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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro
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Solved: In a common classroom demonstration, a balloon is filled with air and submerged

Chapter 11, Problem 127P

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QUESTION:

In a common classroom demonstration, a balloon is filled with air and submerged into liquid nitrogen. The balloon contracts as the gases within the balloon cool. Suppose the balloon initially contains 2.95 L of air at \(25.0^{\circ} \mathrm{C}\) and a pressure of 0.998 atm. Calculate the expected volume of the balloon upon cooling to \(-196^{\circ} \mathrm{C}\) (the boiling point of liquid nitrogen). When the demonstration is carried out, the actual volume of the balloon decreases to 0.61 L. How well does the observed volume of the balloon compare to your calculated value? Can you explain the difference?

Equation Transcription:

25.0°C

-196°C

Text Transcription:

25.0 degree C

-196 degree C

Questions & Answers

QUESTION:

In a common classroom demonstration, a balloon is filled with air and submerged into liquid nitrogen. The balloon contracts as the gases within the balloon cool. Suppose the balloon initially contains 2.95 L of air at \(25.0^{\circ} \mathrm{C}\) and a pressure of 0.998 atm. Calculate the expected volume of the balloon upon cooling to \(-196^{\circ} \mathrm{C}\) (the boiling point of liquid nitrogen). When the demonstration is carried out, the actual volume of the balloon decreases to 0.61 L. How well does the observed volume of the balloon compare to your calculated value? Can you explain the difference?

Equation Transcription:

25.0°C

-196°C

Text Transcription:

25.0 degree C

-196 degree C

ANSWER:

Solution 127P

This has to do with Charles Law that states volume is proportional to temperature (if one goes up the other one does and vice versa).

The formula you must use is

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