hydrogen peroxide manganese dioxide experiment

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Decomposition of H₂O₂ with MnO₂

Avoid contact with hydrogen peroxide.

Chemicals and Solutions

• Hydrogen Peroxide, 30%
• Manganese Dioxide, solid

Pour some hydrogen peroxide into the cylinder and add a small spatula scoop of MnO₂. Bubbles of O₂ will form immediately (the reaction also produces heat).

Alternate Procedure: Genie in a bottle

Apparatus and materials.

• vase or foil covered bottle with stopper
• solid MnO ₂
• 30 mL of 30 % hydrogen peroxide
• Use a vase or cover a pop bottle with foil so students cannot see inside the bottle.
• Place 30 mL of 30% hydrogen peroxide (USE CARE!) in the bottle.
• Carefully remove the tea from a tea bag and in its place put in solid manganese dioxide.
• Now put the "tea bag" in the bottle such that it dangles above the hydrogen peroxide. Stabilize the "tea bag" in this position by inserting a stopper.
• When you are ready to present the demonstration simply remove the stopper and release the "genie".
• The "tea bag" of MnO₂ will fall into the hydrogen peroxide catalyzing the following reaction:

\( \ce{ H2O2 -> H2O + O2 } \)

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Genie in a Bottle Chemistry Demonstration

The genie in a bottle chemistry demonstration is an exciting reaction often performed as a science magic trick. The person doing the demonstration commands a genie to appear from a bottle, which produces a dramatic cloud of steam. The genie in a bottle demonstrates a decomposition reaction , catalysis, a chemical change , and an exothermic reaction . It’s particularly appropriate accompanying the elephant toothpaste reaction, which works on the same principle and uses some of the same chemicals.

The basis for the genie in the bottle reaction is the decomposition of hydrogen peroxide. But, you need a more concentrated solution that household peroxide. Get the 30% peroxide solution from a beauty supply store, online, or a chemical supply company.

• 30 to 50 milliliter 30% hydrogen peroxide (H 2 O 2 )
• 1/4 teaspoon (about 0.5 grams) manganese dioxide (MnO 2 )

Popular glassware choices include a colorful wine bottle or 1-liter volumetric, Florence, or Erlenmeyer flask. You can substitute sodium iodide (NaI) for the manganese dioxide, although the effect won’t be as dramatic. Both chemicals are available online from chemical suppliers.

Perform the Genie in a Bottle Chemistry Demonstration

In a nutshell, all you do is pour the peroxide into the bottle and add the manganese dioxide or sodium iodide. With a little preparation, you can easily improve the dramatic effect.

• Pour the manganese dioxide or sodium iodide onto a piece of tissue paper or toilet paper.
• Wrap the paper around the chemical and make a little packet. Tie it closed using a bit of string.
• Pour 30 to 50 milliliters of 30% hydrogen peroxide into the bottle.
• Dangle the packet into the bottle, but keep it from contact with the peroxide by holding the string with a stopper. Make sure the stopper is loose, just in case the packet drops. You don’t want pressure to build up and break the glassware.
• When you’re ready, uncap the bottle. If you like, command the genie to appear. Maybe it will grant you three wishes! Probably not, but at least you’ll get a nice cloud of vapor.

How the Genie in a Bottle Works

Hydrogen peroxide has a shelf life because it slowly decomposes into water and oxygen:

H 2 O 2  (aq) → 2H 2 O (l) + O 2  (g) + heat

While this is an exothermic reaction, a stored bottle of peroxide does not feel hot because the rate of the reaction is very slow. A catalyst greatly speeds up the reaction. In this reaction, the catalyst is either manganese dioxide or else sodium iodide. Similarly, the elephant toothpaste reaction uses either potassium iodide, sodium iodide, or else catalase from yeast.

Uncapping the bottle releases the string and drops the packet of catalyst into the hydrogen peroxide. The catalyzed reaction releases so much heat that it boils the water that is present in the hydrogen peroxide solution and released by its decomposition. The narrow bottle opening directs the steam so it exits the bottle as a visible cloud.

