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Question: What is the balanced equation for the combustion of benzene \(\left( {{C_6}{H_6}} \right)\)?...

What is the balanced equation for the combustion of benzene (C6H6)\left( {{C_6}{H_6}} \right)?

Explanation

Solution

We know that combustion reaction is a substance response in which a fuel goes through oxidation by responding with an oxidizing specialist, bringing about the arrival of energy (typically as warmth). Combustion responses are for the most part exceptionally exothermic redox responses between an oxidant and a fuel. The item framed in a combustion response is typically the oxidized fuel (which is for the most part freed in the vaporous state). This is regularly alluded to as smoke. It isn't unprecedented for combustion responses to be joined by flares. In any case, it is fundamental for note that not all combustion responses bring about flames.

Complete answer:
We need to know that the benzene is a particle consisting of six carbon molecules and six hydrogen iotas. At the point when benzene goes through ignition in air, the carbon and hydrogen iotas consolidate with the atoms of oxygen present in air to frame carbon dioxide and water separately.
Carbon responds with oxygen to given carbon dioxide: C+O2→CO2C + {O_2} \to C{O_2}
Hydrogen responds with oxygen to frame water: 2H2+O2→2H2O2{H_2} + {O_2} \to 2{H_2}O
The fair condition of the substance response of the burning of benzene in air is,
2C6H6+15O2→12CO2 + 6H2O2{C_6}{H_6} + 15{O_2} \to 12C{O_2}{\text{ + }}6{H_2}O

Note:
We have to remember that strong energies like coal and wood are known to at first go through endothermic pyrolysis, bringing about the formation of vaporous powers. The combustion of these vaporous energizes is known to give the warmth needed to drive more burning. Additionally, it isn't phenomenal for combustion to likewise be adequately hot to produce glowing light as either a fire or some gleaming. The change of hydrogen and oxygen into water fumes, a cycle generally used to control rocket motors, can be viewed as a basic illustration of combustion. Here, hydrogen is utilized as a fuel and oxygen is utilized as an oxidizing specialist. This burning response is known to deliver more than 242242 kilojoules of warmth for each mole of fuel exposed to combustion.