosynthesis. Additional carbon dioxide is created by the combustion of fossil fuels or vegetable matter, among other chemical processes.

Carbon dioxide is an important greenhouse gas because of its ability to absorb many infrared wavelengths of the Sun's light, and because of the length of time it stays in the Earth's atmosphere. Due to this, and the role it plays in the respiration of plants, it is a major component of the carbon cycle.

In its solid state, carbon dioxide is commonly called dry ice. Carbon dioxide has no liquid state at pressures below 5.1 atm.

Carbon dioxide is a colorless, odorless gas. When inhaled at concentrations higher than usual atmospheric levels, it can produce a sour taste in the mouth and a stinging sensation in the nose and throat. These effects result from the gas dissolving in the mucous membranes and saliva, forming a weak solution of carbonic acid. This sensation can also occur during an attempt to stifle a burp after drinking a carbonated beverage. Amounts above 800 ppm are considered unhealthy, amounts above 5,000 ppm are considered very unhealthy, and those above about 50,000 ppm are considered dangerous to animal life.

At standard temperature and pressure, the density of carbon dioxide is around 1.98 kg/m³, about 1.5 times that of air. The carbon dioxide molecule (O=C=O) contains two double bonds and has a linear shape. It has no electrical dipole, and as it is fully oxidized, it is not very reactive and is non-flammable.


Small pellets of dry ice subliming in air.At −78.5° C, carbon dioxide changes directly from a solid phase to a gaseous phase through sublimation, or from gaseous to solid through deposition. Solid carbon dioxide is normally called "dry ice", a generic trademark. It was first observed in 1825 by the French chemist Charles Thilorier. Dry ice is commonly used as a versatile cooling agent, and it is relatively inexpensive. As it warms, solid carbon dioxide sublimes directly into the gas phase, making its use convenient as it leaves no liquid. It can often be found in groceries and laboratories, and it is also used in the shipping industry. The largest non-cooling use for dry ice is blast cleaning.

Liquid carbon dioxide forms only at pressures above 5.1 atm; the triple point of carbon dioxide is about 518 kPa at −56.6°C (See phase diagram, above). The critical point is 7,821 kPa at 31.1°C.

An alternative form of solid carbon dioxide, an amorphous glass-like form, is possible, although not at atmospheric pressure.[2] This form of glass, called carbonia, was produced by supercooling heated CO2 at extreme pressure (40–48 GPa or about 400,000 atmospheres) in a diamond anvil. This discovery confirmed the theory that carbon dioxide could exist in a glass state similar to other members of its elemental family, like silicon (silica glass) and germanium. Unlike silica and germania glasses, however, carbonia glass is not stable at normal pressures and reverts back to gas when pressure is released.

Narendra

Answer 4

neither i would use a more reactive metal like Al

Answer 5

carbon monoxide.