pure oxygen with gasoline combustion???

[Guest meet]

Hey guys,

 

I have this really cool project that I'm doing in chemistry class. Havin trouble though, please help me out, this is all of the info that I was presented with and must complete a formal lab on it.

 

problem:

 

a concerned environmentalist wants to eliminate nitrous oxides NOx emmssions that occur when gasoline is burned with air. To solve this problem the environmentalists want to burn gas with pure oxygen in his vehicle. Fin the amount of oxygen required for the vehicle to travel 1000 km and the size of the tank compared to the vehicle if the oxygen is stored at STP.

 

thanks a lot all,

 

 

MEET

[Crash]

Need more info, what is the weight of the car.

most internal combustion engines are only about 30% efficent so i need more info like is it 1000km straight line etc what revz is the vechile pulling?

[Skye]

I'd say you could just assume the car uses some arbitrary amount of fuel, like 100 litres for the 1000 km. If you also assume that the fuel is simply octane, C8H18, then just write up the formula, calculate how many moles of octane is used, then use this to work out how many moles of oxygen are used.

[YT2095]

and just be carefull too!, Goddard used the same mix in his rocket engines and they worked! that may give you an idea of it`s potency and potential dangers too!

[Cap'n Refsmmat]

Didn't Goddard use kerosene, not gasoline?

And, if you did do it, you'd have to change the valves, since when it would intake air it would be purely oxygen, not 21% or whatever oxygen. Pure oxygen in the same quantities as normal air burns very fiercly (or, should I say, is an accellerant).

Just ask the crew of Apollo 1.

[Crash]

any way.........

since no ones attempted i will try,

C8H18 + 12.5O2 -> 8CO2 + 9H20

 

then octane= 5512 Kj per Mole

 

THIS IS WHAT I COPULDNT FIND

Octane =???????? Mol per Litre

 

then work out your average car which is 800Kg, then its distance its going 1000Km, then for basics (to tired) use w= F times D

W=8000N*100000metres

work =800000000j

 

then work out how many moles or litres of octane it would take to produce this and there you go for a basic one anyway.

 

Remeber this isnt possible due to heat produced, getting pure oxygen, fuel isnt just actane the list goes on for what really happens here you go

 

(C8H18)+ 12.5(O2+3.76N2)--> 8(CO2)+ 9(H2O)+ 47(N2)

[Crash]

this is a type of engine developed around the 1950s

The exhaust temp was cool enough to put your hand near due to the almost complete combustion of fuel (including the hydrogen which favors an oxygen rich environment and high heat). Also, the fuel burned so quickly, driven by the hydrogen flame propagation, that the end of the piston stroke during expansion was actually a refrigeration cycle which cooled the spent gasses before exhausting them. The combustion "event" is very much like a sharp detonation and only the in-line piston design saves the engine from becoming a pile of aluminum sand. The traditional Bourke engine has no flywheel and reaches ungodly rpm's. The torque vs. rpm plotted curve looks similar to that of a turbine.

 

http://bourke-engine.com/index1.htm