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Gas Laws: Summary
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<strong><font size="5" color="#FFFFFF" face="Verdana, Arial, Helvetica, sans-serif">Gas
Laws:</font></strong><font size="5" color="#FFFFFF" face="Verdana, Arial, Helvetica, sans-serif">
Summary</font>
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<font size="4" face="Verdana, Arial, Helvetica, sans-serif">A
careful scientist looks at something as complex as the Gas Laws by
looking at a single variable and seeing how other variables
influence it. In the experiments with the model gas you should have
been able to see how volume depends on pressure, if you hold the
number of molecules and the temperature constant. Similarly, you
could figure out how volume depends on temperature if you hold the
number of molecules and the pressure constant. These are just two of
the experiments. So, let's return to real-world experiments and see
how understanding the gas behavior can explain what has happened in
the pictures below. </font>
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<img src="balloon1.gif">
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<img src="balloon2.gif">
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<font size="6">❶</font> A flask containing very cold liquid
nitrogen is prepared to be poured on a balloon.
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<font size="6">❷</font> The liquid nitrogen is poured.
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<img src="balloon3.gif">
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<img src="balloon4.gif">
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<font size="6">❸</font> The balloon looks almost flat.
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<font size="6">❹</font> As the liquid nitrogen evaporates
the balloon re-inflates.
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<i><font size="2">Image credits: Ed O'Sullivan </font></i>
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<strong><font size="4" face="Arial, Helvetica, sans-serif">Which
relationship of the following best explains this experiment?</font></strong>
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V-P relationship
T-V relationship
T-P relationship
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<strong><font size="4" face="Arial, Helvetica, sans-serif">Explain why the
balloon shrank and then expanded in this experiment.</font></strong>
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<strong><font size="4" face="Arial, Helvetica, sans-serif">List two ways
you can increase the pressure in a container with a fixed volume and
explain why this causes a pressure increase. </font></strong>
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<strong><font size="4" face="Arial, Helvetica, sans-serif">SCUBA tanks
have to be built to withstand very high pressure because many gas
molecules are put inside them. Why would putting more molecules inside
cause high pressure?</font></strong>
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<strong>You have reached the end of the activity.<br>Please submit a
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Gas Laws
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