Question

A helium filled ballon had a volume of 8.50 L on the ground at 20.0 C and a pressure of 750.0 Torr. After the ballon was released, it rose to an altitude where the temperature was -40.0 C and the pressure was .550 atm. What is the new volume of the balloon in liters at the high altitude?

Answer 1

Answer:

$V_2=12.1L$

Explanation:

Hello!

In this case, according to the given data of volume, pressure and temperature, it is possible to infer this problem can be solved via the combined gas law:

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

Thus, regarding the question, we evidence we need V2, but first we make sure the temperatures are in Kelvins:

$T_1=20+273=293K\\\\T_2=-40+273=233K$

Then, we obtain:

$V_2=\frac{P_1V_1T_2}{T_1P_2}\\\\V_2=\frac{0.987atm*8.50L*233K}{293K*0.550atm}\\\\V_2=12.1L$

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