Name: dumas method for gas analysis
Uploaded: 2020-03-26T07:22:24.000Z
Duration: 5 min 54 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

NC K-12 Science Standard Course of Study

9-12

Chemistry

Energy

PS.Chm.7.3

Ideal Gas Law

<ul><li><a href="#" data-time="0.0">Preparation of the Laboratory
</a></li><li><a href="#" data-time="0.0">Preparation and Dispensing of Unknown Liquids
</a></li></ul>

ideal gas law

<p>Source: Smaa Koraym at Johns Hopkins University, MD, USA</p>
<ol class="note-items">
	<li data-note-item="1" data-parent-collapse="">Preparation of the Laboratory<button class="expand">Expand</button>
	<p><em>Here, we show the laboratory preparation for 10 students working in pairs, with some excess. Please adjust quantities as needed.</em></p>
	<ul class="lab-items">
		<li data-sub-note-item="1-2">
		<div class="lab-step">Put on a lab coat, splash-proof safety glasses or goggles, and appropriate gloves for the chemicals you will be handling.</div>
		</li>
		<li data-sub-note-item="1-3">
		<div class="lab-step">The day before the lab, place the Dumas tubes in an oven at 125 &#176;C.</div>
		</li>
		<li data-sub-note-item="1-4">
		<div class="lab-step">Two hours before the lab, remove the tubes from the oven and place them on a heat-resistant surface to cool. Distribute the tubes to each workstation once they have reached room temperature.</div>
		</li>
		<li data-sub-note-item="1-5">
		<div class="lab-step">Place a barometer in an easily accessible location.</div>
		</li>
		<li data-sub-note-item="1-6">
		<div class="lab-step">Set a plastic 250-mL beaker next to each analytical balance, and ensure that a box of laboratory wipes is available for each balance.</div>
		</li>
		<li data-sub-note-item="1-7">
		<div class="lab-step">Set up a Bunsen burner in a fume hood, and place a striker and a test tube holder with the burner.</div>
		</li>
		<li data-sub-note-item="1-8">
		<div class="lab-step">Set out the following glassware and equipment at each workstation (we suggest students work in pairs):
		<table align="center" height="224" style="border-collapse: collapse; font-size: 17px; line-height: 24px;">
			<tbody>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;500-mL Erlenmeyer flask</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;500-mL B&#252;chner flask</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;400-mL beaker</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;100-mL beaker</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;Lab stand</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;3-prong clamp</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;Ring fixture with square of wire gauze</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;Bunsen burner and fire striker</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;2&#160;&#160;&#160;&#160;18-in length of latex tubing</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;18-in length of silicone tubing</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;Thermometer and thermometer clamp</td>
				</tr>
				<tr>
					<td style="border: 1px solid; padding: 0px;">&#160;1&#160;&#160;&#160;&#160;Single-hole #4 rubber stopper</td>
				</tr>
			</tbody>
		</table>
		</div>
		</li>
	</ul>
	</li>
	<li data-note-item="2" data-parent-collapse="">Preparation and Dispensing of Unknown Liquids<button class="expand">Expand</button>
	<ul class="lab-items">
		<li data-sub-note-item="2-1">
		<div class="lab-step">Label one 50-mL glass bottle and one 20-mL glass syringe as &#39;deionized water&#39;.</div>
		</li>
		<li data-sub-note-item="2-2">
		<div class="lab-step">Label three 50-mL brown glass bottles, three 5-mL glass syringes, and three 25-mL glass beakers as &#8216;1&#8217; through &#8216;3&#8217;, and set them in a reserved fume hood.</div>
		</li>
		<li data-sub-note-item="2-3">
		<div class="lab-step">Place a watch glass and 20-mL volumetric pipette next to each numbered bottle along with a pipetter. Set four 22-gauge, 6-in needles next to each syringe.</div>
		</li>
		<li data-sub-note-item="2-4">
		<div class="lab-step">Group the glassware by label in a reserved fume hood according to their chemical compound: 1,2-dichloroethane, trichloroethylene, and 2-bromopropane.</div>
		</li>
		<li data-sub-note-item="2-5">
		<div class="lab-step">Transfer at least 20 mL of each organohalide into its assigned bottle using a volumetric pipette: 1,2-dichloroethane in bottle 1, trichloroethylene in bottle 2, and 2-bromopropane in bottle 3. Cap each bottle once the liquid has been added.</div>
		</li>
		<li data-sub-note-item="2-6">
		<div class="lab-step">Label a fifth 50-mL bottle, 5-mL glass syringe, and 25-mL beaker as &#39;acetone&#39;, and set a 22-gauge, 6-in needle next to the syringe.</div>
		</li>
		<li data-sub-note-item="2-7">
		<div class="lab-step">Add about 20 mL of acetone in the appropriately labeled bottle and cap it.</div>
		</li>
		<li data-sub-note-item="2-8">
		<div class="lab-step">When it is time to dispense the unknown liquids during the laboratory, pour at least 5 mL of an unknown into the matching beaker. Submerge the tip of the matching syringe in the unknown and slowly withdraw the plunger to fill the syringe to the 5-mL mark. Connect the needle and set down the syringe on a weight paper. Cover the beaker with a watch glass after filling.</div>
		</li>
		<li data-sub-note-item="2-9">
		<div class="lab-step">Repeat this process for each organohalide.</div>
		</li>
		<li data-sub-note-item="2-10">
		<div class="lab-step">Call up each student group one by one. Insert the needle of the syringe with their assigned unknown liquid into the long neck of the Dumas tube and dispense 0.5 mL. Withdraw the needle, taking care to avoid letting the liquid drip on the outside of the tube. The student group can now begin their trial.</div>
		</li>
		<li data-sub-note-item="2-11">
		<div class="lab-step">Dispense the unknowns for the rest of the lab in this way, refilling the syringes as needed. At the end of the lab, follow the same procedure to dispense 0.5 to 1 mL of acetone into each tube for cleaning by students. The amount of acetone will depend on the amount of water left over in the tube.</div>
		</li>
		<li data-sub-note-item="2-12">
		<div class="lab-step">If students need to re-weigh their empty Dumas tube in the middle of the experiment, you will flame dry the tube so that they can obtain an accurate measurement.</div>
		</li>
		<li data-sub-note-item="2-13">
		<div class="lab-step">Light a Bunsen burner and hold the Dumas tube with a test tube holder, and pass the tube through the flame until it appears dry. <strong>Note: </strong>Three of the organohalides are flammable, so keep the opening of the tube away from the flame.</div>
		</li>
		<li data-sub-note-item="2-14">
		<div class="lab-step">Then, hold the tube away from the flame for 1 min to allow any remaining vapor to condense. If you see liquid at the bottom of the tube after that, pass the tube through the flame again until it appears dry. Once no liquid condenses in the tube after one minute out of the flame, return the tube to the student group so that they can measure the mass.</div>
		</li>
	</ul>
	</li>
</ol>

