IN 1992 HUBERT ALYEA published an ingenious method for the safe generation of gases, including noxious gases, for classroom use.*  The method utilizes 60 mL disposable plastic syringes.  We began using this approach with our students in our descriptive inorganic laboratory course in 1992 and found the technique to be convenient, easy to use, safe, and reliable. Since 1992, when we first employed this method, we have developed numerous modifications that significantly improve the ease and safety of gas generation using syringes. We also have developed numerous experiments with a variety of gases, most of which are suitable for use as high school and introductory college level microscale laboratory experiments.  All of these experiments and classroom demonstrations have been published in a series of articles that have appeared in Chem13 News from 1996 – present.  This series is collected here in a refined state where all pertinent improvements have been included.  *(Hubert N. Alyea is considered by many to be the “grand-daddy” of chemical demonstrations.  His chemical antics in front of public audiences earned him a reputation that inspired the character in Walt Disney’s The Absent-Minded Professor.  His proposal to use syringes to generate and collect gases is published in J. Chem. Educ., 69 65 (1992)) 

    Laboratory experiments involving gases are almost never included in modern chemistry laboratory books although throughout most of the 19th and 20th centuries the generation and study of gases were integral parts of a college course in chemistry.  The general perception is that gases are hard to see, hard to contain, and hard to use as chemical reagents. The word “gas” causes most teachers to think of expensive lecture bottles that mysteriously become empty without notice and are then impossible to dispose of — or of the drawings in textbooks that show pneumatic troughs and the exotic apparatus with its delivery funnel, round-bottom flask and tubing.  (We won’t mention what students think of when they hear the word “gas.”)  If you are one of the very few individuals who has actually produced and collected a gas in a laboratory setting, it was probably using pneumatic troughs and a method of water displacement that is over 200 years old!(Drawing is from General Chemistry, Harry N. Holmes, Macmillan Company, 1930.)   You may have vivid recollections of tippy inverted test tubes, water soaked lab books, and long rubber tubing that tended to tip over the round-bottom flask filled with bubbling acid. You may shudder at the memories of messy pneumatic troughs and the frustrations and dangers of trying to push long-stem glass funnels through rubber stoppers in order to construct the apparatus. With our microscale gas chemistry techniques, you and your students will learn that gases can be produced cleanly, quickly, and cleverly in completely self-contained reaction chambers (big syringes without needles) while your students watch in awe at the reaction taking place in their own hands in front of their very eyes.

    You are undoubtedly interested in the chemistry of gases or you probably would not own this book.  Here are several reasons why we are “gas enthusiasts”!

Gas Chemistry...

...is fun and easy!  Students find it easy to learn how to prepare gases and do the reactions.  Gas samples are ready in 5 minutes.

...is a source of great labs and great demos!  Students enjoy making gases.  Some of the demonstrations are nothing short of spectacular.

...is visual!  He best way to see a gas is to watch it being produced. 

...is microscale!  It’s microscale in terms of quantities, but large enough to see (60 mL).

...is inexpensive.  It costs less than 1/2 cent to prepare a syringe filled with carbon dioxide.  Other gases are a bit more expensive, but never more than a few cents per syringe full of gas. 

...is green chemistry.  There is little or no chemical waste.  Well over 90% of the experiments have no chemical waste that require professional waste handlers. 

...is a valuable resource for teaching a wide variety of chemistry concepts.  Important concepts of the high school and college chemistry curriculum can be taught with gases.  The emphasis of this book is mostly on the chemical reactions of gases, however, the list of concepts covered includes gas laws, environmental issues (acid rain, air pollution), reaction stoichiometry (limiting reagents, law of combining volume, theoretical yield), intermolecular forces, catalysis, combustion, molar mass as well as more advanced topics such as kinetics and equilibrium.  Experiments involving microexplosions and rocketry are favorites among the students. 

    How do you get started with microscale gas chemistry?  I suggest an easy, “lets-slip-into-this-slowly” approach.  Gas chemistry doesn’t have to be all-or-nothing — it isn’t like changing religions or trying parenthood — it is more like deciding to explore more new places or resolving to try different things.  Keep it easy and fun for yourself.  The students will enjoy these techniques and experiments because they are fun and easy to learn and do. 

