Question

A collapsible balloon for carrying meteorological testing instruments aloft is partly filled with 626 liters of helium, measured at $25^{\circ} \mathrm{C}$ and 756 torr. Assuming the volume of the balloon is free to expand or contract according to changes in pressure and temperature, what will be its volume at an altitude where the temperature is $-58^{\circ} \mathrm{C}$ and the pressure is 0.641 atm?

Name: Problem 43, Chapter 4: Introductory Chemistry: An Active Learning Approach
Uploaded: 2020-10-25T03:30:25-08:00
Duration: 1 min 34 s
Channel: Shashika Bandara
Description: A collapsible balloon for carrying meteorological testing instruments aloft is partly filled with 626 liters of helium, measured at 25^∘ C and 756 torr. Assuming the volume of the balloon is free to expand or contract according to changes in pressure and temperature, what will be its volume at an altitude where the temperature is -58^∘ C and the pressure is 0.641 atm?

   A collapsible balloon for carrying meteorological testing instruments aloft is partly filled with 626 liters of helium, measured at $25^{\circ} \mathrm{C}$ and 756 torr. Assuming the volume of the balloon is free to expand or contract according to changes in pressure and temperature, what will be its volume at an altitude where the temperature is $-58^{\circ} \mathrm{C}$ and the pressure is 0.641 atm?

Introductory Chemistry: An Active Learning Approach

Mark S. Cracolice,… 3rd Edition

Chapter 4, Problem 43

Instant Answer

Solved by Expert Shashika Bandara

10/25/2020

Step 1

We do this by adding 273 to the Celsius temperature. So, the initial temperature $T_1$ is $25^{\circ} \mathrm{C} + 273 = 298 \, \mathrm{K}$ and the final temperature $T_2$ is $-58^{\circ} \mathrm{C} + 273 = 215 \, \mathrm{K}$. Show more…

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A collapsible balloon for carrying meteorological testing instruments aloft is partly filled with 626 liters of helium, measured at $25^{\circ} \mathrm{C}$ and 756 torr. Assuming the volume of the balloon is free to expand or contract according to changes in pressure and temperature, what will be its volume at an altitude where the temperature is $-58^{\circ} \mathrm{C}$ and the pressure is 0.641 atm?

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Key Concepts

Ideal Gas Law

The ideal gas law (PV = nRT) relates the pressure, volume, and temperature of an ideal gas, providing a fundamental framework for understanding how gases behave under different conditions. In problems where the amount of gas remains constant, this law helps predict changes in one parameter when the other two are varied.

Combined Gas Law

The combined gas law is a derivation from the ideal gas law that applies when the number of moles is constant. It integrates Boyle's law and Charles's law, allowing the prediction of a gas's new volume when both its pressure and temperature change.

Unit Conversions in Thermodynamics

In thermodynamic calculations, it is essential to work with consistent units. This includes converting temperatures to Kelvin for accurate computation in the gas laws and converting pressures into the same units where necessary, ensuring proper application of formulas.

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