What is reaction of oxygen and acetylene?

Answer 1

it is used for cutting metals ( example with a proper mixture by regulators you use a cutting torch)

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The mixture as such is just oxygen and acetylene, but acetylene is highly flammable and when additional oxygen is introduced, the flame is hot enough to melt steel to weld it.

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For cutting, the metal is first brought to melting-point or nearly so by the gas flame, then excess oxygen is added to burn rather than melt the iron itself, with the gas flame maintaining the heat input and temperature. The oxy-gas cutting torch differs from the welding torch by a different type of nozzle and having a trigger on its side to operate the cutting-oxygen valve.

Answer 2

There are many possible situations depending on what fuel / oxygen ratio you have:

With sufficient oxygen: 2C2H2 + 3O2 = 4CO2 + 2H2O

That's the ideal situation when you have a stoichiometric mixture. If the oxygen is lower than stoichiometric and close to 1:1 by volume you get:

C2H2 + O2 = 2CO + H2

In fact, at the temperature that it reaches (above 3000 deg. C) some of the molecular H2 will be actually dissociated in atomic Hydrogen. The real outcome will be something like:

60.7% CO

21.4% H2

17.7% H (atomic)

That is what you get after the first flame front (cone) in an acetylene torch. In other words, carbon monoxide, and hydrogen.

Now! What you ACTUALLY get in a low-oxygen environment (you haven't turned your oxygen on yet, or you ran out) is very much different. Carbon monoxide has a much stronger tendency to form than H2O, so only when all carbon is consumed hydrogen will have a chance to oxidize. For instance, a mixture (by weight) of 95% Acetylene with 5% oxygen will give something like:

61.8% C (solid) <- that is the Carbon Black produced by low oxygen flames

31.8% H2

3.0% CO

2.1% C2H2

1.2% H

0.1% C2H

When you light an oxyacetylene torch, you turn on the acetylene first, light it, then turn the oxygen on. When you turn the torch off, you turn off the oxygen first. Until you get the oxygen on or the acetylene off, the carbon (which is more reactive than hydrogen) is going to grab all the oxygen it wants, and the hydrogen won't get any. If there is not enough oxygen even for the carbon, it will have no choice but to bond to itself, forming the product Carbon Black. That's what all the black smoke coming off the flame is, just plain ol' Carbon Black.

Carbon monoxide and hydrogen have nearly the same affinity for oxygen, so as more oxygen comes to the mix, both, CO2 and H2O will start to form.

The equation in the beginning of this answer is also considering that the compounds reach equilibrium at room temperature. The real compounds formed right after the stoichiometric combustion of H2O2 in pure O2 the products will be at a temperature above 3000 C, so H2O and CO2 are not always dominant species. Hot combustion products will look more like this:

33.3% CO

12.5% O2

12.0% CO2

11.1% O

10.5% H2O

9.5% HO

7.4% H

3.7% H2

It might look funny how free Oxygen and free Hydrogen coexist in equilibrium at those temperatures, but at 3000C that is how it goes.

References:

All combustion product calculations were based on the algorithms created by D.R. Cruise at "Theoretical Computations of Equilibrium Compositions, Thermodynamic Properties and Performance Characteristics of Propellant Systems".

Answer 3

the cause an explosion, depending on the balance of each element

Answer 4

u get carbon dioxide C=carbon O2 =oxygen CO2=carbon dioxide

cmon im only 13 and i no dis

Answer 5

When ethanol is burned in oxygen, carbon dioxide and water are formed as the products.

Answer 6

This is a combustion reaction. Here is the balanced equation: C2H2(g) + (5/2)O2(g) --> 2CO2(g) + H2O(g)

Answer 7

nothing#$%^&*((REDFGUJIO

Answer 8

Carbon dioxide and water

Answer 9

A fart