Keeping the number of moles constant, what is the final pressure in atm if the temperature was cooled from -91.5°c to -239°c, the volume decreased from 3.41l to 3.3l and the original pressure was 3990 torr?

change celcius to kelvin.

The answer to your question is:      P2 = 772.35 torr.

Explanation:

Data

P1 = 3990 torr.

V1 = 3.41 L

T1 = -91.5°C  = 181.5°K

P2 = ?

V2 = 3.3 L

T2 = -239°C = 34°K

Formula

                                 P2 = \frac{(3990)(3.41)(34)}{(181.5)(3.3)}[/tex]

                                 P2 = 462600.6 / 598.95

                                 P2 = 772.35 torr.

you need to have a picture of the atom that way we can answer it