Question

At 35 C, a sample of gas has a volume of 256 ml and a pressure of 720.torr. What would the volume

be if the temperature were changed to 22 C and the pressure to 1.25 atmospheres?

Answer 1

Answer: Volume would be 196.15 mL if the temperature were changed to
`22^(o)C` and the pressure to 1.25 atmospheres.

Step-by-step explanation:

Given:
`T_(1) = 35^(o)C = (35 + 273) K = 308 K`,
`V_(1)` = 256 mL,

`P_(1)` = 720 torr (1 torr = 0.00131579 atm) = 0.947368 atm

`T_(1) = 22^(o)C = (22 + 273) K = 295 K`,
`P_(2) = 1.25 atm`

Formula used to calculate volume is as follows.

`(P_(1)V_(1))/(T_(1)) = (P_(2)V_(2))/(T_(2))`

Substitute the values into above formula as follows.

`(P_(1)V_(1))/(T_(1)) = (P_(2)V_(2))/(T_(2))\\(1 atm * 256 mL)/(308 K) = (1.25 atm * V_(2))/(295 K)\\V_(2) = 196.15 mL`

Thus, we can conclude that the volume would be 196.15 mL if the temperature were changed to
`22^(o)C` and the pressure to 1.25 atmospheres.