Question

<p>In Sample Exercise 10.16 in the textbook, we found thatone mole of Cl2 confined to 22.41L &#160;at 0C deviatedslightly from ideal behavior. Calculate the pressure exerted by1.00 mol Cl2 &#160;confined to a smaller volume, 3.00 L, at 25C.<br />a) Use the ideal gas equation.<br /><br/>b) Use van der Waals equation for your calculation. (Valuesfor the van der Waals constants are a = 6.49 , &#160; b&#160;= 0.0562 .)<br /><br />c) Why is thedifference between the result for an ideal gas and that calculatedusing van der Waals equation greater when the gas is confined to3.00L &#160;compared to 22.4 L?</p>
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<p>I figured out parts a and b, but i'm not sure about partc.&#160;</p>