| 953-08    (6bkxj dist, 3.5 mean)
 Selected-By: mchevalier@WELLESLEY.EDU
 The Internet Oracle has pondered your question deeply.
Your question was:
 
And in response, thus spake the Oracle:| > Oh Oracle most wise, I'm having some difficulty with an> extremely important scientific project.  Can you help me
 > solve it, please?  Let me explain...
 >
 > As we all know, it takes 1 calorie to heat 1 gram of water 1
 > degree centigrade. Translated into meaningful terms, this
 > means that if you eat a very cold dessert (generally
 > consisting of water in large part), the natural processes
 > which raise the consumed dessert to body temperature during
 > the digestive cycle literally suck the calories out of the
 > only available source, your body fat.
 >
 > For example, a dessert served and eaten at near 0 degrees C
 > (32.2 degrees F) will, in a short time, be raised to the
 > normal body temperature of 37 degrees C (98.6 degrees F).
 > For each gram of dessert eaten, that process takes
 > approximately 37 calories as stated above. The average
 > dessert portion is 6 oz, or 168 grams. Therefore, by
 > operation of thermodynamic law, 6,216 calories (1
 > cal./gm/deg. x 37 deg. x 168 gms) are extracted from body
 > fat as the dessert's temperature is normalized.
 >
 > Allowing for the 1,200 latent calories in the dessert, the
 > net calorie loss is approximately 5,000 calories.
 >
 > Obviously, the more cold dessert you eat, the better off you
 > are and the faster you will lose weight, if that is your
 > goal.
 >
 > This process works equally well when drinking very cold beer
 > in frosted glasses. Each ounce of beer contains 16 latent
 > calories, but extracts 1,036 calories (6,216 cal. per 6 oz.
 > portion) in the temperature normalizing process. Thus, the
 > net calorie lss per ounce of beer is 1,020 calories. It
 > doesn't take a rocket scientist to calculate that 12,240
 > calories (12 oz. x 1,020 cal./oz.) are extracted from the
 > body in the process of drinking a can of beer.
 >
 > Frozen desserts, e.g., ice cream, are even more beneficial,
 > since it takes 83 cal./gm to melt them (i.e., raise them to
 > 0 deg. C) and an additional 37 cal./gm to further raise them
 > to body temperature. The results here are really remarkable,
 > and it beats running hands down.
 >
 > Well, I've been experimenting for several years, and I'm sad
 > to report that my experimental results do not agree with the
 > theory above at all.  What went wrong?
 |  
| }       [The Internet Oracle walks up to the gates of Heaven...]}       <knock, knock>
 }       [Saint Pete sez] "Myeeeezzzzzz?"
 }       "I've got question for the big guy, Pete.  Run along and fetch
 } him, won't you?"
 }       "Right away, sir."
 }       ...
 }       "YES, MR. ORACLE, WHAT CAN I DO FOR YOU TODAY?"
 }       "I'm a bit irked about the current version of Humanitas,
 } actually;  it's still not fully case sensitive, you know."
 }       "YES, THE PATCH IS A BIT SKETCHY.  I'M STILL NOT QUITE SURE WHY
 } YOU THOUGHT THEY NEEDED TWO CASES, ANYWAY;  I DO FINE WITH JUST ONE."
 }       "Well, they *are* made in your image, but they aren't quite up to
 } the original standard.  F'rinstance, I've got one supplicant right now
 } who can't tell the difference between a calorie and a Calorie.
 }       "OH, IS THAT SO?  THAT'S OK, THERE'S A RUNTIME KLUDGE FOR THAT:
 } CALL THE LATTER A 'FOOD CALORIE'."
 }       "Well, yeah, but that's hardly a general solution to the problem.
 } I expect you to get to work on that right away, bud, or maybe I'll have
 } to think about transfering control of the Humanitas project to Zeus.
 } *He*, at least, got stuff done."
 }       "I'LL DO MY BEST, MR. ORACLE."
 }       [The Internet Oracle tramps back upstairs to His computer]
 }
 }       Okay, so anyway: the food Calorie is 1000 heat calories, so if
 } you eat a 1,200 Calorie dessert, you need to use up 1.2 million heat
 } calories to cancel it out.  At 83 cal/gm to melt, and 37 cal/gm to
 } heat, your typical frozen dessert uses up only 20,160 cal on its way to
 } body temperature.  That leaves you with a good 1,179,840 cal to burn
 } off.
 }       Of course, you could repeat the same argument at a lower
 } temperature;  let's see how cold your ice cream would have to be to
 } cancel out its fat and sugar content, Caloriewise:
 }       You need to get rid of 1.2 million heat calories by warming your
 } 168-gm mostly-water dessert.  Melting it takes care of 13,944 cal,
 } leaving you with 1,186,056 cal to burn.  Dividing that by the 168 gm
 } present, assuming 1 cal/(gm*degree), we get a required change in
 } temperature of approximately 7060 degrees Celsius, for an initial
 } temperature of -6750 K if you want to raise it to body temperature.  So
 } take heart!  All you have to do to lose weight by eating ice cream is
 } chill it to several thousand degrees below absolute zero.  Get to work!
 }
 }       You owe the Oracle an argument using quantum field theory to
 } nullify the laws of thermodynamics, a heat sink at -6751 K, a perfect
 } heat engine, and a pint of Ben and Jerry's Chocolate Chip Cookie Dough.
 |  |