For this problem, we have to determine the final volume of the balloon at 1.00 x 10^{2} K

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 temperature. The value

Therefore, the initial and final pressure and volume of the gas are related by **Charles' ****Law**:

$\overline{)\frac{{\mathbf{T}}_{\mathbf{1}}}{{\mathbf{V}}_{\mathbf{1}}}{\mathbf{=}}\frac{{\mathbf{T}}_{\mathbf{2}}}{{\mathbf{V}}_{\mathbf{2}}}}$

The given values are:

T_{1} = **20°C + 273.15 = 293.15 K ** T_{2} = 1.00 x 10^{2} K

V_{1} = **7.00 x 10 ^{2} mL ** V

We can rearrange the combined gas law to solve for V_{2}:

A balloon is filled to a volume of 7.00 x 10^{2} mL at a temperature of 20.0°C. The balloon is then cooled at constant pressure to a temperature of 1.00 x 10^{2} K. What is the final volume of the balloon?

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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 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 Demesa's class at BAYLOR.

What textbook is this problem found in?

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.