A mercury mirror forms inside a test tube by the thermal decomposition of mercury(II) oxide.?
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It seems that you have problems with moles and Avagadro's number. You will need to refer to your periodic table to get the molecular weights that your teacher wants you to use.\n\nSo get the molecular weights of the elements you are working with from your periodic table and substitute in the formula.\n\nI am using round numbers to show the substitution you should know how many decimal points you need to work to.\n\nHG atomic weight 200\nO atmic weight 16\n\nSubstitute in the formula to get the masses involved\n\n2 HgO(s) - 2 Hg(l) + O2(g) Hrxn = 181.6 kJ\n 2 (200g + 16g)   =  2(200g) + 2(16g) = 181.6 kj  \n\n432g oxide decomposes releasing 181.6Kj\n\nQuestion a)\nStraightforward ratio. X = the no of KJ required\n\n572g/432g = xkj/181.6kj\n\nYou'll need to calculate the molecular mass from you periodic table substitute it for the 432 and then refine the equation.\n\nQuestion b) Straightforward ratio. X = the no of KJ required\n\nYou'll need to calculate the molecular mass from you periodic table substitute it for the 432 and then refine the equation.\n\n289/181.6 = xg/432\n\nA mole is the amount of pure substance containing the same number of chemical units as there are atoms in exactly 12 grams of carbon-12 (i.e., 6.023 X 1023). This involves the acceptance of two dictates -- the scale of atomic masses and the magnitude of the gram. Both have been established by international agreement. Formerly, the connotation of "mole" was "gram molecular weight." Current usage tends to apply the term "mole" to an amount containing Avogadro's number of whatever units are being considered. Thus, it is possible to have a mole of atoms, ions, radicals, electrons, or quanta. This usage makes unnecessary such terms as "gram-atom," "gram-formula weight," etc.
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Mercury is toxic in several ways.\nAt room temperature is gives off a vapour (which can be seen if you shine an ultra-violet light onto a screen in front of which is a bowl of mercury). As a vapour it is quickly absorbed through the lungs.\nIt is absorbed through the skin but very slowly. Only a small proportion is absorbed by the digestive system if the metal is swallowed. You would have to take almost a table-spoon full to make you seriously ill or kill.\nMercury compounds are seriously poisonous especially soluble ones like the chloride. Organo-mercury are the worse as they are very readily absorbed into the tissues of the body.\nMercury is very good at replacing the trace metal elements in the body such as copper, cobalt, chromium etc. At autopsy it can be found in almost every tissue in the body.\nIt is slowly eliminated from the body taking about 70 days for half of it to leave and another 70 days for half of the remaining to go.\nIt causes a whole host of illnesses from loosening of teeth, mental disturbance and organ failure.
319335
It's liquid hydrogen and oxygen.  I imagine they just make it in a factory by cooling down those gases to very low temperatures.
678316
what I know is that its a special machine that can magnify the elements to nanometers where you are able to see it. If you used this machine on lets say a NaCl crytyl lattics, you would see the solid as Na+ ions and Cl- ions coming together in an organized lattice.
35280
The Ksp of the reaction\n\nHgS <--> Hg + S\n\nis 2*10^-53. Extremely insoluble.
676026
Wild guess here... a dihydrate of copper chloride.\n\nSecond guess would be copper sulfate, possibly from the manufacturing process.
484472
This could happen one of two ways:\n\n1) The mirror is made of another material than glass or the usual material used.\n\nOR\n\n2) The mirror has curvatures somewhere along the way creating a distorted image.\n\nHope this helps!
62318
Chemical companies sell it.  check out this:\nhttp://www.sigmaaldrich.com/catalog/search/ProductDetail/SIAL/215457\nAldrich sells 99.9995% pure mercury.  That's as good as it's going to get.
260568
Depending upon whether it is metallic mercury or a mercury compound, different rules apply.\nYou can get some ideas at the site below:
373543
A nitric acid solution should break mercury down to it's ions.
