Mean-Green Demos by Dr. Diana Mason

8/8/2019 Mean-Green Demos by Dr. Diana Mason

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MEAN-GREEN

DEMOS

presented by

Dr. Diana Masonand

The Mean GreenChemistry Demo Team



Safety Guidelines

1. GOGGLES MUST BE WORN AT ALL TIMES.

2. Individuals participating in demonstrations must be dressed appropriately.Appropriate clothing includes: closed toe shoes and long pants. It is also suggested

that participants have on a lab coat for additional protection.

3. It is suggested that latex gloves be worn when handling strong oxidizers. (e.g.,sulfuric acid, 30% hydrogen peroxide, and potassium chlorate)

4. Gloves (e.g., heavy duty work gloves or ZetexTM

gloves) MUST be worn when

handling dry ice or liquid nitrogen.

5. A fire extinguisher MUST be readily available throughout demonstrationscontaining potential fire hazards in case of fire.

6. The audience should be directed to use “elephant ears” for demonstrations

containing loud noises to deflect intense noises from their ears without potentialdamage of their eardrums. The exhibitor should darn ear protection during the

demonstration.

7. The audience should be made aware of all exits from the demonstration chamber with the intent of allowing them to exit safely upon the event of an unforeseen

major accident.

8. In the event of a chemical spill in one of the following scenarios, the followingshould be adhered to

a. Spill on an individual – Rinse the affected area with excessive amount of water.

b. Acid spill – Use sodium bicarbonate to neutralize the acid and then clean thespill up using copious amounts of water.



Exploding BalloonsDiana Mason, PhD

July 2003

Materials

4 helium quality Balloons of different color

String

Gases

Hydrogen

Helium

Oxygen

Blowtorch or candle, yardstick and lighter

Preparation

1. Fill 1st balloon with oxygen

2.

Fill 2nd balloon with helium3. Fill 3rd balloon with hydrogen

4. Fill 4th balloon _ full with oxygen and then add hydrogen until balloon begins to float. Note: Since

hydrogen is less dense than air, the balloon containing O2 will rise considerably only when the

correct stoichiometric ratio is “good”.

Demonstration

Light each balloon using either a blowtorch or a candle taped to a yardstick.

Possible Topics to Discuss

Historic significance:

The dirigible Hindenberg was launched during WWII times when Germany and the US were at war. In

order for a dirigible to float it is necessary that it be filled with a gas that is lighter than air leaving hydrogen

and helium as the two options. During the war and to this date the US maintains the largest supply of helium

with one of the primary sources being located in Amarillo, TX, and therefore the Germans were forced to

utilize their other option, hydrogen. Hydrogen by itself is not flammable but when mixed with the oxygen in

the air becomes the fuel for fire. The Hindenberg is a result of this principle. Today all dirigibles like the

Goodyear blimp are filled with helium.

Density importance:

Oxygen is heavier than air whereas hydrogen and helium are lighter than air.

Flame triangle:

It takes three things to cause fire: fuel, oxygen, and a source of activation energy.

Hazards

Helium quality balloons are not leak proof.

Static electricity can potentially supply the necessary activation energy to cause the balloons to explode.

Journal of Chemical Education, Vol 80, No. 7, July 2003.

Disposal

None, except the clean-up of balloon pieces.



Color is a Many Splendid Thing(Briggs-Rauscher Oscillating Clock Reaction)

Diana Mason, PhD

July 2003

Materials

30% Hydrogen peroxide

Distilled water

Potassium iodate

Malonic acid

Manganese(II) sulfate monohydrate

Concentrated sulfuric acid

Soluble starch

Sodium Thiosulfate

Magnetic stirrer

4 – Magnetic stirring bars

Stirring bar remover 1 – 4000 mL-beaker

3 – 1500 mL-beaker

3 – 500 mL-beaker

1 – 150 mL-beaker

1 – 10 mL-pipette (0.1 mL divisions)

Pipette bulb

1 – 500 mL-graduated cylinder

3 – 250 mL-graduated cylinder

Preparation

Prepare the following 3 solutions.

Solution A. In a 1500 mL-beaker, dilute 410 mL of 30% hydrogen peroxide by adding 590 mL of distilled

water.

Solution B. In a 1500mL-beaker, dissolve 43 g of potassium iodate in about 800 mL of distilled water and

4.3 mL of concentrated sulfuric acid. Add distilled water to mixture until the total solution equals 1000 mL.

Solution C. (This solution must be freshly prepared for the reaction to work effectively.)

