# Does more fire create a hotter fire?

If we lit a single fire that was fueled by a substance that burns at 500°F, then around that fire we lit directly against it another fire surrounding the original one. This second fire's fuel also burns at 500°F. Would the original fire increase in temperature? If yes, is there any topic related to this event that I can take to research it further?

• Where is the difference between 2 fires burning at 500°F and a single larger one burning at 500°F here? Why do you think it might get hotter? Commented Aug 30, 2020 at 14:56
• According to the answers, the flames have the potential to reach temperatures beyond 500°F. Do you disagree? I've differentiated the two fires so I can hopefully receive a more specific answer. Commented Aug 30, 2020 at 19:10
• Will the fire surrounding the inner fire take away oxygen that otherwise would be used by the inner fire?
– Mast
Commented Aug 31, 2020 at 9:27

By 500 F I assume you are talking about the ignition temperature of the material being burned when it first ignited, not the temperature of the surface and the flame above the burning material after ignition, which would be considerably higher than 500 F (500 F is around the ignition temperature of wood). Once the fuel, say wood, ignites then the surface temperature and flames will be greater than 500 F.

In that case, I would think that making the fire larger (increasing the circumference of the fire) may increase the temperature of the burning surface and flames and the rate of burning of the fire (heat release) as follows:

The figure below is a simplified representation of a burning surface showing heat and mass transfers (based on the Drysdale fire protection textbook "Introduction to Fire Dynamics".) Part of the heat released in the combustion process is fed back to the burning surface to maintain the combustion process. Part of the heat released is lost to the atmosphere, $$\dot Q_{atm}$$. (a key to the other terms is given below, if you are interested).

One would expect that most of the heat loss occurs above the flame. But some heat loss also occurs to the side of the flame (i.e., around the perimeter of the burning area). Thinking of the perimeter as the surface of a cylinder surrounding the burning area, the larger the perimeter the lower the surface area to volume ratio. That could favor heat retention in the center of the flaming area and an increase in the temperature of the flames at the center.

A more detailed explanation of the figure is below. In particular I draw your attention to the last two equations. The first gives the heat release rate. The greater that rate the higher the burning temperature, all other things being equal. It is proportional to the mass burning rate.

The last equation gives the mass burning rate. Note that the lower the heat loss rate the greater the mass burning rate. The lower surface to volume ratio of the fire the lower the heat loss rate, all other things being equal.

Hope this helps

Key to Terms in Figure:

$$\dot Q_{c}$$ = rate at which energy (heat) is released in the fire (kW)

$$\dot Q_{F}$$ = the heat flux supplied by the flame fed back to the fuel surface ($$\frac{kW}{m^2}$$)

$$\dot Q_{L}$$ = heat losses expressed as the heat flux through the fuel surface ($$\frac {kW}{m^2}$$)

$$\dot Q_{atm}$$ = heat lost to atmosphere (kW)

$$\dot m$$ = the rate of burning of the fuel ($$\frac{kg}{m^{2}.s}$$)

According to Drysdale, "...the rate at which energy is released in a fire ($$\dot Q_{c}$$) is the most important single factor which characterizes its behavior"

The heat release rate ($$\dot Q_{C}$$) can be roughly related to the rate of burning $$\dot m$$ and the heat of combustion of the fuel by the following:

$$\dot Q_{c}= x.\dot m . A_{f}\Delta H_{c}$$

where

$$A_f$$ is the fuel surface area ($$m^2$$)

$$\Delta H_{c}$$ is the heat of combustion of the volatiles ($$\frac{kJ}{kg}$$) and

$$x$$ is a factor to account for incomplete combustion (<1.0) which is a function of the mixing of air drawn in from the surrounding atmosphere with the volatiles.

The rate of burning can, in turn, be expressed generally as

$$\dot m=\frac{\dot Q_{F}-\dot Q_{L}}{L_{v}}$$

Where $$L_{v}$$ is the heat required to convert the fuel into volatiles. For a liquid, that would be the latent heat of vaporization.

