Mike Voigt
Supporting Actor
- Joined
- Sep 30, 1997
- Messages
- 799
Ajay - here's the issue:
Oil has a tremendous amount of energy already stored in it. It is also combustible, i.e. provide it with a heat source (even if just instantanoeus) and an oxidizer (does not have to be oxygen, but usually is), and it will burn - merrily. For a really harsh example, look at the lit oil wells left behind by the Iraqis in the first Gulf War.
You can do the same with coal, paper, wood, etc. The energy density varies - the amount, per cubic inch, that is stored in the material. So, per cubic inch, hard coal/black coal/anthracite has the highest, and wood has much less. You don't get as much heat out of one cubic inch of wood as you do out of one cubic inch of coal. Ditto with oil - it gives up much more energy than wood.
In water, you have no such thing. You cannot burn it; it is largely inert matter. The waater molecule is very difficult to pry apart; you need energy to do so. You have to introduce and store that energy - in the case of water, separation of water into hydrogen and oxygen, then storign those gases - before you can use it. Using it is essentially "burning" the hydrogen with oxygen. Result - you get water. And start over - except it took more energy to separate the water into gases than you got out of the hydrogen "burn"... moreover, you have to get that energy from somewhere.
Int eh case of oil, it is much easier to use - you don't have to make it, nature already has it ready for you. You don't have to stick nearly as much energy into retrieving it (although that cost goes up and up over time) as you would into having to split water into hydrogen and oxygen.
I like Cees' analogy of a battery. You are storing up energy to use later. In the case of oil, that's done for you. In the case of hydrogen, it isn't, and you have to provide the means (read: energy) to "make" the battery in the form of two substances: hydrogen and oxygen.
Now, we've talked about water, but there are other sources of hydrogen. For example, we could take ethane (C2H6) and change it into ethene (C2H4) - this would gain us two hydrogen atoms. Unfortunately, this also takes energy to do.
In all instances, though, you will have to add energy to gain the hydrogen. Only then can you use it.
The trick is to find a process using the absolute minimum amount of energy and resources to do this. Then, designing a process such that the energy required to generate hydrogen is as smallishly greater than the energy you get back out, i.e. optimize the energy returned (from the burn) on the energy invested (to make the hydrogen). Better yet, the process is easily reversible so you don't have to go through lots of extra steps.
Mike
Oil has a tremendous amount of energy already stored in it. It is also combustible, i.e. provide it with a heat source (even if just instantanoeus) and an oxidizer (does not have to be oxygen, but usually is), and it will burn - merrily. For a really harsh example, look at the lit oil wells left behind by the Iraqis in the first Gulf War.
You can do the same with coal, paper, wood, etc. The energy density varies - the amount, per cubic inch, that is stored in the material. So, per cubic inch, hard coal/black coal/anthracite has the highest, and wood has much less. You don't get as much heat out of one cubic inch of wood as you do out of one cubic inch of coal. Ditto with oil - it gives up much more energy than wood.
In water, you have no such thing. You cannot burn it; it is largely inert matter. The waater molecule is very difficult to pry apart; you need energy to do so. You have to introduce and store that energy - in the case of water, separation of water into hydrogen and oxygen, then storign those gases - before you can use it. Using it is essentially "burning" the hydrogen with oxygen. Result - you get water. And start over - except it took more energy to separate the water into gases than you got out of the hydrogen "burn"... moreover, you have to get that energy from somewhere.
Int eh case of oil, it is much easier to use - you don't have to make it, nature already has it ready for you. You don't have to stick nearly as much energy into retrieving it (although that cost goes up and up over time) as you would into having to split water into hydrogen and oxygen.
I like Cees' analogy of a battery. You are storing up energy to use later. In the case of oil, that's done for you. In the case of hydrogen, it isn't, and you have to provide the means (read: energy) to "make" the battery in the form of two substances: hydrogen and oxygen.
Now, we've talked about water, but there are other sources of hydrogen. For example, we could take ethane (C2H6) and change it into ethene (C2H4) - this would gain us two hydrogen atoms. Unfortunately, this also takes energy to do.
In all instances, though, you will have to add energy to gain the hydrogen. Only then can you use it.
The trick is to find a process using the absolute minimum amount of energy and resources to do this. Then, designing a process such that the energy required to generate hydrogen is as smallishly greater than the energy you get back out, i.e. optimize the energy returned (from the burn) on the energy invested (to make the hydrogen). Better yet, the process is easily reversible so you don't have to go through lots of extra steps.
Mike