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

`V_2=12.1L`

Step-by-step 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:

`(P_1V_1)/(T_1) =(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=(P_1V_1T_2)/(T_1P_2)\\\\V_2=(0.987atm*8.50L*233K)/(293K*0.550atm)\\\\V_2=12.1L`

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