taking it away from  a solution... Im not quite sure of the right wording-just trying to comprehend the theory, process and solution end product. Ok lets say you have a water pipe? rt.? & so u are smoking  through it what does the water do..anything- does it filter  the bad /harsh chemicals or are you  still inhaling the?? but lets say your substance to begin with went through a process of seperating the oxygen molecule from the hydrogen in order to form its state now and you put that in your water pipe-and drawing it through the water as u smoke- now is that just defeating the purpose. I DO APOLOGIZE if this sounds all screwy-Im not sure of how 2 phrase what Im looking to say...but if u understand or grasp a little bit of a notion or understanding of what Im having a 'brain freeze' on saying -could u explain it 2 me ? THANKS ALOT!!!
130624
I'm not exactly sure what you're talking about, but yes, water can be separated into hydrogen gas (H2) and oxygen gas(O2). It's the following redox reaction.\n\nreduction: 2e- + 2H+ + H2O --> H2 + H2O\noxidation: 2H2O --> O2 + 4H+ + 4e-\n\nMultiply the reduction reaction by two and add the two together to get the final reaction.\n\n2H2O --> 2H2 + O2\n\nThe hydrogen goes down from a +1 state to a 0 state, and the oxygen goes up from a -2 state to a 0 state.
555211
I'm not 100% sure, but it seems like this procedure would neutralize any acids in the solution.  The Hydroxide would turn acid to water.  Any remaining hydroxide would combine with Calcium to form Calcium Hydroxide, which has a low solubility.  This would then precipitate out of the solution.  If the solution is mostly organic, it would also adsorb most of the water and remove it form the organic phase.
553114
H2SO4 will dehydrate and remove water.\n\n\n(CH3)2 CH - CH2-CH=CH-(CH3)2
356752
&#92;\n..&#92;\n..-----&#92;\n........&#92;\n.........&#92;\n(ignore the periods)\nx axis: time\nY axis: temperature\nThe step is there because the nature of cooling objects. As the naphthalene is cooled, its temp first decreases normally. However, when it begins to solidify, the heat being removed is used up as naphthalene molecules are subjected to intermolecular forces and begin to become a solid. Therefore, the horzontal part is where the substance becomes a solid. Finally, when the naphthalene is fully a solid, the temperature decreases again. An easy way to picture this concept is with boiling water. As some water molecules change to the gaseous state, the temperature of the water does not rise above its boiling point. This is equivilent to the horzontal part of the naphthalene cooling curve. As the substance changes states, energy is being generated/used up, and the temperature does not change for a time. When the conversiion is fully made, the temperature continus on its original course.
17492
I remember watching a vid withe a guy bringing a couple all sorts of bottled water from around the world. I mean we're talking $10 a bottle, but he let them sample them all. They noticed extreme differences to their liking.\n\nHis trick? Taking different shaped bottles into the back and filling them with hose water.\n\nMy point? It's pretty much a placebo effect. Kind of like seeing what you want to see ya know? I'm willing to bet that if you took a drink of one bottle, then the next, then were blind folded and drank each out of the glass, people couldn't pick the right one if you say had 6 bottles and had to do it 1,000 times. Because really, water is water. \n\nSpring water is clean, and that's why it will be better to a degree, but filtered water of the same temperature is just as good.
591866
Simple really...the H has already burned!  That's what formed the water.\n\nBurning is a chemical reaction...basically elements recombine w/ other elements.  The water is the end result of the burning, and cannot burn further.
