Some New Ideas:
1. Replace the light bulbs in your home with long life CFL (compact fluorescent) bulbs. These last up to 15 times longer than regular bulbs and use up 80% less electricity than regular bulbs. You could simply replace your regular bulbs as and when they burn out
2। Use rechargeable batteries to reduce your carbon footprint by up to 1,000 pounds over the life of the batteries
3. Buy locally produced goods and services. Goods and services that are produced locally eliminate thousands of pounds of carbon by reducing fossil fuel transportation demands.
4. Clean the lint filter in your dryer. This will reduce your energy used, saving the environment and your electric bill
5. Whenver possible hang your washing out on the clothesline rather than using the dryer.
Wednesday, May 18, 2011
Wednesday, May 4, 2011
how to reduce your carbon footprint
Choose to have 2 children or adopt. Nothing else makes makes this much difference.
Use vegetable-based and biodegradeable cleaning products
Use recycled wood chips to keep the weeds down, retain moisture, and prevent erosion.
Don't water your grass.
Borrow seldomly used items such as ladders and chain saws.
Put leaves in a compost heap instead of burning them or throwing them away.
Install water barrels to collect rain water from troughs. Place a small bucket in your sink to collect water when washing produce. Use this water in the garden.
Recycle your plastic bags (or use the reuseable bags) , aluminum, and water bottles.
Make a craft with household items, make a toilet paper roll into a penguin, make an old glass plate into a new one by repainting it.
Switch your water mode- if you are going to be away from your house for a while, switch your water heater to "vacation or away" mode. It keeps your water warm but, will not use the energy it takes to keep a full-tank of boiling water.
Make time for errands- instead of leaving to go straight home, run some errands while your already in the area. It saves gas and it causes less pollution to the environment.
Use vegetable-based and biodegradeable cleaning products
Use recycled wood chips to keep the weeds down, retain moisture, and prevent erosion.
Don't water your grass.
Borrow seldomly used items such as ladders and chain saws.
Put leaves in a compost heap instead of burning them or throwing them away.
Install water barrels to collect rain water from troughs. Place a small bucket in your sink to collect water when washing produce. Use this water in the garden.
Recycle your plastic bags (or use the reuseable bags) , aluminum, and water bottles.
Make a craft with household items, make a toilet paper roll into a penguin, make an old glass plate into a new one by repainting it.
Switch your water mode- if you are going to be away from your house for a while, switch your water heater to "vacation or away" mode. It keeps your water warm but, will not use the energy it takes to keep a full-tank of boiling water.
Make time for errands- instead of leaving to go straight home, run some errands while your already in the area. It saves gas and it causes less pollution to the environment.
Friday, November 19, 2010
Different Kinds of Chemical Reactions
There are many chemical reactions that take place between chemicals and their reactants, most of them occuring inside our body without us realizing it. These reactions include synthesis, decomposition, single-replacement, double replacement, and combustion.
Synthesis is a chemical reaction in which it is purposely made to react with another chemical or chemicals. it is also physically or chemically manipulated. This usually means that the reaction is reproducible and reliable.
Another type of reaction is known as chemical decomposition. This involves the seperation of chemical compounds, and, in turn, breaking the compound down to simpler elements or compounds. These type of reactions are usually undesired.
Single-replacement reactions are yet another type of reaction. This type of reaction is also known as an oxidation-reduction chemical reaction. This is when an element or ion moves from one compund to another. the elements usually replace each other in their respective compounds.
Another similar reaction to the single- replacement reaction is called the double-replacement reaction. It is also called the metathesis reaction. Instead of exchanging single elements, like the single-replacement reaction, this involves the exchange of bonds resulting in chemical species with similar bonding affiliations.
The last form of reaction is called combustion. This, no doubt, involves heat. It is a series of exothermic reactions with fuel and its oxidant accompanied by heat. This heat usually causes glowing or flames. Many fuels often include hydrocarbons.
These reactions provide the basis of what created life and helped to create the world we know today.
Synthesis is a chemical reaction in which it is purposely made to react with another chemical or chemicals. it is also physically or chemically manipulated. This usually means that the reaction is reproducible and reliable.
Another type of reaction is known as chemical decomposition. This involves the seperation of chemical compounds, and, in turn, breaking the compound down to simpler elements or compounds. These type of reactions are usually undesired.
