<p>This question is little different from asking why, if the Sun is a ball of Hydrogen, it hasn't already exploded (or burned out). It is difficult for me to take it seriously. But I'll try. </p>

<p>Methane and Oxygen are gases and will react at room temperature and pressure in certain concentration ranges and when exposed to a spark (or other high energy density discharge; a flame, friction, etc.). We call these limits the LEL and UEL (abbreviations for Upper and Lower Explosion Limits) for hydrogen which change as the atmospheric concentration of Oxygen changes. A tragic example of this was the enormously stupid decision by NASA to use pure oxygen in the Apollo space capsules. During testing of Apollo 1, three astronauts burned to death in a flash fire in which the extreme oxygen concentration allowed almost all plastic materials (wire jackets, clothing, etc.) to burn intensely. An urban myth I have heard, but can neither confirm nor contradict, is that if you held a cigarette lighter under your finger in a pure O2 atmosphere, it would start to burn, and continue to burn even after the lighter was put out. </p>

<p>The temperature of a gas is an indication of how fast the atoms/molecules are going. As you lower the temperature, the average speed declines. For the $\mathrm{CH_4+O_2}$ reaction to proceed, you need the methane and the oxygen molecules' collision to impact hard enough to break chemical bonds. As temperature drops, this becomes increasingly unlikely. OTOH, the reaction also releases energy, so if there is enough energy both from the speed of the molecules and the energy released from the reaction products to induce more that one additional reaction, then you will have a chain reaction and the result will depend on whether the supply of both molecule types is large enough to sustain the reaction. It can self-quench, stay in a steady state (form a flame) or explode. Note that while on Earth, the most common reaction in the air is using oxygen as the oxidizer (one of the reactants), methane can react with many other gasses, for instance $\mathrm{F_2}$, fluorine or $\mathrm{Cl_2}$, Chlorine. </p>

<p>Since there is virtually no oxidizer present in Titan's atmosphere, methane can't burn, even if the temperature, pressure, and concentration were high enough.</p>

CC BY-SA 3.0
2016-07-09T18:06:37.860Z
Can you try to format your answer a little to make it easier to read?
SE - stop firing the good guys
CC BY-SA 3.0
2016-07-09T16:51:49.317Z
2016-07-09T19:15:07.763Z
2016-07-09T19:15:07.763Z
Li Zhi
<p><a href="http://en.wikipedia.org/wiki/Atmosphere_of_Titan" rel="nofollow noreferrer">Titan</a> is one of Saturn's moons. Titan has a dense atmosphere, at about 1.5 bars. It also seems to have lakes of liquid methane.</p>

<p>For a conventional combustion, you would need a good Methane-Oxygen mix. Every combustion is basically an oxidization. Apart from very energetic events, such as <a href="https://astronomy.stackexchange.com/questions/490/why-did-the-comet-shoemaker-levy-9-fragments-cause-such-large-explosions-on-jupi">SL9 hitting Jupiter</a>, you will need quite a bit of oxygen to get a nice, explosive fireball in Titan's atmosphere.</p>

<p><a href="http://en.wikipedia.org/wiki/Methane#Combustion" rel="nofollow noreferrer">According to Wikipedia</a>, you need two Oxygen molecules for every Methane molecule you want to burn.</p>

CC BY-SA 3.0
2014-04-02T09:53:06.327Z
@GreenMatt assuming that the kinetic energy released in a large enough impact locally raises the temperature to a few thousand degrees, that seems negligible?
usethedeathstar
CC BY-SA 3.0
2013-10-23T00:48:59.393Z
While it is a few degrees C above Methane's ignition point, Titan's surface temperature is very cold compared to Earth, which can't help.
GreenMatt
CC BY-SA 3.0
2013-10-18T11:40:39.473Z
2013-10-21T17:01:02.083Z
2017-04-13T12:59:06.910Z
Arne
<p>If Titan has a methane atmosphere and seas of methane, then why doesn't some meteoroid / chemical reaction ignite and blow the whole thing?</p>

CC BY-SA 3.0
2015-11-30T16:56:26.553Z
@Robert You'd probably get some reaction, because CO2 bonds are stronger than H2O bonds:http://www.chemguide.co.uk/physical/energetics/bondenthalpies.html  Since it's hard to ignite gasoline under water, I expect you'd see a far slower reaction than what we usually call fire.
Wayfaring Stranger
CC BY-SA 3.0
2013-10-27T22:12:44.437Z
It is a very legitimate question, please don't misinterpret me. I have upvoted it. But that "blow the whole thing" together with the mental picture it suggests, suddenly made laugh like hell.
Eduardo Guerras Valera
CC BY-SA 3.0
2013-10-29T05:26:28.010Z
Maybe i have seen too many sci-fi movies.
cowboysaif
CC BY-SA 3.0
2013-10-29T11:53:09.630Z
I love sci-fi too, and have read nearly all that Philip Dick wrote. The question is ok, it's just the lack of oxigen in that atmosphere what prevents "the whole thing to blow" (I am happy I have learnt that expression, my english has improved a bit!). Having the enormous amount of $O_{2}$ we have in our Earth atmosphere is a very rare thing. It is sustained by algae and plants. Otherwise, oxygen would be combined with other things, like it happens in Mars, and you would not be able to light a match here.
Eduardo Guerras Valera
<titan>
Why does Titan's atmosphere not start to burn?
cowboysaif
# Why does Titan's atmosphere not start to burn?

