why the fire in the stove looks blueish color when it is in high flame
Don't say due to CO2 i want physical answer from physics theories....!
Answers
Answer:
Oxidation is what happens when a chemical with electrons to give meets a chemical that is electron deficient.
So, you’ve got a chemical that is electron rich, and those electrons aren’t tightly bound. In the case of fire this is the fuel, be it candle wax or paper or wood or gasoline. You’ve got another chemical that has an affinity for electrons. In the case of fire this is the oxygen in the air.
Now, you can take a candle and some air and stare at them until you starve to death - you’ll see no oxidation. That’s because another factor is required for fire: speed.
And in chemistry, speed is heat. The hotter a thing is, the faster its molecules are moving.
Thus, at room temperature, the rate at which oxidation occurs is painfully slow. In fact, wax is stable for decades at least.
But, for every 10ºC you increase the temperature, you roughly double the rate at which a reaction takes place. So, at say 20ºC (room temperature) the reaction is very slow. But at 800ºC (roughly the temperature of a candle flame), you’ve increased the rate of the reaction by a factor of very roughly 2^78 power. That’s about a million billion billion times faster.
So yeah, a lot faster.
Anyway, what’s happening in that candle?
Well, you’ve got some wax stuck to the wick. When you place the lit match near the wick, that wax melts as its molecules speed up. The air nearby is also greatly accelerated, and oxygen molecules start to bang into wax molecules. They were doing this before, of course, but really slowly. They lacked the activation energy necessary to, well, activate the reaction.
But now that you’ve added all that thermal energy, some of these collisions have what it takes to make a reaction. You can think of it like tapping glasses against the countertop. If you tap them very slowly, you can tap them over and over and over and over and over and almost never break a glass. But if you speed up the collisions, breaking a glass becomes more and more likely.
Anyway, as these collisions start possessing a lot of energy, some of them result in broken molecules. Literally. The oxygen molecules break and combine with the wax molecules. This releases a significant amount of energy which, in turn, heats up the molecules nearby. Again, remember this means speeding them up. This makes more collisions happen, and increases the energy of those collisions.
In other words, fire makes more fire.
And thus, the reaction self-perpetuates.
Were this a puddle of gasoline, the whole thing would be up in flames in short order. But a candle has something going for it that limits the reaction rate - most of the wax is solid and far from the hot spot. In fact, the hot spot is far enough away from the wax that the body of the candle itself doesn’t burn - only the wax that gets sucked into the wick has access to the necessary energy.
Now, why does it glow?
Well, remember how I said the energy released heats up the other molecules? That’s not entirely true: some of the energy is released as light. ALL fires glow, but not all of them glow in wavelengths we can see. Methanol famously burns without emitting much visible light, which makes methanol fires horribly dangerous. Methanol is sometimes used in racing fuel and, as a result, fires in auto races are sometimes invisible. YouTube this for some rather horrific videos.
Finally, other chemical reactions give off light, but they almost exclusively involved oxidation (though not always with oxygen gas). The glow sticks that you crack to activate work by oxidizing a chemical with hydrogen peroxide. The resulting product is unstable and slowly leaks away its energy in a constant glow of light.
You get a blue gas flame with a hydrocarbon gas when you have enough oxygen for complete combustion. When you do have sufficient oxygen, the gas flame appears bluebecause complete combustion creates enough energy to excite and ionize the gas molecules in the flame.
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