Manganese dioxide is a heterogeneous catalyst. What this means is that the phase of the catalyst is different from the phase of the reaction. The solid manganese dioxide surface makes the decomposition reaction favorable, although the exact mechanism of action is not well understood. The size of the catalyst particles influence the rate of the reaction. So, you’ll get a different effect using a fine powder compared with granules. One advantage of the genie in a bottle reaction over the elephant toothpaste reaction is that you can recover the catalyst following the reaction and prove to students that it isn’t used up.

Safety and Clean-Up

• Wear proper lab safety gear, including goggles and gloves.
• Ideally, use a borosilicate flask or bottle. But, most glass bottles work fine. If you use a plastic bottle, expect warping and shrinking from the heat of the reaction.
• Do not point the bottle toward a person or pet. Similarly, because the bottle may become hot, don’t hold it while performing the reaction.
• Read the product labels for chemical safety information. In particular, note that hydrogen peroxide is a strong oxidizing agent and manganese(IV) dioxide is toxic. Unlike the 3% hydrogen peroxide commonly found in homes, it is not safe to touch. Do not sniff or drink the contents of the bottle.
• Dilute the bottle contents with water. You can filter out the manganese dioxide, dry it, and re-use it. Wash the liquid down the drain. Dilute any spills with plenty of water before clean-up.
• Dirren, Glen; Gilbert, George; Juergens, Frederick; Page, Philip; Ramette, Richard; Schreiner, Rodney; Scott, Earle; Testen, May; Williams, Lloyd (1983). “Chemical Demonstrations.” A Handbook for Teachers of Chemistry . 1: 180–185. doi: 10.1021/ed062pA31.2
• IUPAC (1997). “Chemical decomposition.” Compendium of Chemical Terminology (2nd ed.) (the “Gold Book”). Oxford: Blackwell Scientific Publications. ISBN 0-9678550-9-8. doi:10.1351/goldbook
• Kauffman, George B.; Shakhashiri, Bassam Z. (2013). “Chemical Demonstrations: a Handbook for Teachers of Chemistry, Volume 5.” Foundations of Chemistry . 15(1): 119-120. doi: 10.1007/s10698-011-9137-6

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Reaction intermediates of MnO2 catalyzed H2O2 decomposition reaction

Manganese dioxide catalyzes the decomposition of hydrogen peroxide to water and oxygen gas.

But what are the intermediates in this catalyzed reaction?

• inorganic-chemistry
• decomposition

2 Answers 2

Reaction conditions.

As Watts et al. have shown, the decomposition products of this Fenton-like reaction strongly depend on the $\mathrm{pH}$ of the solution. 1

If performed in acidic conditions, the reaction generates mostly hydroxy radicals, but no reductants (which would be the hydroperoxide and superoxide anions). If, conversely, the reaction is held in neutral conditions, Watts et al. have shown that the reaction produces significantly more of the aforementioned reductants.

Do et al. have conducted further research into the reaction mechanism at $\mathrm{pH}=7$ and concluded that the observed reaction order may be approximated as a pseudo 1 st order reaction, where the ratio $\ce{[H2O2]}/\ce{[#MnO2]}$ is vital to the description of the decomposition rate. 2 They have further shown that reactive intermediates, such as superoxide and hydroperoxide anions are generated by the reaction. After slightly modifying the pH towards alkaline conditions, the production rates for the reactive anions increased drastically.

Reaction mechanism

Do et al. have meticulously assembled a table with a proposed reaction pathway:

And finally, I quote one of their closing statements: 2

The existence of hydroperoxide/superoxide anion implies that the suggested reaction mechanism could be explained by hydrogen peroxide being decomposed, not only directly on the surface of manganese oxide, but also through a propagation reaction involving intermediates such as hydroperoxide/superoxide anion in solution.

• Watts, R., Sarasa, J., Loge, F., and Teel, A. Oxidative and Reductive Pathways in Manganese-Catalyzed Fenton’s Reactions. J. Environ. Eng. , 131(1), 2005, 158–164, DOI link .
• Si-Hyun Do, Bill Batchelor, Hong-Kyun Lee, Sung-Ho Kong. Hydrogen peroxide decomposition on manganese oxide (pyrolusite): Kinetics, intermediates, and mechanism . Chemosphere , Volume 75, Issue 1, March 2009, Pages 8-12, DOI link .