262420
Now, THAT is what I call a challenging question! It requires some thinking in addition to the book-ish knowledge and I love it! But, before I continue with my answer, I'd just like to correct one statement:- "I know that peroxide reacts with metals and glass", It does NOT. Metals and glass act as catalysts i.e. they accelerate the reaction of conversion of Peroxide into Water and Oxygen but they don't participate in the reaction.\n\nNow coming to your question, the varying levels of fumes that you are observing have nothing to do with an organic reaction.\n\nLet's address all your situations one-by-one:\n======= ========== ============\n1- When you pour it around the faucet and it bubbles furiously around the crud and not on the spigot itself.\nThe reaction going on in there is the same ol' Peroxide converting to Water and Oxygen.\nOne molecule of Peroxide (liquid) ----> One molecule of Water (Liquid) + Half molecule of Oxygen (gaseous)\n\nWhich is Symbolically-\nH202 (l) -------> H2O (l) + (1/2)O2 (g)\n\nIt's just that the reaction takes place at a faster rate around the crud around the base! \n\nIn general, ANY rough surface acts as a CATALYST for this reaction. Try it yourself, put some peroxide on a smooth surface and then put some on a rough surface. You can easily see that it fumes and bubbles more on a rough surface. It is because on a rough surface there is more AMOUNT of surface on a given area due to all the unevenness of the surface. And more area accomodates more peroxide which leads to more reaction for a given area and hence a faster rate.\n\n======= ========== ============\n2. When you drop earings into peroxide, the whole earings don't bubble only the "gunk" does and when that's gone it stops!\n\nHmm.. This required a little bit of thought process: The "gunk" in your earrings can be two things-\na) Deposition of Dust or dead skin-\nIf this is the case, then the answer would be- "Rough surfaces and dust CATALYZE the reaction of conversion of Perxide into Water and Oxygen which I have already metioned."\n\nb) Deposition of METAL OXIDE because of rusting or corrosion  or tarnishing of your earring.\nNow, if THIS is the case, then the bubbles are coming out due to the REDUCTION reaction by peroxide in the acidic medium.\nLet's see what's happening in there-\nThe Metal Oxide on the surface of your metal earrings is an oxidising agent i.e. it releases Oxygen (Oxygen atom). In presence of an oxidising agent, the Peroxide acts as a reducing agent. It reacts with the oxygen atom like this-\n\nH2O2 (Peroxide) + [O] (Oxygen atom from the rust) -----> H20 (Water) + O2 (Oxygen molecule)\n\nYou can see that Oxygen is being released here, THAT CAUSES THE BUBBLES!\n\n======= ========== ============\n3- It bubbles on cuts but, not on normal skin!\nWhoa whoa whoa... Don't put it on your skin, the reaction of it's conversion to water is exothermic (gives out heat) and sometimes, explosive!\nNow, to answer the question, it might be the tiny dust particles in your abrasion that could be triggerin' off the decomposition reaction & causing the release of Oxygen gas bubbles \nOR as you might be knowing that the pH of the blood is MORE THAN 7, i.e. it is basic or alkaline in nature AND in alkaline solution, this reaction takes place-\nFerrous(Iron) Ions (Fe +3) + Peroxide (H2O2) + Hydroxyl Ions (OH-) ----------> Ferric (Iron) Ions (Fe 2+) + Water (H20) + OXygen Molecules\n\nDid you see that? One of the products in the reaction up there was Oxygen molecules!! Now, that means that we are gonna have some bubbles there as Oxygen gas is gonna bubble baby!\n\nP.S. This is perhaps the longest answer I have ever typed in my entire life!
39368
It depends on the specific heats of the compounds in the liquid.  Specific heat is a measure of how much energy it takes to raise the temperature of one gram of the compound by one degree (and consequently the amount of energy it will need to get rid of to cool back down), and is a property of the compound (i.e. it doesn't change unless you alter the chemical composition of the compound).  Basically, if you have something with a high specific heat, it has to get rid of a lot more heat (a measure of energy, not temperature) to reach the same temperature as something with a lower specific heat.  When the liquids cool, they have to give the extra heat to the air, and can only do so if the air they are touching is cooler than they are.  So it takes time for a liquid to transfer some if its heat to the air.  If there's more to transfer, it takes longer (just like downloading a bigger file).\n\n__________\nFreezing and boiling points and intermolecular forces are only relevent to phase changes.  The question is about a liquid that is staying a liquid and just changing temperature.  The above answers are all wrong.
474401
As the temperature of a liquid increases, the less gas it can hold dissolved. If you set a cold glass of water on the counter, it contains dissolved air. That is what th fish breath, dissolved air. As it warms less air can stay dissolved, so it comes out of solution on the side of the glass.\n\nIt is not the H or O from H2O
275536
Sorry but to divulge Genters location would be futile.  Attempts made at this, will result in your molecules being vaporized and then transformed into 46c4 carbon based atoms, which will then be erased
253664
The reaction is as follows:\n\nCaCO3 + 2HCl -----------> CaCl2 + H2O + CO2\n\nThe reaction produces H2O & CO2 as biproducts and CO2 at room temperature will be a gas. So it will escape from the recation media (Contaner)\nAs a result, this reaction is not a reversible reaction (since one byproduct is missing) and hence as time goes water will adds up and HCl will dilute more and more ... rection kinetics slowed down.\n\nCaCl2 is very much  soluble in water.. so its not the reason\n\nIs this answer is enough to deserve 10 pts from you?\n\nHave fun in chemistry always!