Single-replacement reactions are yet another type of reaction. This type of reaction is also known as an oxidation-reduction chemical reaction. This is when an element or ion moves from one compund to another. the elements usually replace each other in their respective compounds.
Another similar reaction to the single- replacement reaction is called the double-replacement reaction. It is also called the metathesis reaction. Instead of exchanging single elements, like the single-replacement reaction, this involves the exchange of bonds resulting in chemical species with similar bonding affiliations.
The last form of reaction is called combustion. This, no doubt, involves heat. It is a series of exothermic reactions with fuel and its oxidant accompanied by heat. This heat usually causes glowing or flames. Many fuels often include hydrocarbons.
These reactions provide the basis of what created life and helped to create the world we know today.
COMBUSTION
A combustion reaction takes place when a fuel and an oxidant react, producing heat or heat and light. The most recognizable form of combustion reaction is flame, with explosions being an even faster form of combustion reaction. A combustion can happen at a wide range of speeds, and can occur in many different environments, but the majority of combustions we know and recognize happen in a fairly limited spectrum.
DECOMPOSITION
A decomposition reaction is a type of chemical reaction in which a substance degrades into two or more basic components. It is a process in direct contrast to that of chemical synthesis, which involves molecular bonding so that two or more components may join to form a single chemical compound. The decomposition reaction often requires exposure to a catalyst, such as a heat source or solvent.
SYNTHESIS
A synthesis reaction or direct combination reaction is one of the most common types of chemical reactions. In a synthesis reaction two or more chemical species combine to form a more complex product.
A + B → AB
SINGLE-REPLACEMENT
A single replacement reaction, sometimes called a single displacement reaction, is a chemical reaction where one element replaces another element in a compound to increase stability. An example of a single replacement reaction that takes place in real life is when oxidation forms rust on cars.
DOUBLE-REPLACEMENT
double replacement reaction - a chemical reaction between two compounds where the positive ion of one compound is exchanged with the positive ion of another compound.
A combustion reaction takes place when a fuel and an oxidant react, producing heat or heat and light. The most recognizable form of combustion reaction is flame, with explosions being an even faster form of combustion reaction. A combustion can happen at a wide range of speeds, and can occur in many different environments, but the majority of combustions we know and recognize happen in a fairly limited spectrum.
DECOMPOSITION
A decomposition reaction is a type of chemical reaction in which a substance degrades into two or more basic components. It is a process in direct contrast to that of chemical synthesis, which involves molecular bonding so that two or more components may join to form a single chemical compound. The decomposition reaction often requires exposure to a catalyst, such as a heat source or solvent.
SYNTHESIS
A synthesis reaction or direct combination reaction is one of the most common types of chemical reactions. In a synthesis reaction two or more chemical species combine to form a more complex product.
A + B → AB
SINGLE-REPLACEMENT
A single replacement reaction, sometimes called a single displacement reaction, is a chemical reaction where one element replaces another element in a compound to increase stability. An example of a single replacement reaction that takes place in real life is when oxidation forms rust on cars.
DOUBLE-REPLACEMENT
double replacement reaction - a chemical reaction between two compounds where the positive ion of one compound is exchanged with the positive ion of another compound.
Friday, November 5, 2010
The making of the "Halloween Reaction"
Austin performing on stage: 
When Austin performed this demonstration on stage, i was surprised too. Even though we were already told of what was going to happen i was amazed by how the colors changed so quick. I felt the the audience like it because all the excitement i heard from them. Austin looked great up there because he was constantly smiling and he looked like he totally knew what he was doing, like it has already been practiced on a few times. when the colors changed you could see his face light up, before when he was pouring in the chemicals, he look like he wasn't sure of what was going to happen; he was probably thinking the same as me when i saw it, i didn't know that the demonstration was actually going to work because we haven't experimented it before the show, but when the color changed i was relieved, happy that it did what it was supposed to do. I think that this was a great experience to be able to show how fun science is to other peers. I don't know how the others felt about the show, but I felt really good about it.
The Video to show the making of the "Halloween Reaction"
When Austin performed this demonstration on stage, i was surprised too. Even though we were already told of what was going to happen i was amazed by how the colors changed so quick. I felt the the audience like it because all the excitement i heard from them. Austin looked great up there because he was constantly smiling and he looked like he totally knew what he was doing, like it has already been practiced on a few times. when the colors changed you could see his face light up, before when he was pouring in the chemicals, he look like he wasn't sure of what was going to happen; he was probably thinking the same as me when i saw it, i didn't know that the demonstration was actually going to work because we haven't experimented it before the show, but when the color changed i was relieved, happy that it did what it was supposed to do. I think that this was a great experience to be able to show how fun science is to other peers. I don't know how the others felt about the show, but I felt really good about it.