389575
GOLD-PLATINUM-PALLADIUM TEST\nBy Delos Toole\n\nSelect ore samples suspected to contain Gold-Platinum-Palladium and use concentrates equal to the size of one navy bean or pea. Place the concentrates in a clean test tube and add 1cc Nitric Acid and 3cc Hydrochloric Acid, (this a solution named Aqua Regia which is used regularly when testing.) Boil this over a lamp flame for about 5 to 8 minutes. Should this Aqua Regia solution contain Gold-Platinum-Palladium then the following tests will react with various colors, (good idea to practice on known samples of Gold-Platinum-Palladium for color and reaction identification and become familiar to them.)\n\nTest for Gold (Au).\n\nPrepare a solution for Stannous Chloride for each 8 hour period as this solution does not hold up under extended time periods. Dissolving Metallic Tin (Sn) in Hydrochloric Acid (HC1), where the resulted solution will be called Stannous Chloride (SnC1). Place about 2cc of HC1 in a clean test tube and add 1 or 2 small bit pieces of Metallic Tin to the test tube and bring this to a slight boil. You now have Stannous Chloride (SnC1).\n\nNow begin the gold test by making a spot test with freshly made Stannous Chloride by placing a piece of filter paper onto a clean piece of glass and place one drop of Aqua Regia solution in the center of the filter paper, and then add to this mixture one drop of freshly made Stannous Chloride solution. If gold is present there will show up on the filter paper a purple or rose colored spot when the filter paper has dried; the darker the color the more gold will be present; for low grade ore the spot color will appear plainer. Should the filter paper dry out completely, then add 1 more drop of Stannous Chloride solution to the filter paper to bring out the color.\n\nBegin the test for Platinum (Pt) by placing 20 drops of Aqua Regia solution onto a clean porcelain evaporating dish and boil this over a lamp flame until it is dry, then allow this to remain over the lamp flame for about an extended one second.\n\nPlace the dish where it can cool for a few minutes so as not to break the dish. After cooling, place 4cc of distilled water, (or water free from Chlorine), and reheat just to the boiling point. Filter this solution onto another clean porcelain evaporating dish. Add to this dish, Potassium Iodide equal to one grain of rice. Warm this solution slightly over the lamp flame and observe the color that appears. The results for this test will show if Platinum (Pt) is present as the solution will begin to turn to a light or dark rose color within a few minutes time.\n\nThe more Platinum present in the solution, (ore sample), the quicker and darker the color will appear.\n\nSulphides and other impurities, most likely will give a red color to the solution and will be mistaken for the rose color, if so, then boil off about one-half of the solution to quicken the evaporation process. Then let the porcelain dish set until completely dry, then add a few drops of clean plain water, (no chlorine water). The result will then be a bright rose color, and should there be Sulphides or other impurities in the solution they will appear as colorless. If this solution should appear red, then add a few cc’s of plain water to dilute the dark rose color to a lighter rose color, then you have Platinum (Pt).\n\nTesting for Palladium(Pd).\n\nIn the test for Platinum (Pt), upon adding Potassium Iodide (KI) and warming the procedure, if Palladium (Pd) is present in the sample ore, the solution will turn a dark color or black, which depends upon the amount of Palladium (Pd) present. The more Palladium (Pd) present, the darker the color will be, and also there will be a black precipitate in the bottom of the porcelain dish, which when adding an excess of Potassium Iodide (KI) will dissolve giving a wine-red color appearance.
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it dissolves alot of stains. and it has a certain alkali quality to it that it helps cleaning chemically without hurting the test tube.
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Some oxide of chlorine. No idea about which one would be stable at those conditions, though.
431570
um, no. It's not mercury. Liquids can mean any liquid, not just a periodic element. Lauric Acid has an atomic mass of 280g/mole, which is OVER any element by itself and it's melting point is at *negative*16 degrees Celsius. Long fatty chains like vegetable oils are in multiples of that.
429367
It doesn't form into anything. You said it yourself, it's soluble. The hydroxide part of the milk of magnesia (magnesium hydroxide) and the hydrogen of the sulfuric acid combine to form water, but then you're left with Mg+2 and HSO4- ions. It's just a clear liquid.
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When silane burns, SiO2 is formed (and water). You can now draw up the balanced equation.\n\nManganese(IV) oxide catalyses the decomposition of hydrogen peroxide:\n\n2H2O2 ----> 2H2O + O2
110506
Ammoniated mercury is an effective material for dermalogical cases ,how ever if th econcentrationis more than the therapeutic need it may be absrbed by the skin and cause mercury poisining