Question

A gas-filled weather balloon has a volume of 59.0 L at ground level, where the pressure is 759 mmHg and the temperature is 20.4 "C. After being released, the balloon rises to an altitude where the temperature is -3.81 °C and the pressure is 0.0819 atm. What is the weather balloon's volume at the higher altitude? V = 43344.9 L

Answer 1

Answer : The volume of balloon at higher altitude will be 654.338 L

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 =
`759mmHg=0.99atm`

conversion used : (1 atm = 760 mmHg)

`P_2` = final pressure of gas = 0.0819 atm

`V_1` = initial volume of gas = 59.0 L

`V_2` = final volume of gas = ?

`T_1` = initial temperature of gas =
`20.4^oC=273+20.4=293.4K`

`T_2` = final temperature of gas =
`-3.81^oC=273+(-3.81)=269.19K`

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

`(0.99atm* 59.0L)/(293.4K)=(0.0819atm* V_2)/(269.19K)`

`V_2=654.338L`

The final volume will be, 654.338 L

Therefore, the volume of balloon at higher altitude will be 654.338 L