<p>Hey guys can you explain the answers to the following two questions for me please? I'd really appreciate it!</p>
<ol>
<li>The following mistakes were made when carrying out the "Determination of the Molar Mass of Volatile Liquids" experiment. What effect does eac hahve on the calculated molar mass? Be specific. For example, too large because...</li>
</ol>
<p>a. Only part of the pipet was immersed in the boiling water, so the temperature in part of the pipet was less than that of the water bath.</p>
<p>b. The mass of the condensed liquid was not determined quickly. Instead, the pipet was allowed to stand for a while before immersing it in room temperature water and then massing the pipet. </p>
<p>Yea it’s a lab. It’s called “determination of the molar mass of volatile liquids”</p>
<p>basically, the purpose is to determine the molar masses of various volatile liquids. The liquids are volatilized and condensed in a fixed volume. The condensed volume is massed and the liquid’s molar mass is calculated from the experimental data. </p>
<p>The ideal gas law is used to determine the molar masses of gases and volatile liquids. </p>
<p>The molar msses of several volatile liquids with boiling points well below the boiling point of wtaer are determined. A small sample of the liquid is placed in a tared 15-mL pipet and the piept is then heated in boiling water to vaporize the liqudi. The air and excess vapor escape, leaving the pipet filled only w/ the volatile liquid vapor at atmospheric pressure and at the temperature of boiling water. The pipet is then removed and cooled to condense the vapor.
Once cooled, the pipet is weighed. By massing the same pipet filled with deionized water, the volume of the pipet is calculated. The molar mass of the volatile liquid is then determined from Equation 3 using the mass of the condensed vapor, the volume of the pipet, the atmospheric pressure, and the temperature of the boiling water.</p>