    We assume that you have already read the section called "Getting Started".  And now you are reading about the "In-Syringe" method.  Good.  We suggest that you plan to cover the section of this website titled "3 Easy Gases" during the first year that you try microscale gas chemistry.  The first section introduces you and your students to the techniques as you learn to make carbon dioxide from vinegar and baking soda.  The next part contains five easy experiments that can be performed with carbon dioxide.  Next, you and your students prepare hydrogen and perform several reactions with the gas.  The third easy gas is oxygen; you will  make oxygen and study its reaction chemistry.  Each gas takes one or two 40 minute laboratory periods. 

    The next section of the website (Lab Experiments) consist of full period laboratory experiments, some involving data-sharing.  The experiments in these sections are easily performed with the three gases that the students know how to prepare. The experiments can be done in any order. 

    Looking ahead to when you have mastered the 3 easy gases, in the section titled "All 17 Gases", we present experiments for eight other gases that can be made using the "In-Syringe" method.  Also in this section, we introduce you to a new method of generating gases that cannot be prepared by the "In-Syringe" method and we use this new method to made five new gases.  Even microwave ovens can be used to prepare gases.  

    In the section titled "Gas Catalyst Reactions", we describe our Gas Reaction Catalyst Tube and the experiments that can be done with it. 

    But for now, let’s return to learning the most useful "In-Syringe" method for generating gases.  We suggest that learning the technique and using the syringes be given at least one complete laboratory period, perhaps two if you use the video or have a set of rules that need to be covered.  During the first period, you can show your students the equipment and go over the names for everything.  This is a good time to emphasize that there are five small parts that are easy to lose and they must not lose them or (fill in the blank) will happen.  Also during the first lab session, you should demonstrate the technique once or twice (or you could play the video and watch me show how it’s done (order video).  During the second lab period, the students can handle the equipment for the first time and use it to generate carbon dioxide. By the end of the lab period, they will be good at it and will be able to generate a gas sample within five minutes.  And what they don’t know yet is that the same general approach is used to generate quite a few different gases.  Another goal of this first encounter with the syringes is to let your students work through any immature thoughts they may be harboring.  After all, they are working with huge syringes and “making gas”, so there will be the odd deviation from model student behavior.  But that quickly passes.  It will also occur to one or two proportional thinkers that if they use lots of reagents, they could get the plunger to go flying from the barrel.  Well, they are right, however they will soon learn (providing they try this) that the plunger does not go very far at all and they have created a mess.  If this is something they are going to try, it’s best that they try it with baking soda and vinegar.  They will also realize that making the plunger pop out costs them a syringe full of gas and requires them to start all over after cleaning up and enduring your wrath, etc.

THE IN-SYRINGE METHOD FOR PREPARING GAS SAMPLES
    Here we describe the most general method for gas generation, the “In-Syringe Method” and use the method to prepare carbon dioxide.  Originally described by Alyea, the In-Syringe Method features the generation of gases by reacting two chemicals, typically one solid and one aqueous liquid, inside a plastic syringe.  Interestingly, Alyea did not suggest a practical way in which the solid and aqueous reagents should be brought together inside the syringe — he suggested, and I quote, “Into the cap put enough reagent to generate 50 mL of gas.  Drop the cap into the syringe, and immediately fully insert the plunger.” The synthesis of hydrogen sulfide (one of the gases suggested by Alyea) by these exact instructions must have caused quite an annoyance to others working in the same wing of the building!  It is in this area that we have made important contributions by designing a few simple modifications to Alyea’s procedure that assure that the reaction is safely contained within the syringe and exposure to the gases produced is prevented. (The In-Syringe Method was originally described in our first article on microscale gas chemistry that appeared in the October, 1996 issue of Chem13 News (Number 251.))

