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Bromine weighs 3.104 gram per cubic centimeter or 3 104 kilogram per cubic meter, i.e. density of bromine is equal to 3 104 kg/m³; at 25°C (77°F or 298.15K) at standard atmospheric pressure.1 mol O contains 6.022×1023O atoms;its mass is 16.00 g. 1 mol Br contains 6.022×1023Br atoms;its mass is 79.90 g.Density of Bromine is 3.12g/cm3.
| Atomic number | 35 |
|---|---|
| Density | 3.1 g.cm–3 at 20°C |
| Melting point | – 7.2 °C |
| Boiling point | 58.8 °C |
| Vanderwaals radius | 0.165 nm |
Contents
How many grams does bromine have?
1 mol O contains 6.022×1023O atoms;its mass is 16.00 g. 1 mol Br contains 6.022×1023Br atoms;its mass is 79.90 g.
What is the density of bromine?
| Atomic number | 35 |
|---|---|
| Density | 3.1 g.cm–3 at 20°C |
| Melting point | – 7.2 °C |
| Boiling point | 58.8 °C |
| Vanderwaals radius | 0.165 nm |
What is the density of bromine in kg m3?
Density of Bromine is 3.12g/cm3.
What is the density of bromine g mL?
In your case, liquid bromine is said to have a density of 3.102 g mL−1 , which means that every 1 mL of bromine has a mass of 3.102 g .
What is bromine used for in hot tubs?
Bromine is a popular hot tub sanitiser, an alternative to chlorine. It’s more suitable for those with sensitive skin and has a less harsh odour than chlorine. It’s also more stable, so the levels stay more consistent.
Is bromine a heavy metal?
Properties. Bromine is the third halogen, being a nonmetal in group 17 of the periodic table.
What happens if you touch bromine?
Immediate signs and symptoms of exposure to bromine
Getting bromine liquid or gas on your skin could cause skin irritation and burns. Liquid bromine that touches your skin may first cause a cooling sensation that is closely followed by a burning feeling.
What happens if you drink bromine?
Ingestion of liquid bromine can cause abdominal pain and hemorrhagic gastroenteritis with secondary shock. Signs and symptoms might also include brown discoloration of mucous membranes and the tongue (1, 2).
Is bromine an explosive?
The reaction between potassium and bromine (gas) is vigorous with incandescence. A violent explosion will occur if potassium is brought in contact with liquid bromine. The system bromine-plus-sodium, however, requres a small impact to cause an explosion.
What is the molar mass of br2?
What is the density of bromine water?
…
Section 1: Properties of Bromine.
| Density of Liquid Bromine (g/ml) | |
|---|---|
| 15°C | 3.1396 |
| 20°C | 3.1226 |
| 25°C | 3.1055 |
What is the densest element?
…
| Discovery date | 1803 |
|---|---|
| Origin of the name | The name is derived from the Greek word ‘osme’, meaning smell. |
| Allotropes |
Why is bromine a liquid?
Bromine, on the other hand, has a slightly higher molecular weight than fluorine and has stronger intermolecular interactions, thus it persists as a liquid at ambient temperature.
What is the difference between bromine and bromide?
Bromine is a chemical element of the halogen group, which includes fluorine, chlorine, iodine and astatine. Bromide is an anion of bromine, commonly found in trace amounts as salt in sea-water, along with sodium chloride (common table salt).
How many grams does bromine react?
| Substance | Before Reaction | After Reaction |
|---|---|---|
| Aluminum | 10.3 g | 0.0 g |
| Liquid Bromine | 100.0 g | 8.2 g |
| Compound | 0.0 g |
What is the mass number of bromine?
What is bromine made of?
Natural bromine is a mixture of two stable isotopes: bromine-79 (50.54 percent) and bromine-81 (49.46 percent).
What is bromine gas?
Bromine is a naturally occurring element that is a liquid at room temperature. It has a brownish-red color with a bleach-like odor, and it dissolves in water.
