what is a complete and incomplete combustion reaction ??

A complete combustion occurs when there is sufficient oxygen to react completely with the other material; i.e.., when the material being oxidized is the limiting reagent. An incomplete combustion occurs when there is insufficient oxygen to burn the other material completely; i.e., oxygen is the limiting reagent.

A complete combustion reaction occurs when a substance (usually a hydrocarbon) combines with oxygen (O2) in the air to produce carbon dioxide (CO2) and water (H2O) as the only products. This type of reaction releases a large amount of energy, typically in the form of heat and light. Here's an example of a complete combustion reaction:

C6H12O6 + 6O2 → 6CO2 + 6H2O

In this reaction, glucose (C6H12O6) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). Notice that there are no byproducts other than CO2 and H2O, making it a complete combustion.

On the other hand, an incomplete combustion reaction occurs when there is a limited supply of oxygen during the reaction. This leads to the formation of products other than just carbon dioxide and water. Incomplete combustion is usually less efficient and releases less energy compared to complete combustion. These additional products can include carbon monoxide (CO), carbon (C), and water vapor (H2O). Here's an example of an incomplete combustion reaction:

2C4H10 + 9O2 → 8CO + 10H2O

In this reaction, butane (C4H10) combines with oxygen (O2) to produce carbon monoxide (CO) and water (H2O). As you can see, CO is produced instead of CO2, indicating an incomplete combustion.

To identify whether a combustion reaction is complete or incomplete, you need to analyze the products formed. If carbon monoxide (CO), carbon (C), or soot is present as byproducts, it suggests incomplete combustion. If only carbon dioxide (CO2) and water (H2O) are formed, it indicates complete combustion.