• I think this is close to answering my question. I am talking about the temperature of the flames above the material, as well as the ignition temps. If the flames can reach temperatures higher than the ignition temp of their fuel, does that mean the fire could ignite something that burns at a temperature higher than the substance the fires are burning on? (Couldn't edit comment, took more than 5 minutes I guess) Commented Aug 30, 2020 at 19:02
• I’ve edited the beginning since I now understand you were not talking about the initial ignition temperature but the burning temperature of the surface and flames after ignition. Hope it helps Commented Aug 30, 2020 at 19:03
• I added two more paragraphs before seeing your completed comment that directly links burning temperature with heat loss rate. Regarding completed comment the short answer is yes. The burning temperature will generally be higher than the Ignition temperature. So a material above the surface with an ignition temperature greater than 500 F (the ignition temperature of the original surface) could ignite Commented Aug 30, 2020 at 19:26
• Good analysis. Really hard to say what that does to the oxygen supply though, which then has much stronger effects on reaction rate. Commented Aug 31, 2020 at 13:42
• @fectin Good point. I believe the oxygen supply affects $x$ (rate of burning of fuel) in the second to last equation. So it reduces the heat release rate. But whatever the heat release rate is, part of it is lost to the atmosphere and the rest fed back to the fuel surface. Commented Aug 31, 2020 at 14:00

Fire is caused by an exothermic oxidation reaction. For example if chemically we represent the wood in a wood fueled fire as a generic hydrocarbon $$\text{C}_n\text{H}_m$$, then the oxidation reaction will be:

$$\text{C}_n\text{H}_m(s) + \frac{4n+m}{4}\text{O}_2(g) \to n\text{CO}_2(g) + \frac{m}{2}\text{H}_2\text{O}(g)+\Delta H$$

During the reaction much heat ($$\Delta H$$) is released: the reaction is exothermic.

But chemical reactions don't have some set point at which they proceed, as the OP implies. Instead the rate at which they proceed (the reaction rate) depends on temperature. According to Arrhenius reaction speed increases strongly with reaction temperature.

This second fire's fuel also burns at 500°F. Would the original fire increase in temperature?

The problem here is that neither fire is contained so that all energy generated can escape all the time. This is a problem we usually rectify, if we want to achieve the highest possible temperature, by running the fire in a enclosure known as a oven or furnace. Below is pictured a highly efficient reverberatory furnace (courtesy Wikipedia):

With containment higher temperatures can be achieved; with higher amounts of combustible and higher reaction rates due in turn to higher furnace temperatures.

• So this means that the original fire could exceed 500°F if the fires were contained in some way that forces their energy to be more directed toward each other? Commented Aug 30, 2020 at 18:51
• Yes, absolutely.
– Gert
Commented Aug 30, 2020 at 18:53
• Clearly observable in a wood-fired pottery kiln. Wood ignites at 400-500 F, pottery fires at 1800-1900 F. Commented Aug 30, 2020 at 22:27

### Heat generation

Fire is an exothermic chemical reaction between one or more substances. As the input substances react and form the output substances, energy is released. Most of this energy will be in the form of heat.

### Heat distribution

This heat is at first concentrated in the reaction products. Some of the heat will be used to do work, providing a draft. Some will be radiated to everything around it, but in an open fire, most of it will remain in the combustion products, flying off into the sky.

### Temperature

Heat and temperature are not the same thing. The amount of heat required to raise the temperature of a kilogram of one substance by one degree can be completely different from the amount of heat required to raise the temperature of another substance by one degree. In any case, concentrating the heat in less substance, will result in a higher temperature.

In addition to this, adding heat will raise the temperature, so the hotter the reactants are going in, the hotter the result will be going out.

To concentrate the heat produced, you want a reaction between your fuel and somewhere near the stoichiometrically optimal amount of oxygen. However, unless you have a bottle of oxygen lying around, you'll also be bringing in a lot of nitrogen, about four times as much as the oxygen you needed. If your fuel is wet, you'll also be spending a lot of your heat on vaporizing the water. Similarly, as you heat wood, you will spend part of the heat pyrolyzing it, driving off combustible gases while leaving charcoal behind.