Part 1 – Dissolve 16 g of malonic acid and 3.4 g of manganese (II) sulfate monohydrate using 500

mL of distilled water contained in a 1500 mL-beaker.

Part 2 – In a 150 mL-beaker, dissolve 3 g of soluble starch in 100 mL of boiling distilled water.

Part 3 – Pour the solution from part 2 into the beaker containing part 1 and dilute mixture until total

volume equals 1000 mL.

Demonstration

Pour solutions A, B, and C into a 4000 mL-beaker. The reaction will begin to oscillate from clear to amber to

blue-black once all ingredients are combined. To increase the speed of the reaction, stir the solution using a

stir plate and stir bar.


The Briggs-Rauscher Reaction is:

IO3- + 2H2O2 + CH2(CO2H)2 + H+

Æ ICH(CO2H)2 + 2O2 + 3H2O



and is really combined of the two components:

IO3- + 2H2O2 + H+

Æ HOI + 2O2 + 2H2O (A)

HOI + CH2(CO2H)2Æ ICH(CO2H)2 + H2O (B)

The first of these two reactions can occur via two different processes: a radical and a non-radical process. Thefactor determining which of these processes occur, is the concentration of iodide ions. At low iodide

concentrations, the radical process dominates the reaction, whereas, at high iodide concentrations, the non-

radical process is the dominant method. The dramatic color effects are the result of one of these processes,

radical or non-radical, reacting with reaction B. When the solution contains a low iodide concentration due to

reaction A occurring by a radical process, the solution will have an amber color. The blue-black color occurs

when the non-radical process of reaction A reacts with reaction B, therefore, the solution contains a higher

iodine content and a lower HIO content.

The following diagram (found at http://chemlearn.chem.indiana.edu/demos/TheOsci.htm illustrates this a fore

mentioned concept.

Hazards

Handle 30% hydrogen peroxide and concentrated sulfuric acid only when wearing gloves. 30% hydrogen

peroxide is corrosive and is a strong oxidizing agent and therefore, contact with skin should be avoided.

Concentrated sulfuric acid can cause severe burns and is a powerful dehydrating agent. If either of these

chemicals comes in contact with skin, rinse area thoroughly with excessive amounts of water. Additionally,

the sulfuric acid spill can be treated with sodium hydrogen carbonate to help neutralize in residual acid after

the skin has been rinsed.

Disposal

Add sodium thiosulfate in small quantities to the Briggs-Rauscher solution while stirring until the solution becomes pale yellow. Caution: this reaction is highly exothermic and the effervescent chemicals produced

can burn you. After the reaction cools, the neutralized mixture may be poured down the sink drain and all

glassware washed thoroughly.



Statue of Liberty(Chemiluminescence)

Diana Mason, PhDJuly 2003

Materials

1 - 4000 mL-beaker

2 - 1000 mL-Erlenmeyer flask 2 – Rubber stoppers to fit Erlenmeyer flasks

Tygon®

tubing (about 6’)Funnel or something similar

4.0 g sodium carbonate (anhydrous)3 L distilled water

0.2 g luminol (3-aminophthalyhdrazide)24.0 g sodium bicarbonate

0.5 g ammonium carbonate monohydrate0.4 g copper(II) sulfate pentahydrate or 0.25 g copper(II) chloride dihydrate

50 mL 3% hydrogen peroxide

Preparation

Solution A: In a 1000 mL-Erlenmeyer flask, dissolve 4.0 g of sodium carbonate in

approximately 500 mL of distilled water. To this solution add 0.2 g luminol and stir todissolve. Next dissolve 24.0 g sodium bicarbonate, 0.5 g ammonium carbonate

monohydrate, and 0.4 g copper(II) sulfate pentahydrate into this solution. Finally, dilutethis solution to a final volume of 1000 mL using distilled water.

Solution B: In a 1000 mL Erlenmeyer flask, dilute 50 mL of 3% hydrogen peroxide to a

total volume of 1000 mL using distilled water.

Demonstration

Have one participant hold a funnel (or similar receptical) slightly above their head in their

right hand. The funnel should be attached to Tygon®

tubing that has been gently wrappedaround the individual’s body and drains into a large beaker. The demonstrator pours

solutions A and B simultaneously into the funnel so that the reaction illuminates as it wrapsits way around the participant. This demonstration is most effective when performed in a

darkened chamber.


All chemiluminescent reactions of luminol are all oxidations. The variations in light

produced when comparing different chemiluminescent demonstrations containing luminol



is due to the solvent system, protic or aprotic, used. This particular demonstration uses a protic solvent system since hydrogen peroxide is used as the base. The exact mechanism

through which chemiluminescence occurs has yet to be identified. What is known is thatthe luminol (I) is oxidized and that the emitting species is some form of aminophthalate ion

(II).