655482
You can perform electrolysis of water (or electrolysis of dilute sulphuric acid as it is called). The apparatus used is a Hoffman's voltmeter, with platinum electrodes. On passing an electric current, H+ and OH- ions in the water molecule dissociate and migrate to the corresponding electrodes.\n\nAt cathode: H+  + e- --------> H(g)\nH(g) + H(g) --------> H2(g)\n\n2 volumes of hydrogen are released at cathode.\n\nAt anode: OH- (aq) -----------> OH(g) + e-\nOH(g) + OH(g) -----------> H2O + O(g)\nO(g) + O(g) -------------> O2(g)\n\n1 volume of oxygen released at anode\nThus hydrogen and oxygen are released at a ratio of 2:1
338815
Ok, here's how it breaks down.  Water freezes in a unique way compared to most other liquids.  Water freezes in a crystalline latice structure that looks like layers of hexagons.  That's why water expands when it freezes into ice.\n\nNow the second part of the answer is that when you dissolve something like salt or sugar into water, you lower the freezing point of water.  The additives or solutes disturb the way that water freezes by interfering with the water molecules as they try to freeze into their lattice pattern.  This disturbance does not fully prevent water from freezing, it only lowers the freezing point.  As long as it's cold enough, water can still freeze into ice.  By lower the freezing point, the water needs to get colder and colder to be able to turn into ice.  The other side of this is that you can dissolve more things in a hot liquid than a cold liquid.  When you dissolve something to its limit into a liquid, it's called saturating the liquid.  Also, you can dissolve a lot of something in a liquid when it's hot, but then let it cool without disturbing it and it will be a supersaturated solution.\n\nBeer is not only a solution (something dissolved in water), it is a special solutions because of carbonation.  The process of carbonation involves forcing carbon dioxide bubbles through water to  force the carbon dioxide to dissolve in the water or in this case beer.  When they bottle beers, the company is actually supersaturating the beer with carbon dioxide, that's why it always foams a little when opened.\n\nBecause beer has carbon dioxide in it, it's freezing point is lowered so it is less likely to freeze.  When you cool the beer down below freezing with the cap on, the beer will not freeze, but once you open it, you release the carbon dioxide.  As the beer quickly loses the dissolved carbon dioxide, the freezing point for the beer quickly goes up.  Once freezing point gets up to the temperature of the superchilled beer, the beer freezes and turns into a solid.
585810
Water, when heated from a solid to liquid state, but ultimately in a gaseous state it again expands.  It still obeys all the laws of chemistry, but the bonds just arrange themselves in a more space efficient manner in liquid than in solid form.\n\nAnd moses with a P, no metals exist with the properties you say.  It is physically impossible, sorry man, but I'm a biochem major and it's my job to know what stuff does under different stresses, and nothing does what you claim.  However, if you do have a material that does this, get in touch with me, we'll talk to the patent office, and we'll license it out to companies for billions of dollars.
132882
Extracting Methane from Water?\n\nUsually, there isnt much methane in water.  Methane, being a non-polar Hydrocarbon, does not readily dissolve in polar solvents like water.\nHowever, if by chance you actually did have some CH4 dissolved in water, a gas' solubility in water decreases as pressure decrease and temperature increases, so by boiling the water and/or lowering the atmospheric pressure above the liquid, the methane can be removed.
276982
I don't know that you can, different solvents react differently to pressure, so I don't think it's a one eqaution fits all kind of process.  That's why they all have different graphs for phase vs temperature/pressure.  I'm sorry.\nSounds like you have a pretty high boiling point though, the things I've taken off that had to be real high temp were water, toluene, and pyridine.  Could it be one of them?  They smell pretty different, so you'd know which.  \nThat's an interesting question though, I've never stripped a solvent that I didn't know what it was.
668779
WoW Dude! Hydrogen and oxygen BOTH in water! Now that is just so new-age and just today right? \nDamn Man! If you and I could just figure how to separate the two...\nSorry got lost in the thought! Please submit your picture to Ripley"s...