### Conclusion

So, to get the hottest flame you can, you will want to do the following things, in a rough order.

1. Dry your fuel (you can do this by just piling it around the center of the fire)
2. Enclose your fire, if possible (an open hearth tends to be less than 10% efficient, while a fairly simple stove can already reach over 90%)
3. Heat your fuel (a properly built fire will do this all by itself)
4. Use higher energy fuel (charcoal is already pyrolyzed and dry, and will give off more heat per amount of oxygen used to burn it).
5. Heat your oxidizer (this is a bit harder to do. air that moves through the fire will heat up, but will also be depleted in oxygen. Various types of iron smelting furnaces use the exhaust gases to heat the incoming air though)
6. Enrich your oxidizer (get rid of all (or at least some of) that pesky nitrogen diluting your oxygen, and your flames will burn much hotter)

To answer your actual question: a bigger fire does not necessarily burn hotter, but it will insulate the center of the fire from the cold not-fire surrounding it, and it will serve to do many of the things stated above. There are definitely limits though, if you don't use excessive technological tricks to work around them. (if you use a wood-fired power plant to power a plasma generator, did your fire burn at 10 kilokelvin?)

Several answers have mentioned how multiple fires can supply heat to each other, but that isn't the most significant mutual heating effect.

The most important factor is the oxygen supply, which under certain conditions can be greatly increased beyond a critical level, creating a firestorm:

A firestorm is created as a result of the stack effect as the heat of the original fire draws in more and more of the surrounding air. … As the updraft mushrooms, strong inwardly-directed gusty winds develop around the fire, supplying it with additional air. … The greater draft of a firestorm draws in greater quantities of oxygen, which significantly increases combustion, thereby also substantially increasing the production of heat. The intense heat of a firestorm manifests largely as radiated heat (infrared radiation), which may ignite flammable material at a distance ahead of the fire itself. This also serves to expand the area and the intensity of the firestorm. Violent, erratic wind drafts suck movables into the fire and as is observed with all intense conflagrations, radiated heat from the fire can melt asphalt, some metals, and glass, and turn street tarmac into flammable hot liquid. The very high temperatures ignite anything that might possibly burn, until the firestorm runs low on fuel. — Firestorm - Wikipedia

Also see Scijinks.gov:

Anyone with a log burner will tell you that two logs burn hotter and more fiercely than one. It makes sense that twice the fuel would produce twice the energy, but there is more going on than that.

What appears to happen is that some of the heat radiated by one log is absorbed by the other and vice-versa, raising the temperature of the fuel and allowing it to burn more quickly, at least up to the limit of the oxygen available. The increased surface area is also a factor, and also possibly the increased airflow if the fire draws in more air.

Practically speaking, if you put one big log in the burner it can be difficult to maintain a fire. Placing two smaller logs is more effective, but if they are directly adjacent, not so much. Placing two logs with a gap between them usually results in a strong fire, especially if they have flat surfaces facing each other. The airflow between them is a major factor (the gap is like a chimney), but it is clear that the heat from one log is helping maintain the fire in the other that might have otherwise gone out.

In forest fires, the effect known as a Firestorm appears to be related with the increase in airflow.

Depending on the distance between the fires, depletion of the oxygen content of air entering them, may well reduce the flame temperature of one or both.

I had the same issue to get higher degree with multiple flames, however above answer about burning a log can be true but in lab-scaled situation it can be different. lack of oxygen between two flame is important to get the highest efficiency but its not all. if we assume A is our flame and B is a log and we want to burn the log, difference between temperature of A and B makes what we want in an exothermic reaction, energy is released because the total energy of the products is less than the total energy of the reactants then it means difference. so when you have no difference there will be no reaction, when there is two flame with exactly same degrees there will be no change because of no difference. in reality its not common to have two flames with constant temperature in a period of time so we can't do it while picnicking and whenever we use two flames we feel its warmer than one flames. maybe its better to discuss about multiple flames instead of a big flame

You may have some localized temperature increases due to air circulation... but it is the fuel that mostly determines the temperature of the flame.