When propene gas is bubbled through a solution of bromine in aqueous sodium chloride,?
371449
CH3-CH=CH2 has an electrohilic addition of bromine.  The bromine adds to the double bond via an intermediate known as a bromonium ion.  This is essentially a polarised bromine molecule, with a small dipole.\n\n\n....Brd-\n....Brd+\n../....&#92;\nCH2-CH-CH3 (ignore the dots, only there for spacing).\n\n---->\n\n............+\nBr-CH2-CH-CH3   secondary carbocation is formed\n\nThe Br-Br bond then breaks the bromonium ion formally forms a single covalent bond with the terminal carbon, and creates a secondary carbocation.  The Br- formed from the breaking of the Br-Br bond then attacks the carbocation to form 1,2-dibromopropane.\n\nBecause you are doing the reaction in the presence of NaCl and H2O, then Cl- (from the NaCl) or -OH, from the water can also attack the formed carbocation, giving 1-bromo-2-chloropropane and 1-bromopropan-2-ol as a result.  \n\nThe reason for not generating any 2-bromo-1-chloropropane for example is that this would require the preparation of a primary carbocation.  This is far less stable than a secondary carbocation, so the three products described by far predominate in the reaction mixture
44675
For starters, these bubbles are not coming from the oxygen present in H2O, or any transition from gas to liquid state. The amount of activation energy it would take to break the H2O bond (plus the surrounding hydrogen bonds) to send liquid Oxygen to gas form is not going to come from room temperature. More likely, the gas bubbles you see are dissolved air. Your water has gone through many filtration stops and a multitude of meshes, all of which can dissolve small microscopic bubbles of air in the water. These either come out to the water-air interface or combine with neighboring bubbles (I would guess this reduces surface tension). You see the larger air bubbles.
661119
sodium chloride or salt
836098
Water vapor. If all water vaporize u will receive NaCl (crystal)  in vessel.
793017
Take 1.875 L of the .2 molar stock solution of NaBr and add .625 L of water to it and you get 2.5 L of a .15 molar solution of NaBr this just use the c1v1=c2v2 equation.\n\nNote:\nThis is the only way it could work. You do not want to add more NaBr because your concentration is already higher then desired.   If you just added 0.5L of water to the 2.0 L of .2 molar stock solution your molarity would still be to high at .16 meaning you have to dilute a smaller portion of your 2L .2 molar stock solution.
727659
1.when sodium and chlorine combine they lose their harmful properties and become altogether new substance\n\n2.carbon di oxide\n\n3.bauxite(alumina)
966324
Ether has a higher saturated vapor pressure than water. Thus the former boils at a lower temperature than the latter.
830149
Could be Liquid Gas. Need more info.
883409
I will assume that "salt" is referring to sodium chloride, NaCl.  The solubility of NaCl increases with increasing temperature and decreases with decreasing temperature.\n\nSince you are starting with a saturated solution (meaning that it contains the MAXIMUM amount of NaCl at that temperature) and you are cooling the solution to 20oC from 60oC, the cooler solution will not be able to keep the NaCl dissolved and you will observe small crystals of NaCl precipitating from the solution.
1420
Good question.   Could be a number of reason, but my guess would be that you have some salt in your boiling water.    When NaCl solution is placed in a flame the Na cation gets ionized and yellow light is given off.    It doesn't take much salt for you to see this effect.   You will see this even with regular tap water, since it also has a small amount of salts dissolved in it.    \nIn fact, standard distilled water is usually not pure enough to avoid this effect.    That's why chemist buy special stills to make ultrapure water for experiments.
38126
A gas can also flow and wet through condensation.
737669
Bond energy (in kJ/mol)\n\nF-F:158\nCl-Cl: 244\nBr-Br-:193\nI-I: 151\n\nHence, in order of decreasing bond strength:\nCl-Cl => Br-Br => (F-F) =>  I-I\nFluorine is an anomaly.\n\nBond strength decreases from chlorine to iodine as down the group, the atomic size becomes larger and thus the valence electron orbitals become more diffused, causing the overlap of orbitals to become less effective. Therefore the halogen-halogen bond becomes weaker from chlorine to iodine.\n\nFluorine is an exception due to its extremely small size. The F-F bond length is so short that the lone pairs of electrons on the fluorine atoms repel each other and weakens the F-F bond.\n\nI hope that answers your question.
710667
A) Sodium and Chlorine yields Sodium Chloride.\n\nB and C) --> http://en.wikipedia.org/wiki/Conservation_of_mass
540602
it's a brine solution. as the salt dissolves on the water...
921966
Br2 is extremely soluble in CCl4 - much more soluble than in water.\nLook up "partition".
351009
Water with a high salt concentration, and plasma (electrically charged gas)
163806
It dissociates the bond between the sodium and chlorine atoms. Technically, it ceases to be a "salt" and becomes an electrolyte.