I am adding a more recent study to complement the answer given by tschoppi. This journal addresses the kinetics and mechanism for the decompostion of $\ce{H2O2}$ on transition metal oxide surfaces. However, the paper only considers $\ce{ZrO2}$, $\ce{TiO2}$, $\ce{Y2O3}$. Although $\ce{MnO2}$ is also a transition metal oxide, $\ce{MnO2}$ may be different enough to lead to different paths or kinetics. The authors even state:

effects such as solution pH, type of oxide , temperature, and oxide particle size have profound effects on the kinetics and energetics of this type of reactions

Thus, take the results of the study with a grain of salt. I will focus more on the mechanism part of the journal. According to the journal

The kinetic experiments on the decomposition of $\ce{H2O2}$ together with the experiments on $\ce{HO•}$ detection show the existence of an adsorption step prior to decomposition. This type of process is also predicted with the DFT calculations. The decomposition of $\ce{H2O2}$ follows a similar mechanism for the three metal oxides studied. The obtained transition states are largely mediated by hydrogen bonding between $\ce {H2O2}$ and surface $\ce{HO}$ groups. Nevertheless, direct interaction between the oxygen atoms of $\ce{H2O2}$ and the metal atoms present in the oxide was also observed in the geometries of the transition states. The formation of two $\ce{HO}$ radicals as the primary product of the decomposition of $\ce{H2O2}$ is confirmed with both the DFT calculations and the experiments. One of these radicals can further abstract a $\ce{H}$ atom initially bound to a surface $\ce{O}$ and form $\ce{H2O}$. The other $\ce{HO}$ radical can adsorb to the surface by forming bonding states with the metal cation.

• Claudio M. Lousada, Adam Johannes Johansson, Tore Brinck, and Mats Jonsson. Mechanism of $\ce {H2O2}$ Decomposition on Transition Metal Oxide Surfaces J. Phys. Chem. C , 2010, 116 (17), DOI link .

• $\begingroup$ you said that the statement, effects such as solution pH, type of oxide, temperature, and oxide particle size have profound effects on the kinetics and energetics of this type of reactions. Makes the paper not that credible. If you could please state any reason why you said so ,that would be really helpful for me to further understand the problem statement. $\endgroup$ –  Omkar Kedge Commented Feb 26, 2019 at 9:04

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Question Video: Identifying the Correct Statement For the Decomposition of Hydrogen Peroxide Using a Manganese Dioxide Catalyst Chemistry • Third Year of Secondary School

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Manganese dioxide is used as a catalyst in the decomposition of hydrogen peroxide to form water and oxygen. Which statement is untrue when using MnO₂ as a catalyst? [A] The oxygen will be formed more quickly. [B] More oxygen will be produced. [C] The mass of MnO₂ before and after the reaction will be the same. [D] An alternative reaction pathway is provided by the catalyst. [E] The catalyst remains unchanged at the end of the experiment.

Video Transcript

Manganese dioxide is used as a catalyst in the decomposition of hydrogen peroxide to form water and oxygen. Which statement is untrue when using MnO2 as a catalyst? 2H2O2 aqueous produces 2H2O liquid plus O2 gas. (A) The oxygen will be formed more quickly. (B) More oxygen will be produced. (C) The mass of MnO2 before and after the reaction will be the same. (D) An alternative reaction pathway is provided by the catalyst. (E) The catalyst remains unchanged at the end of the experiment.

In this question, we’re being asked about how a catalyst, which is manganese dioxide, behaves in a decomposition reaction. In this decomposition reaction, a single reactant, the hydrogen peroxide, decomposes to form new products. The products are water and oxygen gas. This decomposition reaction is very slow under normal conditions at room temperature. We would not observe many bubbles of oxygen gas coming from the hydrogen peroxide solution at all. This situation would change rapidly if a small amount of the solid catalyst, manganese dioxide, were added to the hydrogen peroxide solution.

Rapid fizzing or effervescence would be observed as soon as the black powder is added to the hydrogen peroxide. The manganese dioxide catalyst will increase the rate of decomposition of the hydrogen peroxide. More oxygen gas, seen as bubbles, will be produced per unit of time as the reaction rate has been increased. Oxygen gas will certainly be produced more rapidly. This statement is true, so it’s not the correct answer. Remember, in this question, we’re looking for an untrue statement.

