Do you old farts hit the gas on the first yellow?

 

Yep.

Same thing at traffic lights.

 

I've got you by 2 years..... ooooops, that was a contest I didn't really want to win.

I've given up on reaction time.... I seriously doubt I have ever cut better than a .560 light. I just got used to looking at tail lights in the other lane... at least for the first few seconds..... .

 

That puts you in the same 'era' as Don ***, Lee Dykstra and Herb Adams. Not necessarily engine guys, but still pretty good car engineers (for old farts).

 

Man, I feel like a kid again. Started college in '67!

Does this forum have the oldest farts, or what? Rest of the board is all "kids".

Rich Krause

 

Man these were the best answers ever, thanx guys

 

At least you can use Social Security checks for mods someday

 

Back to the whole Boyles Law, Charles Law thing, heres's a break down for future reference.

If you only were to learn one equation dealing with temperature/pressure/volume I would reccomend the Ideal Gas Law, AKA, PV=nRT, because the gas laws mentioned and the combined gas law can be derived from it.
P=pressure in ATM
V= Volume
n= # of moles of gas
R= .0821 L ATM/K mole (gas constant)
T= Temperature in Kelvin


Boyle's law: P1/P2=V1/V2 or P1V1=P2V2 (constant temp)
This law basically states that the volume of a gas is inversely proportional to its pressure at constant temerature and amount of material. (Or in this case, material=combustion gasses)

Charle's Law: P1/P2=T1/T2 (constant volume)
"At constant pressure and amount of material the volume of a gas is directly proportional to the temperature."
This law is the best one to answer our question, why does more heat make more pressure, (power), because of the constant volume and amount of gas in the CC.