I II

Some variation of Chemiluminescence can be found today in the glowsticks purchased

from fairs or from Wal-MartTM in the outdoor department. A variation of chemiluminescence can also be observed in fireflies. In fireflies, the reaction is

luciferine (substrate) + luciferase (enzyme) + ATP (adenosine triphosphate)Æluciferyl adenylate – luciferase + pyrophosphate

luciferyl adenylate – luciferase + O2 Æ oxyluciferin + luciferase + AMP + light

Hazards

If your skin is exposed to copper(II) sulfate pentahydrate, wash the exposed areathoroughly before eating or drinking since copper compounds are harmful if taken

internally.

Disposal

All substances used in this demonstration are water soluble and can be flushed down the

drain.



Sugar MonsterDiana Mason, PhD

July 2003

Materials

1 – 250-mL beaker

1 – 100-mL graduated cylinder

Table sugar

Concentrated sulfuric acid

Sodium bicarbonate

Preparation

Fill 250-mL beaker one-third to one-half full of sugar.

Demonstration

Add 25 mL of concentrated sulfuric acid on top of the sugar in the beaker.


C12H22O11+ H2SO4 Æ 11H2O + 12C + H2SO4 + E

The word carbohydrate is a combination of the words carbon and hydrate (meaning water). The reaction that

occurs when sulfuric acid is added to a pile of sugar is the dehydration (removal of water) of the sugar. As

water is evolved in the form of steam, a black cone is produced that is composed of carbon. In addition to the

steam and carbon produced a noxious smell is generated that is a combination of a burnt sugar odor and sulfur

dioxide.

This reaction is an excellent reaction to use when teaching indicators of a chemical reaction. Five of the primary indicators can readily be observed: (1) There is a color change (white sugar to black carbon), (2)

Heat is generated (intense exothermic reaction), (3) Gas is generated (bubbles are produced as the reaction

proceeds), (4) Water is produced (in most reactions this fact is difficult to observe, but due to the steam

produced, it is easily observed in this reaction), and (5) An odor is produced (a combination of the burnt sugar

smell and sulfur dioxide fumes).

Hazards

Sulfuric acid is extremely corrosive and should be handled using gloves. If skin or clothing is exposed to

sulfuric acid, rinse exposed areas with copious amounts of water.

Disposal

Add sodium bicarbonate while breaking the black column apart to neutralize any sulfuric acid residue. Rinsecolumn thoroughly with water and then dispose in waste paper basket. Clean glassware thoroughly using

large amounts of water.



Elephant ToothpasteDiana Mason, PhD

July 2003

Materials

1 – 1000 to 2000-mL graduated cylinder

White liquid dish soap

Potassium iodide

30% hydrogen peroxide (Available at Beauty Supply Stores)

Food coloring

Gloves

Plastic tub

Preparation

Set the large graduated cylinder inside the plastic tub. Pour approximately 50 mL of 30% hydrogen peroxide

and two squirts of liquid dish soap into the large graduated cylinder. Gently add 2 to 3 colors of food coloringdown the side of the graduated cylinder so that a line of coloring extends from the top of the cylinder to the

solution below.

Demonstration

Add approximately 5 grams of potassium iodide to the cylinder.


I-+ H2O2 + dish soapÆ H2O + O2 + I

-+ foam + E

This demonstration is a good example of a catalyzed exothermic reaction. The foam produced is simply the

result of the oxygen bubbles getting trapped by the dish soap and forming foam due to the intense reactionthat occurs between the potassium iodide and hydrogen peroxide. The foam will have a slight yellow tinge

due to the iodine that is trapped within the bubbles. An additional product of this reaction is the generation of

a vast amount of heat. The heat causes the water produced to boil causing steam to be evolved. The degree of

the reactions exothermic property can be detected from the warmth of the glass cylinder.

Hazards

30% Hydrogen peroxide is a strong oxidizer and should be handled with gloves. Should skin be exposed to

this concentration of peroxide a light spot will occur in the contact area and a burning sensation will be felt.

Upon exposure the skin should be rinsed thoroughly with large amounts of water. The foam produced will

contain a reasonable amount of iodine that can stain surfaces, so care should be exercised to avoid contact

with items when cleaning up.

Disposal

The products of this reaction may be disposed of down a sink drain by rinsing the graduated cylinder and

plastic tub with an abundance of water to dilute the potassium hydroxide formed and residual 30% hydrogen

peroxide.