<div class="section-question"><h4 class="question-sect">What is a gas? </h4><p>A gas is a fundamental state of matter that is a collection of molecules with significant distance between them. Gases are highly compressible and are the least dense state of matter.
</p></div><div class="section-question"><h4 class="question-sect">What is the relationship between pressure, volume, number of moles, and temperature? </h4><p>Pressure and volume are inversely proportional to each other, volume and temperature are proportional to each other, pressure an...

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of the LaboratoryExpand
	Here, we show the laboratory preparation for 10 students ...

Education

JoVE Lab Manual

Lab Manual Sub Articles

dumas method for gas analysis

<p class="jove_content">The Dumas method measures an unknown liquid by turning it into vapor and using gas behavior to analyze the sample. In this lab setup, students work in pairs with Dumas tubes, balances, and a thermometer to carry out the trial safely and consistently.</p>

<p class="jove_content">Before the lab begins, the Dumas tubes are placed in an oven at 125 °C the day before. Two hours before class, the tubes are removed and allowed to cool on a heat-resistant surface until they reach room temperature. A barometer is kept nearby, and each balance has a plastic beaker and laboratory wipes ready for use.</p>

<p class="jove_content">Each workstation also includes the glassware and hardware needed for the experiment. That set includes an Erlenmeyer flask, a Büchner flask, beakers, a lab stand, clamps, a ring fixture with wire gauze, a Bunsen burner with striker, latex and silicone tubing, a thermometer with clamp, and a single-hole #4 rubber stopper. The burner is set up in a fume hood, and students are expected to wear a lab coat, splash-proof safety glasses or goggles, and gloves.</p>

<p class="jove_content">The unknown liquids are prepared ahead of time in labeled containers. Deionized water is set aside in one bottle and one syringe. Three brown bottles, three syringes, and three beakers are labeled 1 through 3 for 1,2-dichloroethane, trichloroethylene, and 2-bromopropane. A fifth bottle, syringe, and beaker are labeled acetone for the cleanup step at the end of the lab.</p>

<p class="jove_content">During the experiment, at least 5 mL of each unknown is placed in the matching beaker. The liquid is drawn into the labeled syringe to the 5-mL mark, and the needle is attached before the syringe is set on weight paper. Each student group receives 0.5 mL of its assigned unknown through the long neck of the Dumas tube, and the outside of the tube is kept dry so the mass reading stays accurate.</p>

<p class="jove_content">If a group needs to weigh the empty Dumas tube again, the tube is flame-dried first. The tube is passed through a Bunsen burner flame until it looks dry, while keeping the opening away from the flame because three of the organohalides are flammable. The tube is then held away from the flame for 1 minute so any remaining vapor can condense. If liquid is still present, the drying step is repeated before the tube is returned for measurement. At the end of the lab, 0.5 to 1 mL of acetone is dispensed into each tube to help students clean the apparatus.</p>

Dumas Method for Gas Analysis

The Dumas method measures an unknown liquid by turning it into vapor and using gas behavior to analyze the sample. In this lab setup, students work in pairs with Dumas tubes, balances, and a thermometer to carry out the trial safely and consistently.<br /><br />Before the lab begins, the Dumas tubes are placed in an oven at 125 °C the day before. Two hours before class, the tubes are removed and allowed to cool on a heat-resistant surface until they reach room temperature. A barometer is kept nearby, and...

