Problem: A weather balloon filled with helium is launched at sea level in Florida on a clear day when the temperature is 35 °C and the atmospheric pressure is 765 torr. Before launch, the balloon has a volume of 75.0 L. After the balloon is launched, it rises to 12,000 meters altitude and three hours later, measurements from the balloon at that altitude indicate that the temperature is -48 °C and that the pressure is 468 torr. Find: A) the mass of helium gas initially in the balloon, B) the new volume (in L) of the balloon at 12,000 meters, and C) the density of helium gas at 12,000 meters.

FREE Expert Solution

We are asked to calculate for the following: 

A) the mass of helium gas initially in the balloon, 

B) the new volume (in L) of the balloon at 12,000 meters, and 

C) the density of helium gas at 12,000 meters.


A) Calculate for the mass of helium initially using the modified ideal gas law.


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Problem Details

A weather balloon filled with helium is launched at sea level in Florida on a clear day when the temperature is 35 °C and the atmospheric pressure is 765 torr. Before launch, the balloon has a volume of 75.0 L. After the balloon is launched, it rises to 12,000 meters altitude and three hours later, measurements from the balloon at that altitude indicate that the temperature is -48 °C and that the pressure is 468 torr. Find: A) the mass of helium gas initially in the balloon, B) the new volume (in L) of the balloon at 12,000 meters, and C) the density of helium gas at 12,000 meters.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ideal Gas Law Density concept. If you need more Ideal Gas Law Density practice, you can also practice Ideal Gas Law Density practice problems.