Notice that the oxygen gas, which is one of the products, originates from the hydrogen peroxide molecules. According to the balanced equation, two molecules of hydrogen peroxide are required to produce one molecule of oxygen gas. If we have a fixed amount of hydrogen peroxide molecules at the start of the reaction, we can only produce a fixed amount of oxygen molecules during the decomposition reaction. Adding the manganese dioxide catalyst does not change the amount of oxygen gas produced. It simply increases the rate of reaction.

The same amount of oxygen gas is produced in much less time. The manganese dioxide does not appear in the overall reaction equation. The amount of oxygen gas obtained will be the same with or without the catalyst present. This means that the statement that more oxygen gas is produced is untrue. Therefore, it’s likely to be the correct answer.

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• Experiments

Burning in pure oxygen

Pure oxygen kindles a smoldering splint!

• Hydrogen peroxide
• Manganese(IV) oxide
• Put on protective gloves and eyewear.
• Conduct the experiment on the plastic tray.
• Keep a bowl of water nearby during the experiment.
• Remove protective gloves before lighting the splint.
• Do not allow chemicals to come into contact with the eyes or mouth.
• Keep young children, animals and those not wearing eye protection away from the experimental area.
• Store this experimental set out of reach of children under 12 years of age.
• Clean all equipment after use.
• Make sure that all containers are fully closed and properly stored after use.
• Ensure that all empty containers are disposed of properly.
• Do not use any equipment which has not been supplied with the set or recommended in the instructions for use.
• Do not replace foodstuffs in original container. Dispose of immediately.
• In case of eye contact: Wash out eye with plenty of water, holding eye open if necessary. Seek immediate medical advice.
• If swallowed: Wash out mouth with water, drink some fresh water. Do not induce vomiting. Seek immediate medical advice.
• In case of inhalation: Remove person to fresh air.
• In case of skin contact and burns: Wash affected area with plenty of water for at least 10 minutes.
• In case of doubt, seek medical advice without delay. Take the chemical and its container with you.
• In case of injury always seek medical advice.
• The incorrect use of chemicals can cause injury and damage to health. Only carry out those experiments which are listed in the instructions.
• This experimental set is for use only by children over 12 years.
• Because children’s abilities vary so much, even within age groups, supervising adults should exercise discretion as to which experiments are suitable and safe for them. The instructions should enable supervisors to assess any experiment to establish its suitability for a particular child.
• The supervising adult should discuss the warnings and safety information with the child or children before commencing the experiments. Particular attention should be paid to the safe handling of acids, alkalis and flammable liquids.
• The area surrounding the experiment should be kept clear of any obstructions and away from the storage of food. It should be well lit and ventilated and close to a water supply. A solid table with a heat resistant top should be provided
• Substances in non-reclosable packaging should be used up (completely) during the course of one experiment, i.e. after opening the package.

FAQ and troubleshooting

You can purchase hydrogen peroxide at your local drugstore. Look for concentrations ranging from 3–5%.

Make sure that the splint is still smoldering when you lower it into the flask, and don’t let it touch the solution.

Step-by-step instructions

Add some manganese dioxide MnO 2 to a hydrogen peroxide H 2 O 2 solution to produce oxygen O 2 .

Make a splint smolder.

See what happens when a smoldering splint meets pure oxygen.

Dispose of solid waste along with household garbage. Pour solutions down the sink. Wash with an excess of water.

Scientific description

Why does the smoldering splint ignite.

Smoldering is a slow, flameless form of combustion – the organic substances on the surface of the splint are reacting with the oxygen in the air. Our splint smolders relatively slowly, and over time may cease to burn altogether.

However, there are several ways to increase the reaction rate of the smoldering splint. For example, we can increase the concentrations of the initial reagents. This is exactly why we put the splint into the flask filled with almost pure oxygen – we are surrounding the splint with a much higher concentration of oxygen molecules than can be found in air. This, along with the increase in temperature, dramatically speeds up the reaction rate, so the splint ignites with a bright flame.

Where does the oxygen in the flask come from?

