Problem: A sealed balloon is filled with 1.00 L helium at 23°C and 1.00 atm. The balloon rises to a point in the atmosphere wherethe pressure is 220. torr and the temperature is -31°C. What is the change in volume of the balloon as it ascends from1.00 atm to a pressure of 220. torr?

FREE Expert Solution

We are looking for the change in volume and to solve that we would need initial and final values for volume. We are only given the initial volume so we'd have to solve for the final Volume first.

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Problem Details

A sealed balloon is filled with 1.00 L helium at 23°C and 1.00 atm. The balloon rises to a point in the atmosphere where
the pressure is 220. torr and the temperature is -31°C. What is the change in volume of the balloon as it ascends from
1.00 atm to a pressure of 220. torr?

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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.

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Based on our data, we think this problem is relevant for Professor Marin's class at UCF.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.