Yes, that will do.
V = k T
as T goes up, the volume gets big.
If the gas is in your lungs, your lungs get big.
This is not good.
Divers call it "air embolism" when they do not breathe out coming up. (The other Law, Boyle's, P V = k, you put this all together into the ideal gas law, PV/T = n R where n is number of moles of gas and R is the "gas constant") The gas in their lungs expands, and if they are not re-compressed quickly and treated, they die.
In planning to administer a gaseous anesthetic to a patient,
A) why mus the anthesiologist take into account the fact that during surgery the gaseous anesthetic is used both at room temperature (18C) and at the patients body temperature (37C)?
B) What problems might arise if the anesthesiologist did not allow for the patients higher body temperature?
I tried doing this problem but it doesnt make sense to me. I think I'm supposed to use Charles's law: V divided by T = K
can you help please?
Thanks
1 answer
1 answer