(Asked by: username_0 on 2013-10-18)

If Titan has a methane atmosphere and seas of methane, then why doesn't some meteoroid / chemical reaction ignite and blow the whole thing?

**Tags:** titan

> **Comments:**
> **username_2**: It is a very legitimate question, please don't misinterpret me. I have upvoted it. But that "blow the whole thing" together with the mental picture it suggests, suddenly made laugh like hell.  
> **username_0**: Maybe i have seen too many sci-fi movies.  
> **username_2**: I love sci-fi too, and have read nearly all that Philip Dick wrote. The question is ok, it's just the lack of oxigen in that atmosphere what prevents "the whole thing to blow" (I am happy I have learnt that expression, my english has improved a bit!). Having the enormous amount of $O_{2}$ we have in our Earth atmosphere is a very rare thing. It is sustained by algae and plants. Otherwise, oxygen would be combined with other things, like it happens in Mars, and you would not be able to light a match here.  
> **username_1**: @Robert You'd probably get some reaction, because CO2 bonds are stronger than H2O bonds:http://www.chemguide.co.uk/physical/energetics/bondenthalpies.html  Since it's hard to ignite gasoline under water, I expect you'd see a far slower reaction than what we usually call fire.  

---

## 2 answers

### Answer by username_5 on 2013-10-18. Score: 16 | Accepted answer

[Titan](http://en.wikipedia.org/wiki/Atmosphere_of_Titan) is one of Saturn's moons. Titan has a dense atmosphere, at about 1.5 bars. It also seems to have lakes of liquid methane.

For a conventional combustion, you would need a good Methane-Oxygen mix. Every combustion is basically an oxidization. Apart from very energetic events, such as [SL9 hitting Jupiter](https://astronomy.stackexchange.com/questions/490/why-did-the-comet-shoemaker-levy-9-fragments-cause-such-large-explosions-on-jupi), you will need quite a bit of oxygen to get a nice, explosive fireball in Titan's atmosphere.

[According to Wikipedia](http://en.wikipedia.org/wiki/Methane#Combustion), you need two Oxygen molecules for every Methane molecule you want to burn.

> **Comments:**
> **username_7**: While it is a few degrees C above Methane's ignition point, Titan's surface temperature is very cold compared to Earth, which can't help.  
> **username_6**: @username_7 assuming that the kinetic energy released in a large enough impact locally raises the temperature to a few thousand degrees, that seems negligible?  

---

### Answer by username_3 on 2016-07-09. Score: 6

This question is little different from asking why, if the Sun is a ball of Hydrogen, it hasn't already exploded (or burned out). It is difficult for me to take it seriously. But I'll try.

Methane and Oxygen are gases and will react at room temperature and pressure in certain concentration ranges and when exposed to a spark (or other high energy density discharge; a flame, friction, etc.). We call these limits the LEL and UEL (abbreviations for Upper and Lower Explosion Limits) for hydrogen which change as the atmospheric concentration of Oxygen changes. A tragic example of this was the enormously stupid decision by NASA to use pure oxygen in the Apollo space capsules. During testing of Apollo 1, three astronauts burned to death in a flash fire in which the extreme oxygen concentration allowed almost all plastic materials (wire jackets, clothing, etc.) to burn intensely. An urban myth I have heard, but can neither confirm nor contradict, is that if you held a cigarette lighter under your finger in a pure O2 atmosphere, it would start to burn, and continue to burn even after the lighter was put out.

The temperature of a gas is an indication of how fast the atoms/molecules are going. As you lower the temperature, the average speed declines. For the $\mathrm{CH\_4+O\_2}$ reaction to proceed, you need the methane and the oxygen molecules' collision to impact hard enough to break chemical bonds. As temperature drops, this becomes increasingly unlikely. OTOH, the reaction also releases energy, so if there is enough energy both from the speed of the molecules and the energy released from the reaction products to induce more that one additional reaction, then you will have a chain reaction and the result will depend on whether the supply of both molecule types is large enough to sustain the reaction. It can self-quench, stay in a steady state (form a flame) or explode. Note that while on Earth, the most common reaction in the air is using oxygen as the oxidizer (one of the reactants), methane can react with many other gasses, for instance $\mathrm{F\_2}$, fluorine or $\mathrm{Cl\_2}$, Chlorine.

Since there is virtually no oxidizer present in Titan's atmosphere, methane can't burn, even if the temperature, pressure, and concentration were high enough.

> **Comments:**
> **username_4**: Can you try to format your answer a little to make it easier to read?  

---

