Question

helium ballon is filled iwth a volume of 2.88 x 10 to the 3 power at 722 mmHg and 19C. When the ballon is released, it rises to an altituse where the pressuare and temperature are 339mmHg and -55C, respectively. What is the volume of the balloon?

Answer 1

Answer: The volume of the balloon is
`4.58* 10^3`

Step-by-step explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

where,

`P_1` = initial pressure of gas = 722 mm Hg

`P_2` = final pressure of gas = 339 mm Hg

`V_1` = initial volume of gas =
`2.88* 10^3`

`V_2` = final volume of gas = ?

`T_1` = initial temperature of gas =
`19^oC=273+19=292K`

`T_2` = final temperature of gas =
`-55^oC=273-55=218K`

Now put all the given values in the above equation, we get:

`(722* 2.88* 10^3)/(292)=(339* V_2)/(218)`

`V_2=4.58* 10^3`

Thus the volume of the balloon is
`4.58* 10^3`