The Video to show the making of the "Halloween Reaction"
Monday, October 18, 2010
Oct.18, 2010
In the following text, our group found the demonstration for the Halloween reaction or the "Old Nassau Reaction."
Old Nassau
This experiment continues the theme of `clock' reactions. The demonstration is known as the `Old Nassau Reaction', a clock reaction which turns orange and then black (and has therefore also been named the `Halloween Reaction') [1]. As Alyea describes [1] `the formation of orange HgI2 was discovered accidentally by two Princeton undergraduates ... when they were carrying out original research on the inhibition, by Hg2+, of the Landolt reaction'. From this, by reducing the Hg2+ concentration, the present demonstration was subsequently developed [2].
The name `Old Nassau', comes from Nassau Hall which was named after William III, King of England, Prince of Orange and Nassau. Nassau Hall can boast of a colourful history [1]. `At the time it was built it was the largest college building in North America. On January 3, 1777 General Washington crossed the Delaware to sieze the British ammunition stored there: his victorious Battle of Princeton followed. In 1796 it was perhaps the earliest undergraduate chemistry laboratory in the world,* where Dr John Maclean, Professor of Chemistry, had the students, themselves, carrying out chemical experiments. At that time Europe still practised apprenticeship: colleges in the New World gave only lecture demonstrations. In the late 1830s, several years before Samuel Morse sent his first telegraph message, Dean Joseph Henry, using an electromagnet, sent `clicks' from his office in Nassau Hall to his home nearby to alert his servants that he was coming home shortly, and to start heating water for his tea'.
The reaction in this experiment takes place in several steps [5]. First, sodium metabisulphite reacts with water to form sodium hydrogen sulphite:
Preparation. The following three solutions need to be prepared.
A. Make a paste of 4 g of soluble starch with a few mils of water. Pour onto this 500 ml of boiling water and stir. Cool to room temperature, add 13.7 g of sodium metabisulphite (Na2S2O5) and make up to 1 l with water.
B. Dissolve 3 g of mercury(II) chloride in water and make the solution up to 1 l with water.
C. Dissolve 15 g of potassium iodate (KIO3) in water and make the solution up to 1 l with water.
Demonstration. Mix 50 ml of solution A with 50 ml of solution B. Then pour into this mixture 50 ml of solution C. After about 5 seconds the mixture will turn an opaque orange colour as insoluble mercury iodide precipitates. After further 5 seconds the mixture suddenly turns blue-black as a starch-iodine complex is formed. The second colour change (orange to black) is not normally expected by the audience and comes as a real surprise.
This experiment can be extended in several ways [5]. Diluting all the solutions by a factor of two increases the time taken for the colour changes to occur. Using a smaller volume of solution B speeds up the reaction. The effect of changing the amounts and concentrations of the various reactants cannot always be predicted simply because of the complexity of the system. For example, if the volume of solution B is doubled, the appearance of the orange colour is delayed and the blue colour fails to appear at all.
If using mercury salts is not desirable, a somewhat simpler clock reaction can be performed. This is known as iodine clock reaction or Landolt reaction. The experiment is performed by mixing equal volumes of two solutions, one containing 2 g dm-3 KIO3 and H2SO4 0.03 M; the second - 0.4 g dm-3 of NaHSO3 in starch (2 g dm-3) previously dissolved in boiling water. The initially colourless mixture suddenly turns dark blue. There are several extensions to this reaction as well, which can be found, for example in Ref. [7].
Safety. All soluble mercury salts are poisonous and should be treated accordingly.
References.
1. Tested Demonstrations in Chemistry, ed. G.L. Gilbert, et al., Denison University, Granville, OH, 1994, vol. 1, p. I-49.
2. H.N. Alyea, J. Chem. Educ., 1955, 32, 9.
3. B.N. Menschutkin, `A Russian physical chemist of the eighteenth century', J. Chem. Educ., 1927, 4, 1079.
4. H.S. Van Klooster, `The beginnings of laboratory instruction in chemistry in the USA', in Chymia: Annual Studies in the History of Chemistry, ed. T.L. Davis, vol. 2, Philadelphia, University of Pennsylvania Press, 1949, pp. 1-15.