Jug of FireDiana Mason, PhD

July 2003

Materials

1 – 5-gallon carboy (A 5-gallon bottle that water is delivered in works well)

50 mL of denatured alcohol (purchased from a hardware store)Rubber stopper (to fit mouth of jug)

Lighter (preferably with a long neck)

Preparation

Pour approximately 50 mL of denatured alcohol into the 5-gallon carboy and stopper the

jug with a rubber stopper. Let stand for at least 15 minutes.

Demonstration

Out of sight of the audience pour out excess denatured alcohol to give the illusion that the

jug is empty. Stand the carboy on a surface and light the fumes within the carboy using thelighter (e.g., Piezo

®or Scripto

®).


CH3CH2OH + 3O2 + EA Æ 3H2O + 2CO2 + E

This reaction is an example of combustion reaction in oxygen. The products of all

combustion reaction are carbon dioxide and water.

This is also a good example of the hazards associated with an empty gas tank compared toa non-empty gas tank. The fumes present in an empty gas tank are more flammable and

explosive than gasoline.

Hazards

Prior to using a carboy, check for any cracks or other defects so as to prevent unexpected

severance into small pieces. Due to the flammability of alcohol and since the flames willdischarge from the top of the jug, the presenter should stand back from the jug and should

not be peering into the jug when the fumes are lit.

Disposal

None



Electric PickleDiana Mason, PhD

July 2003

Materials

1 - Large kosher dill pickle (available at convenience or grocery stores)

1 – Ring stand

1 - Buret Clamp

Electrode Set-up (as seen below) for “suicide” cord

Preparation

Attach the buret clamp to the ring stand. Place the pickle in the buret clamp so that the pickle does not move.

Insert the nails attached to the positive and negative leads into opposite ends of the pickle making sure that

the nails DO NOT touch each other.

Demonstration

Plug in the electrode setup into a 120V outlet.


After a second or two, the pickle will begin to glow on one end due to the electrolytes contained within the

pickle. Electrolytes found within pickles include vinegar (dilute acetic acid) and brine (salt water). An

electrolyte by definition is a chemical compound that ionizes when dissolved to produce an electrically

conductive medium composed of positive and negative ions. Our bodies require that we maintain a balance of

electrolytes in our system. Perspiration is a combination of water and salts (electrolytes) and therefore these

electrolytes must be replenished. Certain foods, such as pickles, and drinks, such as Gatorade®

, are excellent

sources for these electrolytes.

Hazards

If the nails are touching during the experiment, there is a possibility of sparking, fire and the pickle

exploding. Do not eat the pickle following the experiment because iron oxide residues from the nails will

have accumulated on the inside surface.

Disposal

Throw the pickle away in waste paper bin.

nail (wrap lead around nail and

insulate with electrician tape)nail (wrap lead around nail and

insulate with electrician tape)

wood block wood block

ositive leadne ative lead

plug



Fire and IceDiana Mason, PhD

July 2003

Materials

2 – 5 lb blocks of dry ice

Magnesium turnings or magnesium strip rolled into a loose ballLighter

GlovesTrowel, knife, spatula or flathead screwdriver

Preparation

Wearing gloves dig out an approximate 4-inch diameter by 2-inch deep trench into one of the blocks of dry ice using either a trowel, knife, spatula or flathead screwdriver. Place the

magnesium into the trench so that the top of the magnesium is level with the surface of the block of dry ice.

Have the second block of dry ice sitting beside the block containing the magnesium.

Demonstration

Using a lighter (e.g., Piezo®

or Scripto®

), light the magnesium until it sparks (the spark willlook like the light produced by a welders torch or that produced by white holiday

sparklers). Wearing gloves, quickly place the second piece of dry ice onto the top of the dryice block containing the magnesium and turn out the lights.


2Mg + O2 Æ 2MgO

In this demonstration, it can be observed that the burning magnesium, producing a whitelight, continues to burn even once covered by a second block of dry ice. Dry ice is strictly

frozen carbon dioxide. One common use of carbon dioxide is as the chemical present insome fire extinguishers. Not all fire extinguishers however contain carbon dioxide. What

this demonstration illustrates is that carbon dioxide, while capable of extinguishing manytypes of fire, is not applicable for use as an extinguisher for all types of fire.