The oxygen is produced via the decomposition of hydrogen peroxide as shown in the following reaction:

2H 2 O 2 → O 2 + 2H 2 O

Why, then, can regular pharmaceutical-grade hydrogen peroxide be stored for long periods of time (up to three years if the bottle remains unopened) without any sign of decomposition? The secret is in the reaction rate. On its own, hydrogen peroxide decomposes very slowly. We can, however, make this reaction proceed faster by using special accelerators known as catalysts . Catalysts significantly speed up reaction rates – sometimes even by a factor of several million!

The antibacterial effect of hydrogen peroxide is rooted in its decomposition. A fresh wound expels drops of blood. Blood, in turn, contains compounds that can accelerate the decomposition of hydrogen peroxide. Thus, upon contact with a wound, hydrogen peroxide decomposes and releases bubbles of oxygen. It’s important to note that this isn’t “regular” oxygen; these are not O 2 molecules, but rather very active O∙ particles that eliminate any microbes in their presence. Upon colliding with each other, these same particles bond together to produce molecular oxygen O 2 :

Why did we add manganese dioxide MnO 2 ?

Manganese dioxide MnO 2 serves as a catalyst in the decomposition of hydrogen peroxide. It significantly speeds up the reaction rate. When manganese dioxide is added to regular 3% hydrogen peroxide, the hydrogen peroxide starts to hiss and decompose, releasing a considerable amount of oxygen. Within a short time, oxygen completely fills the flask. This allows us to ignite our splint!

Dozens of experiments you can do at home

One of the most exciting and ambitious home-chemistry educational projects The Royal Society of Chemistry

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Generating, collecting and testing gases

In association with Nuffield Foundation

Gases give rise to particular hazards so great care must be taken when preparing, collecting or testing

Gases give rise to particular hazards so great care must be taken when preparing, collecting or testing them.

How the gas is to be used will differ from experiment to experiment – it is essential to read carefully the specific instructions given or referred to in the experimental procedure and any accompanying technical notes. This is especially important if the gas needs to be dried.

Gases can be collected by upward or downward delivery or over water. Refer to specific information on each gas below.

Health, safety and technical notes 

• Read our standard health and safety guidance.  
• Wear eye and skin protect if required.
• Hydrochloric acid is highly corrosive, refer to CLEAPSS Hazcards  HC047a , plus CLEAPSS Recipe Book RB021.  
• Zinc is of low hazard, refer to CLEAPSS Hazcard  HC108b
• Copper is of low hazard, refer to CLEAPSS Hazcard  HC026 .
• Hydrogen gas is EXTREMELY FLAMMABLE – ensure there are no naked flames. Refer to CLEAPSS Hazcard  HC048
• Hydrogen peroxide (IRRITANT) to manganese(IV) oxide powder (HARMFUL). Collect the gas over water. Refer to CLEAPSS Hazcard  HC050
• Oxygen is an OXIDISING AGENT, refer to CLEAPSS Hazcard  HC069
• Potassium manganate(VII) (OXIDISING, HARMFUL and DANGEROUS FOR THE ENVIRONMENT). Refer to CLEAPSS Hazcard  HC081

Double-check that the acid is hydrochloric and NOT sulfuric.

• Sodium chlorate(I) can cause headache, fatigue, dizziness, and methemoglobinemia. Refer to CLEAPSS Hazcards  HC089 .
• Chlorine is classified as toxic, irritant and dangerous for the environment. Refer to CLEAPSS Hazcard  HC022a

General gas preparation

The diagram below shows a typical set of apparatus which can be used to prepare a range of gases.

Source: Royal Society of Chemistry

Typical apparatus used for preparing a range of gases

Gas collection methods

The diagrams below show three different methods for collecting gas.

Three methods of gas collection

Preparing specific gases

Wear appropriate eye protection. The amounts given below are sufficient to generate 1 litre (1 dm 3 ) of each of the named gases.

Carbon dioxide, CO 2

Slowly add 42 cm 3  of 2 M hydrochloric acid (IRRITANT) to an excess of marble chips. Collect the gas by downward delivery or over water (slightly soluble).

Hydrogen, H 2

Slowly add 28 cm 3  of 3 M hydrochloric acid (CORROSIVE) to excess zinc granules and 1 g of hydrated copper sulfate (HARMFUL). Collect the gas by upward delivery or over water.

Hydrogen gas is EXTREMELY FLAMMABLE – ensure there are no naked flames.