Molar Mass by the Dumas Method

The Dumas method uses the ideal gas law to estimate the molar mass of an unknown liquid. In this lab, a Dumas tube is filled with vapor from a volatile sample, then cooled so the vapor condenses. Because molar mass does not change with phase, the mass of the condensed liquid can be used to find the molar mass of the vapor.<br /><br />The unknown liquids are volatile, toxic, and may be flammable, so the work is done in a fume hood. Students wear a lab coat, safety glasses, and two pairs of nitrile gloves...

lab manual sub articles

Prepare and run a Dumas method lab with unknown liquids, Dumas tubes, safe heating steps, and cleanup using acetone for high school students.

Dumas Method for Gas Analysis | JoVE K12

Virginia  Standards of Learning

HIgh School

CH.6

CH.6.b

Arizona Science Standards

High School

Physical Science

HS+C.P1

HS+C.P1U1.3

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-9.

<p>A gas is simply a dispersed sample of matter that is fluid and expands freely to occupy available space. However, a certain number of gas molecules occupy a specific volume under a defined temperature and pressure. We can describe the behavior of a gas under these parameters using the ideal gas law, which uses the universal gas constant, R, to relate all of these variables.</p>
<p>The universal gas constant is equal to 8.314 joules per mole Kelvin. This equation enables us to understand state relationships in a gaseous system. For example, in a system of constant temperature and pressure, we know that the addition of more moles of gas results in an increase in volume. Similarly, we can look at a system of constant temperature and moles and see that a decrease in volume results in an increase in pressure.</p>
<p>One challenge is that the ideal gas law describes gases behaving ideally. So what do we mean by that? Ideal behavior assumes that first, the molecules themselves are infinitesimally small and essentially have no volume and that the distance between the molecules is significantly larger than the size of the individual molecule.</p>
<p>Second, we assume that the molecules are constantly in motion.</p>

gas laws behind the ideal gas equation

<p class="jove_content">The ideal gas equation brings together the main gas laws used in chemistry. Gases have molecules that are far apart, so their behavior is described with four measurable variables: pressure, volume, number of moles, and temperature. The ideal gas law links these variables with the gas constant, R, which equals 8.314 J·K−1 mol−1.</p>

<p class="jove_content">Boyle’s law describes the link between pressure and volume. When temperature and the number of moles stay constant, pressure and volume change in opposite directions. Charles’s law shows the direct relationship between a gas’s volume and temperature when pressure and moles are constant. Gay-Lussac’s law connects pressure and temperature in an enclosed gas at constant volume and constant moles.</p>

<p class="jove_content">Avogadro’s law adds the relationship between volume and the number of moles. It states that equal volumes of two gases contain equal numbers of molecules when temperature and pressure are the same. These ideas were combined into the ideal gas law, first proposed by Emile Clapeyron in 1834, to create one equation for gas behavior.</p>

<p class="jove_content">The ideal gas law uses a simple model of gas particles. It assumes elastic collisions, frictionless motion, very small molecular volume, no intermolecular forces, and constant motion with large spaces between molecules. Because of these assumptions, an ideal gas would not form a liquid at room temperature, but many real gases do. Those gases can deviate from ideal behavior.</p>

<p class="jove_content">Johannes D. Van der Waals changed the ideal gas law in 1873 to better fit real gases. His equation includes constants a and b, which account for molecular size and intermolecular forces. The value of a is larger for gases with strong intermolecular forces, such as water, and smaller for gases with weak intermolecular forces, such as inert gases. The value of b represents the volume occupied by 1 mole of gas molecules, and lower b values raise the pressure.</p>

<p class="jove_content">The ideal gas law also helps explain the Dumas method, which was developed by Jean Baptiste Andre Dumas to find the molar mass of an unknown gas sample. A Dumas tube is a long glass bulb with a capillary neck. A volatile compound is placed in the tube, then heated in boiling water so it vaporizes and pushes air out. When the tube cools, the vapor condenses, and the mass of the liquid equals the mass of the gas that filled the tube.</p>

<p class="jove_content">Using the known mass, volume, room pressure, and water bath temperature, the moles and molecular weight of the gas can be calculated with the ideal gas law. The method assumes that the vapor behaves ideally, that the tube volume does not change between room temperature and working temperature, and that the gas and water bath reach thermal equilibrium.</p>

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Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Determining the Mass of the Unknown LiquidExpand
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Dumas Method for Gas Analysis

Learning Objectives

What is a gas?

What is the relations...

Lab Prep

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