A second experiment can be done to further illustrate this latter point The materials that

will be needed include a 400-mL beaker, a wood splint, a magnesium strip, a pair of tongs,a lighter and some dry ice. Step 1: Place several chunks of dry ice into the 400-mL beaker

until the beaker is approximately half-full. Step 2: While holding a wood splint with tongs,light the end of the splint until a fire can be observed and then dip the wood splint into the



beaker. Step 3: While holding a magnesium strip with tongs, light the magnesium strip and place it into the beaker. The students will observe that the carbon dioxide gas from the dry

ice extinguishes the wood flame, but not the flame resulting from the burning of themagnesium strip.

In the current demonstration, the trench previously containing magnesium now contains adark residue. This residue is the result of the burning magnesium absorbing the oxygenfrom the carbon dioxide to maintain the fire, leaving a carbon deposit.

Hazards

The temperature of dry ice is at a –78.5 °C whereas your ice freezes at 0 °C. Freezer burn

WILL result if skin is exposed to dry ice, therefore, gloves should be worn at all timesduring this experiment. The light produced by burning magnesium is an extremely strong

white light. It is recommended that you do not stare directly at the magnesium, instead useyour peripheral vision to determine whether the magnesium has caught fire because the UV

light emitted will damage your retina!

Disposal

The residue remaining within the trench can be disposed of in a waste paper bin. The dry

ice can be placed in a sink and allowed to evaporate or warm water can be allowed to flowover the dry ice accelerating the process of evaporation.



Mason DotDiana Mason, PhD

July 2003

Materials

1 – Mason Dot®

(1 – Gummy Bear ®

will also work)

Potassium chlorate

50 mL test tube

Ring stand

Three-finger buret clamp

Blowtorch

Preparation

Place the test tube, filled approximately 1/3 full with potassium chlorate, into the buret clamp, attached to the

ring stand, so that the test tube resides at a 45-degree angle from the table’s surface. Heat the potassium

chlorate with the blowtorch until the solid has decomposed entirely.

Demonstration

Turn out the lights and add the Mason Dot® or Gummy Bear ® and watch the reaction emit purple flames.


2KClO3 + EÆ 2KCl + 3O2 (endothermic reaction)

C12H22O11(Mason Dot®

or Gummy Bear ®

) + 12O2 Æ 12CO2 + 11H2O + E

Potassium chlorate melts at 368 °C and decomposes at 400 °C to form potassium chloride and oxygen. Upon

addition of the Mason Dot

®

or Gummy Bear

®

to the reaction, purple sparks are emitted which is actually thecolor produced by the potassium of the potassium salt. The Mason Dot® or Gummy Bear ® is combusted in the

presence of oxygen to form carbon dioxide and water. Observation of the time during which the purple sparks

gives direct information about the energy produced by one Mason Dot®.

1 food Calorie = 1000 scientific calories = 1 kcal

A Mason Dot® contains about 12 food calories or 12 scientific kcals. The energy produced in this reaction

lasts a minute or two. A Bacon cheeseburger and a regular order of fries from Burger King® contains 882

food Calories, 882,000 scientific calories or 882 kcals and therefore would produce 73.5 times the energy of

one Mason Dot®. Therefore the energy obtained from a lunch from Burger King® should last the consumer

between 1 hour and 14 minutes and 2 and 1/2 hours.

Hazards

Potassium chlorate is a strong oxidizer and slightly toxic. Except during the demonstration, it should be kept

away from sugar as well as ammonium salts, carbon, combustible materials, finely divided materials, sulfur,

phosphorus, sulfuric acid, metal powders, and organic materials. This reaction requires the application of and

produces a large amount of heat, so the test tube should be handled with care after demonstration.

Disposal

The solid produced can be disposed of in a waste paper bin and the test tube washed thoroughly with soap

and water.



Great Balls of FireDiana Mason, PhD

July 2003

Materials

2 – Large, rusted, iron ball bearings

Aluminum foil

Preparation

Wrap one of the ball bearings in aluminum foil.

Demonstration

Holding the ball bearing, wrapped in foil, relatively still in one hand, strike it using the

second ball bearing.


Fe2O3 + 2AlÆAl2O3 + 2Fe

The student will observe a spark being emitted and the sound of a bang. This reaction is a

single exchange reaction and is commonly referred to as a thermite reaction. There areother variations of this reaction, but this one contains the least number of hazards.

One use of the thermite reaction, on a much grander scale than this, is the repair of railroadtracks. Thermite is said to burn at 2200 °C. It is also used as a bomb to destroy file cabinets

and to accomplish under water welding actions.

Hazards

Sparks emitted from this demonstration have the potential to cause a fire.

Disposal

None

Mean-Green Demos by Dr. Diana Mason

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