    The In-Syringe Method is used for generating the following gases:

carbon dioxide, CO2
hydrogen, H2
oxygen, O2
nitric oxide, NO, and nitrogen dioxide, NO2
ammonia, NH3
ethyne, C2H2
sulfur dioxide, SO2
chlorine, Cl2
nitrogen, N2
silane, SiH4
hydrogen sulfide, H2S

Microscale Gas Chemistry Kits
    Each pair of students will need certain equipment in order to prepare gases and perform experiments with the gases.  We recommend organizing this equipment in 8 cup plastic food storage containers.  Each kit should contain:

two 60 mL plastic syringes with a LuerLOK fitting
two Latex LuerLOK syringe caps
two plastic vial caps
one 15 cm length of Latex tubing
one 3 cm length of Latex tubing
one small bottle of silicone oil
one plastic pipet
one clear plastic beverage cup (250 mL/9 oz)
one small plastic weighing dish
one small test tube (12 x 100 mm)
one medium test tube (18 x 150 mm)
one birthday candle

    All of this will fit into the food storage container.  In addition, each pair of students will need a wide-mouth beverage bottle for draining and supporting their syringes.  Ordering information for kit materials is available. 

Suitability
    The preparation of carbon dioxide is suited for either classroom demonstrations or as laboratory experiments conducted by students.  This chapter can be used very early in the first year high school chemistry curriculum.  As a laboratory activity, it is appropriate when discussing matter, chemical compounds, heterogeneous and homogeneous mixtures and physical and chemical changes.  We recommend carbon dioxide as the first gas simply because the chemicals used and the products generated are not dangerous. 

Syringe lubrication options
    We recommend lubricating the black rubber seal of the plunger.  New syringes have been treated with a thin film of silicone oil but this washes off after the first use.  The best lubricants that we recommend are:

Silicone oil. Definitely the lubricant of choice for microscale gas chemistry.  Educational Innovations sells small bottles of silicone oil ideal for student use and Fisher Scientific sells large bottles (500 mL) that can be used to refill small bottles.  Students use only a few drops at a time.

Silicone spray. (available from hardware stores) Easy to use, but messy, also, contains a hydrocarbon propellant that will damage rubber seals after extensive use.  (Petroleum-based lubricants are partially absorbed by the rubber and cause the rubber to expand slightly.  This is irreversible and ruins the syringe after several uses.)

In all instructions intended for students, we only refer to silicone oil. 

Student Instructions
    For classroom use by teachers, one copy per student in the class may be made free of charge and without further permission.  Student instructions and questions only (without teaching tips, suitability information, etc.) can be downloaded free of charge as a Microsoft Word document from the website. Download now.

Answers to the questions, lists of materials and chemicals, and additional reference information.
    This page is fairly similar in content to Chapter 3 in our book Microscale Gas Chemistry.   Our 500-page book includes all of the information included at this website and much more!  Answers to all of the questions, chapter-by-chapter lists of the equipment and chemicals needed to conduct the experiments as classroom demonstrations or laboratory activities for the entire class, construction instructions for various pieces of equipment, information for the preparation of stock solutions, ordering information, and a complete index — are all available in the book, but not at the website.  The book, Microscale Gas Chemistry, can be ordered from Educational Innovations (Part Number BK-590) from  their website.

Inexpensive spatulas
    Cut the top off of a plastic pipet at an angle to make an inexpensive spatula:

THE IN-SYRINGE METHOD FOR PREPARING GAS SAMPLES

GENERATING CARBON DIOXIDE

General Safety Precautions
    Always wear safety glasses.  Gases in syringes may be under pressure and could spray liquid chemicals.  Follow the instructions and only use the quantities suggested.

Toxicity
    Carbon dioxide is a relatively non-toxic gas.  Like all gases other than oxygen, it is a simple asphyxiant if inhaled in very large quantities.  We will not be generating very large quantities of carbon dioxide. 

GETTING STARTED
    Before we start making gases, we need to know a bit more about the equipment that we will use.  Many of the important pieces that we will use are pictured below.  Let’s start with the most dramatic, the large syringe which may invoke pangs of fear and memories of visits to the doctor’s office.  There are no needles, however.  You will notice that after working with these syringes a few times, you will no longer think of them for their medical applications.  (Incidentally, these 60 mL syringes are used by veterinarians to treat large farm animals and are not normally used by medical doctors.) 