Bromine volume to weight conversion
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2.8: The Mole – Chemistry LibreTexts
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Bromine (Br) – Chemical properties, Health and Environmental effects
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Chemical properties of bromine – Health effects of bromine – Environmental effects of bromine
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Bromine – Atomic Number – Atomic Mass – Density of Bromine | nuclear-power.com
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Question #d36b2 | Socratic
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- Most searched keywords: Whether you are looking for Question #d36b2 | Socratic Updating “15.2 mL” As you know, the density of a substance tells you the mass of exactly one unit of volume of that substance. In your case, liquid bromine is said to have a density of “3.102 g mL”^(-1), which means that every “1 mL” of bromine has a mass of “3.102 g”. color(blue)(color(purple)(“3.102 g”) color(white)(.)”mL”^(-1)) -> color(purple)(“3.102 g”)color(white)(.) color(black)(“for every”) color(white)(.)color(blue)(“1 mL”)color(white)(.)”of liquid Br”_2 Now, your goal here is to figure out the volume of liquid bromine that would contain 0.295 moles of bromine. In order to be able to do that, you must convert the number of moles of bromine to grams. Bromine has a molar mass of “159.808 g mol”^(-1), which means that every 1 mole of bromine has a mass of “159.808 g”. In your case, the sample of liquid bromine will have a mass of 0.295 color(red)(cancel(color(black)(“moles Br”_2))) * “159.808 g”/(1color(red)(cancel(color(black)(“moles Br”_2)))) = “47.14 g” You can now use the density of liquid bromine as a conversion factor to determine exactly how many milliliters of bromine would have a mass of “47.14g” 47.14 color(red)(cancel(color(black)(“g”))) * color(blue)(“1 mL”)/(color(purple)(3.102)color(red)(cancel(color(black)(“g”)))) = color(darkgreen)(ul(color(black)(“15.2 mL”))) The answer is rounded to three sig figs, the number of significant figures you have for the number of moles of bromine present in the sample.
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Bromine weight to volume conversion
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- Summary of article content: Articles about Bromine weight to volume conversion Bromine weighs 3.104 gram per cubic centimeter or 3 104 kilogram per cubic meter, i.e. density of bromine is equal to 3 104 kg/m³; at 25°C (77°F or 298.15K) at … …
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Convert moles Bromine to grams – Conversion of Measurement Units
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- Summary of article content: Articles about Convert moles Bromine to grams – Conversion of Measurement Units Do a quick conversion: 1 moles Bromine = 79.904 gram using the molecular weight calculator and the molar mass of Br. … How many moles Bromine in 1 grams? …
- Most searched keywords: Whether you are looking for Convert moles Bromine to grams – Conversion of Measurement Units Do a quick conversion: 1 moles Bromine = 79.904 gram using the molecular weight calculator and the molar mass of Br. … How many moles Bromine in 1 grams? Do a quick conversion: 1 moles Bromine = 79.904 gram using the molecular weight calculator and the molar mass of Br. Check the chart for more details.
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How much does 1 molecule of bromine weigh? I know the atomic mass for bromine is 79.90 g
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2.8: The Mole – Chemistry LibreTexts
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- Summary of article content: Articles about 2.8: The Mole – Chemistry LibreTexts … the introduction to moles would contain 4.080 x 1022 mercury atoms, for example, and the 3.47 cm3 of bromine would contain twice as many … …
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Bromine volume to weight conversion
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Because atoms and molecules are extremely small, there are a great many of them in any macroscopic sample. The 1 cm3 of mercury referred to in the introduction to moles would contain 4.080 x 1022 mercury atoms, for example, and the 3.47 cm3 of bromine would contain twice as many (8.160 x 1022) bromine atoms. The very large numbers involved in counting microscopic particles are inconvenient to think about or to write down. Therefore chemists have chosen to count atoms and molecules using a unit called the mole. One mole (abbreviated mol) is 6.022 x 1023 of the microscopic particles which make up the substance in question. Thus 6.022 x 1023 Br atoms is referred to as 1 mol Br. The 8.160 x 1022 atoms in the sample we have been discussing would be
\[\dfrac {8.160\cdot10^{22}} {6.022\cdot10^{23}\text{ mol Br}} = \text {0.1355 mol Br}
onumber \]
The idea of using a large number as a unit with which to measure how many objects we have is not unique to chemists. Eggs, doughnuts, and many other things are sold by the dozen—a unit of twelve items. Smaller objects, such as pencils, may be ordered in units of 144, that is, by the gross, and paper is packaged in reams, each of which contains 500 sheets. A chemist who refers to 0.1355 mol Br is very much like a bookstore manager who orders 2½ dozen sweat shirts, 20 gross of pencils, or 62 reams of paper.
There is a difference in degree, however, because the chemist’s unit, 6.022 x 1023, is so large. A stack of paper containing a mole of sheets would extend more than a million times the distance from the earth to the sun, and 6.022 x 1023 grains of sand would cover all the land in the world to a depth of nearly 2 ft. Obviously there are a great many particles in a mole of anything.
Why have chemists chosen such an unusual number as 6.022 x 1023 as the unit with which to count the number of atoms or molecules? Surely some nice round number would be easier to remember. The answer is that the number of grams in the mass of 1 mol of atoms of any element is the atomic weight of that element. For example, 1 mol of mercury atoms not only contains 6.022 x 1023 atoms, but its mass of 200.59 g is conveniently obtained by adding the unit gram to the Table of Atomic Weights. Some other examples are
\[\begin{align} &\text{1 mol H contains 6.022} \times 10^{23} \text{H atoms;} & \text{its mass is 1.008 g.} \\&\text{1 mol C contains 6.022} \times 10^{23} \text{C atoms;} &\text{its mass is 12.01 g.} \\&\text{1 mol O contains 6.022} \times 10^{23} \text{O atoms;} &\text{its mass is 16.00 g.} \\&\text{1 mol Br contains 6.022} \times 10^{23} \text{Br atoms;} &\text{its mass is 79.90 g.} \end{align}
onumber \]
Here and in subsequent calculations atomic weights are rounded to two decimal places, unless, as in the case of H, fewer than four significant figures would remain.
