Question

In the manufacture of steel, pure oxygen is blown through molten iron to remove some of the carbon impurity. if the combustion of carbon is efficient, carbon dioxide (density = 1.80 g/l) is produced. incomplete combustion produces the poisonous gas carbon monoxide (density - 1.15 g/l) and should be avoided. if you measure a gas density of 1.77 g/l, what can you conclude?

Answer 1

We can conclude that the gas evolved was carbon dioxide.

Step-by-step explanation:

On an efficient combustion that is on complete combustion of carbon, carbon dioxide is produced.

`C+O_2\rightarrow CO_2` (Complete combustion)

But during incomplete combustion of carbon results in formation of carbon monoxide (poisons gas).

`2C+O_2\rightarrow 2CO` (Incomplete combustion)

Theoretical value density of carbon dioxide = 1.80 g/L

Theoretical value density of carbon monoxide = 1.15 g/L

Experimental measured density of the gas = 1.77 g/L

1.77 g/L ≈ 1.80 g/L

Since, the experimental measured density of the gas is more closer to theoretical value of density of carbon dioxide from which we can conclude that 'the gas evolved after the combustion of carbon impurity was carbon dioxide'.

Answer 2

In the extraction process of steel, one of the step is purification of the iron used to make the steel. In which pure oxygen is blown on the steel at high temperature so that the carbon percentage present in the steel can be thrown out in the form of gas. The process occurs at high temperature which is called combustion process. The reaction occurs can be shown as- C(s)+
`O_(2)`→C
`O_(2)` (g) + CO (g). In presence of excess oxygen, the produced carbon mono oxide (CO) converts to carbon di-oxide. The reaction is CO(g) +
`O_(2)`(g) → C
`O_(2)` (g). From the density of the evolved gas one could identify the gas. If the gas density is 1.77g/L which is very close to the standard density of C
`O_(2)` i.e. 1.80g/L, the gas is carbon dioxide only.