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,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

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:

$\frac{0.99atm\times 59.0L}{293.4K}=\frac{0.0819atm\times V_2}{269.19K}$

$V_2=654.338L$

The final volume will be, 654.338 L

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