Oxygen, O 2

Slowly add 50 cm 3  of 20 vol hydrogen peroxide (IRRITANT) to manganese(IV) oxide powder (HARMFUL). Collect the gas over water.

Oxygen is an OXIDISING AGENT.

Chlorine, Cl 2

Work in a fume cupboard. Method 2 is safer and recommended but slower.

Add 14 cm 3  of concentrated hydrochloric acid (CORROSIVE) to at least 3 g of potassium manganate(VII) (OXIDISING, HARMFUL and DANGEROUS FOR THE ENVIRONMENT).

Add 5 M hydrochloric acid (IRRITANT) to 30 cm 3  of recently purchased (10–14% available chlorine) sodium chlorate(I) solution (CORROSIVE) with plenty of stirring. Note that sodium chlorate(I) is only available as a solution often called ‘sodium hypochlorite’; it must not be confused with sodium chlorate(V) (sometimes just called ‘sodium chlorate’), which is a white, crystalline solid. School samples often react too slowly because old sodium chlorate(I) is used. This will have less than the required 10% available chlorine (as it applies to both methods). 

The equipment required for preparing chlorine gas

Collect the gas by downward delivery. Chlorine is classified as TOXIC, IRRITANT and DANGEROUS FOR THE ENVIRONMENT.

Additional information

This is a resource from the  Practical Chemistry project , developed by the Nuffield Foundation and the Royal Society of Chemistry. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompany  Practical Physics  and  Practical Biology .

The resource is also part of the Royal Society of Chemistry’s Continuing Professional Development course:  Chemistry for non-specialists .

© Nuffield Foundation and the Royal Society of Chemistry

• Teacher notes
• Technician notes
• Practical skills and safety

Specification

• 2.9.5 describe the laboratory preparation and collection of hydrogen using zinc (or other suitable metal) and hydrochloric acid, and recall the physical properties of hydrogen and its uses, including weather balloons and hardening oils, and its potential…
• 2.9.6 describe the laboratory preparation and collection of oxygen by the catalytic decomposition of hydrogen peroxide, and recall the physical properties of oxygen and its uses in medicine and welding;
• 2.9.8 describe the laboratory preparation and collection of carbon dioxide gas using calcium carbonate and hydrochloric acid, and recall the uses of carbon dioxide in fizzy drinks and fire extinguishers.
• 7. Investigate the effect of a number of variables on the rate of chemical reactions including the production of common gases and biochemical reactions.
• Mandatory experiment 6.1 - Monitoring the rate of production of oxygen from hydrogen peroxide, using manganese dioxide as a catalyst.
• Demonstration of the effects on reaction rate of (i) particle size
• 4.8.2.1 Test for hydrogen
• 4.8.2.2 Test for oxygen
• 4.8.2.3 Test for carbon dioxide
• 4.8.2.4 Test for chlorine
• Describe tests to identify selected gases including hydrogen and carbon dioxide.
• Describe tests to identify selected gases including oxygen, hydrogen and chlorine.
• 5.8.2.1 Test for hydrogen
• 5.8.2.2 Test for oxygen
• 5.8.2.3 Test for carbon dioxide
• 5.8.2.4 Test for chlorine
• 3.12 Describe the chemical test for: hydrogen, carbon dioxide (using limewater)
• C1.1.12 describe tests to identify oxygen, hydrogen and carbon dioxide
• C1.4.2 describe a test to identify chlorine (using blue litmus paper)
• C4.2a describe tests to identify selected gases
• C1.3g describe tests to identify selected gases
• Simple tests can be used to identify oxygen, hydrogen and carbon dioxide gases.
• methods for the collection of gases including:
• (o) the reactions of the alkali metals with air/oxygen, the halogens and water
• (p) the test used to identify hydrogen gas
• (j) the tests used to identify oxygen gas and carbon dioxide gas
• (n) the reactions of the alkali metals with air/oxygen, the halogens and water
• (o) the test used to identify hydrogen gas
• (m) reactions of the halogens with metals

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Practical potions microscale | 11–14 years

By Kirsty Patterson

Observe chemical changes in this microscale experiment with a spooky twist.

Antibacterial properties of the halogens | 14–18 years

By Kristy Turner

Use this practical to investigate how solutions of the halogens inhibit the growth of bacteria and which is most effective

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