Problem: A gas-filled weather balloon with a volume of 65.0 L is released at sea-level conditions of 745 torr and 25°C. The balloon can expand to a maximum volume of 835 L. When the balloon rises to an altitude at which the temperature is −5°C and the pressure is 0.066 atm, will it have expanded to its maximum volume?

FREE Expert Solution

Assuming that the gas is ideal and the number of gaseous moles inside the balloon does not change, the change in volume of gas can be determined using the combined gas law.

 

Where P is pressure

           V is volume

           T is temperature in K


Convert the values in appropriate units

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Problem Details

A gas-filled weather balloon with a volume of 65.0 L is released at sea-level conditions of 745 torr and 25°C. The balloon can expand to a maximum volume of 835 L. When the balloon rises to an altitude at which the temperature is −5°C and the pressure is 0.066 atm, will it have expanded to its maximum volume?

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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 Berg's class at MOORPARK.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.