---

In-Syringe Method.

Procedure for Generating Gases Inside Plastic Syringes

      The syringe is composed for two major parts — the barrel (outside part) and the plunger (inside part).  Plungers and barrels are interchangeable.  On one end of the plunger you will notice an air-tight black rubber seal.  Even tiny little hydrogen molecules have trouble sneaking past the seal so these are pretty impressive pieces of equipment.

    The next piece of equipment to find are the two syringe caps.  They are made of rubber and fit snugly onto the syringe barrel — again, an air-tight fit.  They are tiny and easily lost, which would be a problem because they are used to keep the gas in the syringe. Keep an eye on them and don’t lose them down the drain.  

    The vial cap is used to lower the solid reagent into the syringe (as discussed below) and is also small and easily lost.  Again, you should have two of them.  The other items in your gas kit will include a long and short piece of tubing, two weighing dishes, a bottle of silicone oil, a plastic pipet, a plastic cup, two test  tubes (two different sizes) and a birthday candle.

MAKING CARBON DIOXIDE
    You are now about to prepare your first gas sample using the syringe equipment. The general strategy of the method is to react two substances in a large syringe.  The limiting reagent is always used in solid form and is placed in a small vial cap.  The second reagent is prepared as an aqueous solution.  For example, you will generate CO2(g) from vinegar, used in excess, and solid baking soda or sodium bicarbonate, NaHCO3. The steps given below eventually will be used to make all sorts of gases.  

1. Wear your safety glasses!

2. Lubricate the seal.
    Lubricate the black rubber seal of the plunger with silicone oil.     

3. Measure out the solid reagent
    (Use 0.21 g NaHCO3 to make CO2)
    Place the solid reagent into the vial cap.  We recommend that the solid be measured directly into the vial cap to prevent losses from transferring small amounts of solids.  

    

4. Fill the syringe barrel with water
    Fill the barrel with water.  Place your finger over the hole to form a seal.  Fill completely to the top.  

   

5. Float the vial cap
    Float the vial cap containing the solid reagent on the water surface.  This is easiest if the syringe barrel is filled completely to the top with water.

     

6. Lower the cap by flotation
    Release the seal made by finger to lower the cap into the syringe barrel without spilling its contents.  Allow the syringe to drain into a wide mouth beverage container.  When successfully completed, the cap should rest upright on the bottom of the syringe with all reagent still in the cap.   

 

7. Install the plunger
    Install the plunger while maintaining the syringe in a vertical position.  The plunger has a plastic “rib” near the rubber seal that snaps past the “catch” — a small ridge just inside the mouth of the syringe.  Usually it takes a firm push to move the rib past the catch.  After that, the plunger should move smoothly.  The plunger should fit snugly against the rim of the vial cap.  

 

8. Draw aqueous reagent into syringe  (Use 5 mL vinegar to make CO2)
    The aqueous reagent, measured into a small weighing dish, is drawn into the syringe while maintaining the vertical position of the syringe.  The vial cap with the solid reagent should float on the solution. 

   

9. Install syringe cap
    Push the syringe into the syringe cap.  It simply pushes on.

    

10. Generate the gas
    The ‘fun’ part is generating the gas and you are ready to do that now.  Shake the syringe up and down in order to mix the reagents.  As the liquid reagent splashes into the vial cap, gas generation will commence and the syringe plunger should move outward.  It is sometimes necessary to gently help the plunger move up the barrel.

     

11. Remove cap to stop gas collection
    After the plunger has reached the desired mark (usually 50 mL), tip the syringe so that it is positioned with plunger downward and syringe cap upward.  Carefully remove the syringe cap assuming that the syringe may be under positive pressure.  (“Burp that baby with its head up!”)  

 

12. Discharge reagents
    Turn the syringe 180º and discharge the liquid reagent into the plastic cup.    Caution: Never remove the syringe cap with the cap end of the syringe directed downward:  Reagents will spray out of the syringe.  Immediately cap the syringe with the syringe cap to prevent loss of gas by effusion.   

