# Problem: A weather balloon is filled with helium to a volume of 1.61 L at 734 torr. What is the volume of the balloon after it has been released and its pressure has dropped to 0.844 atm? Assume that the temperature remains constant.

###### FREE Expert Solution

A weather balloon is filled with helium to a volume of 1.61 L at 734 torr.

We’re being asked to determine the volume of the gas sample after it has been released and its pressure has dropped to 0.844 atm

Recall that the ideal gas law is:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

The pressure and volume of a gas are related to the number of moles, gas constant and temperatureThe value nRT is constant

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###### Problem Details

A weather balloon is filled with helium to a volume of 1.61 L at 734 torr. What is the volume of the balloon after it has been released and its pressure has dropped to 0.844 atm? Assume that the temperature remains constant.

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 The Ideal Gas Law Derivations concept. You can view video lessons to learn The Ideal Gas Law Derivations. Or if you need more The Ideal Gas Law Derivations practice, you can also practice The Ideal Gas Law Derivations practice problems.

What professor is this problem relevant for?

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

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.