Question

If the pressure of the gas in a 2.31 L balloon is .12 atm and the volume increases to 7.14 L, what will be the final pressure of the air within the balloon?

Answer 1

From Boyle's Law, `"pressure"xx"volume"="constant"`

`P_2~=2/7xx0.12*atm`

Explanation:

`P_1V_1=P_2V_2`

Thus `V_2` `=` `(P_1V_1)/P_2` `=` `(2.31*Lxx0.12*atm)/(7.14*L)`.

The advantage of using Boyle's Law is that I can use any units I like, `"pints"`, `"bars"`, `"mm Hg"`, `"foot pounds"`, `"gallons"` so long as I am consistent.