The mass of a mole of molecules can also be obtained from atomic weights. Just as a dozen eggs will have a dozen whites and a dozen yolks, a mole of CO molecules will contain a mole of C atoms and a mole of O atoms.
The mass of a mole of CO is thus
\[ \text{Mass of 1 mol C + mass of 1 mol O = mass of 1 mol CO}
onumber \]
\[ \text{12.01 g + 16.00 g = 28.01 g}
onumber \]
The molecular weight of CO (28.01) expressed in grams is the mass of a mole of CO. Some other examples are in Table \(\PageIndex{1}\).
Table \(\PageIndex{1}\): Molecular Weight Molecule Molecular Weight Mass of 1 Mol of Molecules Br 2 2(79.90) = 159.80 159.80 g O 2 2(16.00) = 32.00 32.00 g H 2 O 2(1.008) + 16 = 18.02 18.02 g HgBr 2 200.59 + 2(79.90) = 360.39 360.39 g Hg 2 Br 2 2(200.59) + 2(79.90) = 560.98 560.98 g
Chemical properties, Health and Environmental effects
Bromine At ambient temperature bromine is a brownish-red liquid. It has a similarly colored vapor with an offensive and suffocating odor. It is the only nonmetallic element that is liquid under ordinary conditions, it evaporates easily at standard temperature and pressures in a red vapor that has a strong disagreeable odor resembling that of chlorine. Bromine is less active chemically than chlorine and fluorine but is more active than iodine; its compounds are similar to those of the other halogens. Bromine is soluble in organic solvents and in water. Applications Bromine is used in industry to make organobromo compounds. A major one was dibromoethane an agent for leaded gasoline, before they were largely phased out due to environmental considerations. Other organobromines are used as insecticides, in fire extinguishers and to make pharmaceuticals. Bromine is used in making fumigants, dyes, flameproofing agents, water purification compounds, sanitizes, medicinals, agents for photography and in brominates vegetable oil, used as emulsifier in many citrus-flavoured solft drinks. Bromine in the environment Bromine is a naturally occurring element that can be found in many inorganic substances. Humans however, have many years ago started the introduction of organic bromines in the environment. These are all compounds that are not natural and can cause serious harm to human health and the environment. In diffuse crustal rock bromine naturally occurs as bromide salts. Bromine salts have accumulated in sea water (85 ppm), from which bromine is extracted.
World production of bromine is more than 300.000 tonnes per year; the three main producing countries are US, Istrael and the UK. In this last case it is extracted from sea water at a plant on the coast of Anglesey, Wales. Health effects of bromine Bromine is corrosive to human tissue in a liquid state and its vapors irritate eyes and throat. Bromine vapors are very toxic with inhalation. Humans can absorb organic bromines through the skin, with food and during breathing. Organic bromines are widely used as sprays to kill insects and other unwanted pests. But they are not only poisonous to the animals that they are used against, but also to larger animals. In many cases they are poisonous to humans, too.
The most important health effects that can be caused by bromine-containing organic contaminants are malfunctioning of the nervous system and disturbances in genetic materials.
But organic bromines can also cause damage to organs such as liver, kidneys, lungs and milt and they can cause stomach and gastrointestinal malfunctioning. Some forms of organic bromines, such as ethylene bromine, can even cause cancer.
Inorganic bromines are found in nature, but whereas they occur naturally humans have added too much through the years. Through food and drinking water humans absorb high doses of inorganic bromines. These bromines can damage the nervous system and the thyroid gland. Environmental effects of bromine Organic bromines are often applied as disinfecting and protecting agents, due to their damaging effects on microorganisms. When they are applied in greenhouses and on farmland they can easily rinse off to surface water, which has very negative health effects on daphnia, fishes, lobsters and algae.
Organic bromines are also damaging to mammals, especially when they accumulate in the bodies of their preys. The most important effects on animals are nerve damage and next to that DNA damage, which can also enhance the chances of development of cancer.
The uptake of organic bromine takes place through food, through breathing and through the skin.
Organic bromines are not very biodegradable; when they are decomposed inorganic bromines will consist. These can damage the nerve system when high doses are absorbed.
It has occurred in the past that organic bromines ended up in the food of cattle. Thousands of cows and pigs had to be killed in order to prevent contagion of humans. The cattle suffered from symptoms such as liver damage, loss of sight and depletion of growth, decrease of immunity, decreasing milk production and sterility and malformed children. Back to periodic chart.
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