5. T. Lister, Classic Chemistry Demonstrations, ed. C. O'Driscoll and N. Reed, London, Royal Society of Chemistry, 1995, p. 50.
6. B.Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Volume 4, Wisconsin, US, The University of Wisconsin Press, 1992.
7. Ref. 1, p. I-46
Next, our group found the demonstration to the Volcano reaction or the Ammonium Dichromate Reaction.
The eruption of an ammonium dichromate [(NH4)2Cr2O7] volcano is a classic chemistry demonstration. The ammonium dichromate glows and emits sparks as it decomposes and produces copious amounts of green chromium (III) oxide ash. This demonstration is simple to prepare and perform. The decomposition of ammonium dichromate commences at 180°C, becoming self-sustaining at ~225°C. The oxidant (Cr6+) and the reductant (N3-) are present in the same molecule.
(NH4)2Cr2O7 --> Cr2O3 + 4 H2O + N2
The procedure works well in both a lighted or darkened room.
Materials
If you are using a hood:
Chromium III and chromium VI, as well at its compounds, including ammonium dichromate, are known carcinogens. Chromium will irritate the mucous membranes. Therefore, take care to perform this demonstration in a well-ventilated area (preferably a ventilation hood) and avoid skin contact or inhalation of the materials. Wear gloves and safety goggles when handling ammonium dichromate.
References
B.Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Vol. 1, University of Wisconsin Press, 1986, pp. 81-82.
Delights of Chemistry, University of Leeds.
Old Nassau
This experiment continues the theme of `clock' reactions. The demonstration is known as the `Old Nassau Reaction', a clock reaction which turns orange and then black (and has therefore also been named the `Halloween Reaction') [1]. As Alyea describes [1] `the formation of orange HgI2 was discovered accidentally by two Princeton undergraduates ... when they were carrying out original research on the inhibition, by Hg2+, of the Landolt reaction'. From this, by reducing the Hg2+ concentration, the present demonstration was subsequently developed [2].
The name `Old Nassau', comes from Nassau Hall which was named after William III, King of England, Prince of Orange and Nassau. Nassau Hall can boast of a colourful history [1]. `At the time it was built it was the largest college building in North America. On January 3, 1777 General Washington crossed the Delaware to sieze the British ammunition stored there: his victorious Battle of Princeton followed. In 1796 it was perhaps the earliest undergraduate chemistry laboratory in the world,* where Dr John Maclean, Professor of Chemistry, had the students, themselves, carrying out chemical experiments. At that time Europe still practised apprenticeship: colleges in the New World gave only lecture demonstrations. In the late 1830s, several years before Samuel Morse sent his first telegraph message, Dean Joseph Henry, using an electromagnet, sent `clicks' from his office in Nassau Hall to his home nearby to alert his servants that he was coming home shortly, and to start heating water for his tea'.
The reaction in this experiment takes place in several steps [5]. First, sodium metabisulphite reacts with water to form sodium hydrogen sulphite:
Na2S2O5 + H2O ==> 2 NaHSO3 (10.1)
Hydrogen sulphite ions reduce iodate(V) ions to iodide ions:IO3- + 3 HSO3-==> I- + 3 SO42- + 3 H+ (10.2)
Once the concentration of iodide ions is large enough that the solubility product of HgI2 (4.5 x 10-29 mol3 dm-9) is exceeded, orange mercury(II) iodide solid is precipitated until all of the Hg2+ ions are used up (provided that there is an excess of I- ions).Hg2+ + 2 I-==> HgI2 (orange or yellow) (10.3)
If there are still I- and IO3- ions in the mixture, the iodide-iodate reactionIO3- + 5 I- + 6 H+==> 3 I2 + 3 H2O (10.4)
takes place and the blue starch-iodine complex is formed,I2 + starch ==> complex (blue or black) (10.5)
A full account of the reaction can be found in Shakhashiri’s book [6].Preparation. The following three solutions need to be prepared.
A. Make a paste of 4 g of soluble starch with a few mils of water. Pour onto this 500 ml of boiling water and stir. Cool to room temperature, add 13.7 g of sodium metabisulphite (Na2S2O5) and make up to 1 l with water.
