Problem: A helium-filled balloon of the type used in long-distance flying contains 420, 000 ft3 (1.2 times 107 L) of helium. Suppose you fill the balloon with helium on the ground, where the pressure is 741 mm Hg and the temperature is 24.4°C. When the balloon ascends to a height of 2 miles, where the pressure is only 600. mm Hg and the temperature is -33°C, what volume is occupied by the helium gas? Assume the pressure inside the balloon matches the external pressure.

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A helium-filled balloon of the type used in long-distance flying contains 420, 000 ft3 (1.2 times 107 L) of helium. Suppose you fill the balloon with helium on the ground, where the pressure is 741 mm Hg and the temperature is 24.4°C. When the balloon ascends to a height of 2 miles, where the pressure is only 600. mm Hg and the temperature is -33°C, what volume is occupied by the helium gas? Assume the pressure inside the balloon matches the external pressure.


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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 Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Staples' class at USM.