   

13. Wash away contaminants
    The gas-filled syringe may be "washed" in order to remove traces of unwanted chemicals from the inside surfaces of the syringe before the gas is used in experiments.  To wash a gas:

1. Remove the syringe cap,
2. draw 5 mL water into the syringe (shown below),
3. cap the syringe,
4. shake syringe to wash inside surfaces,
5. remove cap,
6. discharge water only, and finally
7. recap the syringe.
8. Repeat?

Repeat these washing steps if necessary.
(All traces of the reactants should be washed away.)

OTHER USEFUL GAS SYRINGE TECHNIQUES

    There are a several other techniques that come in handy when working with gases in syringes.  Here are the most important ones.  Try to use these techniques as much as possible. 

A. Syringe-to-syringe transfer procedure
    This procedure is useful under several circumstances.  For example, when a gas sample needs to be in a clean, dry syringe, simply transfer the gas sample by a short connecting tube between  the two syringes. 

1. Connect a short piece of tubing to a clean syringe.

2. Connect gas-filled syringe to tubing:

3. Transfer the gas with clean, dry syringe on top:

   

B. Controlled discharge of gas from a syringe
    Plungers do not always move smoothly in their syringe barrels.  As a result, gases may be discharged in large unintended portions (such as 40 mL all at once) if the method shown in the left diagram below is used.  Instead, grasp the syringe by its plunger (right figure) and pull the barrel towards your hand.  This simple technique will give you excellent control of gas delivery. 
 

INCORRECT WAY: 
 

CORRECT WAY:

C. Discharging a specific volume of gas
    Position thumb as a “stop” to discharge desired volume of gas and then push inward. 

 

 
D. Safety First!  Cap Up-and-Off!
    If more than 60 mL gas is going to be generated, follow these steps.

1. Position the syringe so the cap is directed upward.
2. Remove the cap by twisting. 

 

3. Discharge the solution to prevent further gas collection.  Recap syringe.

 

Clean-up and storage
    At the end of the experiments, clean the syringe parts, caps and tubing with soap and water.  Use plenty of soap to remove oil from the rubber seal.  This extends the life of the plunger.  It may be necessary to use a 3 cm diameter brush to clean the inside of the barrel.  Rinse all parts with distilled water.  Be careful with the small parts because they can easily be lost down the drain.  Important: Store plunger out of barrel unless both are completely dry.


Disposal
    Unwanted CO2(g) samples can be safely discharged into the room.


Introductory Questions

1. Write the formulas for (a) baking soda; (b) vinegar; and (c) carbon dioxide.

2. Gases usually have “(g)” as the last part of their formula.  For example, oxygen gas would be written as O2(g).  In a similar way, solids have “(s)” and liquids have “(l)”.  Aqueous solutions, substances dissolved in water, have “(aq)” as the last part of their formula.  For example, salt water would written as NaCl(aq).  Add these endings to the three formulas in Question 1.

3. Why should the gas be “washed”?

4. Why is it important to use only the specified amounts of reagents? 

5. Why must the syringe be upright when removing the cap?

Questions

6. What was the purpose of vigorously shaking the syringe? 

7. Why must one start over if some of the solid spills out while the vial cap of sodium bicarbonate is being lowered?

8. What is the molar mass of carbon dioxide? 

Advanced Questions

9. Write the balanced chemical equation for the reaction occurring in your syringe.

10. Using 0.22 g of NaHCO3 and 5.0 mL of 1.0 M HCl, which reactant is the limiting reactant?

11. Use the ideal gas law and your answer to the previous question to determine the volume of gas is predicted.  Assume 25 ºC and standard pressure.

12. Use the ideal gas law to determine the density of carbon dioxide at 25 ºC and standard pressure. 

13. Use the ideal gas law to determine the density of air at 25 ºC and 1 atm pressure.  You can use the “average molar mass of air” in your calculations; its value is 28.964 g/mol.  Compare the density of carbon dioxide (Question 7)  with the density of air.  Calculate the ratio of densities, d_{carbon dioxide}/d_air