B. Dissolve 3 g of mercury(II) chloride in water and make the solution up to 1 l with water.
C. Dissolve 15 g of potassium iodate (KIO3) in water and make the solution up to 1 l with water.
Demonstration. Mix 50 ml of solution A with 50 ml of solution B. Then pour into this mixture 50 ml of solution C. After about 5 seconds the mixture will turn an opaque orange colour as insoluble mercury iodide precipitates. After further 5 seconds the mixture suddenly turns blue-black as a starch-iodine complex is formed. The second colour change (orange to black) is not normally expected by the audience and comes as a real surprise.
This experiment can be extended in several ways [5]. Diluting all the solutions by a factor of two increases the time taken for the colour changes to occur. Using a smaller volume of solution B speeds up the reaction. The effect of changing the amounts and concentrations of the various reactants cannot always be predicted simply because of the complexity of the system. For example, if the volume of solution B is doubled, the appearance of the orange colour is delayed and the blue colour fails to appear at all.
If using mercury salts is not desirable, a somewhat simpler clock reaction can be performed. This is known as iodine clock reaction or Landolt reaction. The experiment is performed by mixing equal volumes of two solutions, one containing 2 g dm-3 KIO3 and H2SO4 0.03 M; the second - 0.4 g dm-3 of NaHSO3 in starch (2 g dm-3) previously dissolved in boiling water. The initially colourless mixture suddenly turns dark blue. There are several extensions to this reaction as well, which can be found, for example in Ref. [7].
Safety. All soluble mercury salts are poisonous and should be treated accordingly.
References.
1. Tested Demonstrations in Chemistry, ed. G.L. Gilbert, et al., Denison University, Granville, OH, 1994, vol. 1, p. I-49.
2. H.N. Alyea, J. Chem. Educ., 1955, 32, 9.
3. B.N. Menschutkin, `A Russian physical chemist of the eighteenth century', J. Chem. Educ., 1927, 4, 1079.
4. H.S. Van Klooster, `The beginnings of laboratory instruction in chemistry in the USA', in Chymia: Annual Studies in the History of Chemistry, ed. T.L. Davis, vol. 2, Philadelphia, University of Pennsylvania Press, 1949, pp. 1-15.
5. T. Lister, Classic Chemistry Demonstrations, ed. C. O'Driscoll and N. Reed, London, Royal Society of Chemistry, 1995, p. 50.
6. B.Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Volume 4, Wisconsin, US, The University of Wisconsin Press, 1992.
7. Ref. 1, p. I-46
Next, our group found the demonstration to the Volcano reaction or the Ammonium Dichromate Reaction.
Ammonium Dichromate Reaction
By Anne Marie Helmenstine, Ph.D., About.com Guide
Introduction The eruption of an ammonium dichromate [(NH4)2Cr2O7] volcano is a classic chemistry demonstration. The ammonium dichromate glows and emits sparks as it decomposes and produces copious amounts of green chromium (III) oxide ash. This demonstration is simple to prepare and perform. The decomposition of ammonium dichromate commences at 180°C, becoming self-sustaining at ~225°C. The oxidant (Cr6+) and the reductant (N3-) are present in the same molecule.
(NH4)2Cr2O7 --> Cr2O3 + 4 H2O + N2
The procedure works well in both a lighted or darkened room.
Materials
- ~20 grams of ammonium dichromate
- sand tray or ceramic tile, for use in ventilation hood OR
- 5-liter round bottom flask and porcelain filtering funnel
- gas burner (e.g., Bunsen) OR
- butane lighter or match, for use with flammable liquid (e.g., ethanol, acetone)
If you are using a hood:
- Make a pile (volcanic cone) or ammonium dichromate on a tile or tray of sand.
- Use a gas burner to heat the tip of the pile until the reaction begins or dampen the tip of the cone with a flammable liquid and light it with a lighter or match.
- Pour the ammonium dichromate into a large flask.
- Cap the flask with a filtration funnel, which will prevent the majority of the chromium (III) oxide from escaping.
- Apply heat to the bottom of the flask until the reaction begins.
Chromium III and chromium VI, as well at its compounds, including ammonium dichromate, are known carcinogens. Chromium will irritate the mucous membranes. Therefore, take care to perform this demonstration in a well-ventilated area (preferably a ventilation hood) and avoid skin contact or inhalation of the materials. Wear gloves and safety goggles when handling ammonium dichromate.
References
B.Z. Shakhashiri, Chemical Demonstrations: A Handbook for Teachers of Chemistry, Vol. 1, University of Wisconsin Press, 1986, pp. 81-82.
Delights of Chemistry, University of Leeds.
Subscribe to:
Posts (Atom)