How can you tell that chlorine is a gas at room tempature?
461298
you observe it at room temperature.\n\nyou can do this by :\n\n1. smelling it ( it smells like clorox or a swimming pool.\n\n2. run it thru water- it will bubble and dissolve causing the water to smell like the above.\n\n3. use chemical analysis to confirm the gas is chlorine at room temp.\n\nhope it answers you question ( unusual )
791970
Use the Gay-Lussac gas law: V/T is constant. Note that T here is the temperature in Kelvin, not in Celsius. Luckily 27 C = 300 K
1030535
Well, this is easy. Just look at each species and see if its oxidation state is going up or down. I'll do the first one--the rest are the same.\n\nH2S + Cl2 --> 2HCl + S\n\nWell, the sulfur is going from a -2 state to a 0 state. This means it's oxidizing. The chlorine is going from a 0 state to a -1 state. This means it's reducing. So, the sulfur is the reducing agent (because it's making the chloringe reduce) and the chlorine is the oxidizing agent. Be careful--oxidizing agent actually means it's reducing.\n\nSolve the other two the same way.
49337
At room temperature, 0.968 g/cm³
171304
Absolutely!  First off, chlorine does evaporate into the air.  So long longer it sits, the less chlorine it has.  Unfortunately that also means the longer it sits, you should boil it before drinking.  At the pool that I worked at, we did a test on the water and the tap water.  Oddly enough, our county water contained a much higher PH level (more alkaline) than the pool which is around 7.6ph.
24312
Depends on temp and pressure, but at room temp, avg. pressure, helium's a gas
1167951
HgCl2 - 0.48 mol / 100 mol water at 25 degrees C\nHg2Cl2 - very insoluble in water
183538
I can't give you a sketch, but I can tell you how.\n\nThere are naturally occuring brines (very salty water if you aren't a specialist) which are mainly Potasium Bromide (KBr) in water. \n\nThis is put into the top of a tower and flows downwards over a series of internal plates or trays. \n\nAt the same time, Chlorine gas is sent upwards though the same tower so that the gas (Cl) and the salts (KBr) are in contact. The Cl replaces the Br in the salts and liberates free Bromine. \n\nThe liquid which come out the bottom of the tower is mainly KCl, potasium chloride solution.\n\nYou should find a typical type of tower if you do a search on Contactor Tower or Contactor Column on the web.
362437
law of conservation of energy\nany gas that is compressed will 'lose' its heat energy to the ambient temperature in the process (ie a refrigerator). in the specific example the gas (1 cm3 at 70F )is at room temperature until its expanded to lets say 1000 cm3, now 70F is spread out 1000x the area,(as is the gas in the can) the more the 70F is expanded the 'colder' it gets (much like the universe or a car tire, but its all relative)
429574
gas emitting visible light as a result of being heated
902790
First, you find the pressure of Cl2.  Then you use PV=nRT to find the moles of Cl2.  Then you convert moles of Cl2 into the mass of Cl2\n\nThe total pressure is the sum of the partial pressures.\n\nTotal pressure = Pressure of CH4 + Pressure of Cl2\n\nPressure of Cl2 = Total pressure - Pressure CH4\n\nPressure of Cl2 = 0.445 - 0.145 = 0.300 atm\n\nNow just use the formula PV=nRT to find the moles of Cl2:\n\nPV = nRT\n\nn = PV/RT\n\nn = (0.300)(.403)/(0.0821)(301)\n\nn = 4.89 x 10^(-3) moles of Cl2\n\nMass of Cl2 = moles of Cl2 * molar mass of Cl2\n\nMass of Cl2 = (4.89 x 10^-3) * (2*35.45)\n\n*** Mass of Cl2 = 0.35 g
561048
Some oxide of chlorine. No idea about which one would be stable at those conditions, though.
942319
This is what you should be looking at:\n\nHCl(gas) + NH3(gas)  -->  NH4Cl (solid)
703096
Charles' law states that, under constant pressure, the ratio between a gas' volume and absolute temperature remains constant.  So if it heats up it expands and if it cools it contracts.  For example, you fill a balloon with helium at room temperature, and then put it in a refrigerator.  The helium will contract, and the balloon will shrink.
327225
The elements Chlorine and Nitrogen are found in their natural, elemental forms of Chlorine gas (Cl2) and Nitrogen gas (N2) in nature, not as atomic Chlorine or atomic Nitrogen.\n \nNitrogen gas makes up the majority of Earth's atmosphere (AKA "air").\n\nChlorine gas is faily easy to produce with electrochemical reactions, or even through standard (non electrolytic) reactions.\n\n\nClorox does NOT contain Chlorine gas.  Amongst other things, the active ingredient in clorox bleach is Sodium Hypochlorite (NaOCl), not "Chlorine".
361097
As you are thinking - no, it doesn't. It stays in solution in the water. If / when some water evaporates, remember that chlorine will just dry, because chlorine has chemically bonded to other minerals in the water so that it can't become a gas. That's the residue left behind (or a part of it, anyway) when the drops in your shower dry.\n\nHowever, let's just say that chlorine does turn into an gas when the water evaporates (for argument's sake). The amount of chlorine in the water is measured using PPM, or Part Per Million. Thus, the level of chlorine that is in the water is so low (just enough to kill micro organisms), that it would cause no ill health effects to either you or me.
604299
Chlorine concentration as in reactive Cl2 or chlorate (which will react similarly): iodometric titration or direct reaction to a dye which can be detected with a photometer.\n\nTotal chlorine content: coulometry (with silver electrodes), e.g. after evaporating an entire water sample in an AOX analyzer with added charcoal and nitrate to transform all the chlorine in the sample into gaseous (and dried) HCl. Elemental analyzers for biological samples work similarly.