what is the flammability of potassium?
488199
Potassium is SO flammable, that if it is dropped in WATER it will rip the oxygen away from the hydrogen and burst into flames! \n\nThat is why it is kept in oil or kerosene, to avoid the possibility that it will come into contact with any moisture. Lithium and sodium will also burn with water this way. Magnesium will spontaneously burn with steam, not liquid water.
170755
Specific heat 0.13 J/gK
509622
Potassium hexachloroplatinate, CAS# 16921-30-5, MW 485.99 grams/mole, density 3.50 grams/cm3, has a solubility of 0.77 grams/100 grams H2O at 20°C.  It is insoluble in ethanol.
396644
Like this?\nhttp://www.webelements.com/webelements/elements/media/pics/rainbow.jpg\n\nTo quote the web site,\n"The picture above shows the result of adding different metal salts to a burning reaction mixture of potassium chlorate and sucrose. The red colour originates from strontium sulphate. The orange/yellow colour originates from sodium chloride. The green colour originates from barium chlorate. The blue colour originates from copper (I) chloride. The lilac colour that should be evident from the potassium chlorate is washed out by the other colours, all of which are more intense."\n\nBasically, certain salts will color the flames various colors due to how the electrons are excited (more complicated than that, look into spectroscopy).
738944
Potassium chloride, Chromium oxide, Barium chlorate, Ammonium chloride, Phosphorus trichloride
607593
K2PtCl6 only reacts with Ferric ions of Iron i.e. Fe3+ this is rate determining reaction
940685
Link to a picture of Potassium:\nhttp://en.wikipedia.org/wiki/Image:K%2C19.jpg\n\nPotassium\n \nGeneral \nName, Symbol, Number potassium, K, 19 \nChemical series alkali metals \nGroup, Period, Block 1, 4, s \nAppearance brownish white\n \nAtomic mass 39.0983(1) g/mol \nElectron configuration [Ar] 4s1 \nElectrons per shell 2, 8, 8, 1 \nPhysical properties \nPhase solid \nDensity (near r.t.) 0.89 g·cm−3 \nLiquid density at m.p. 0.828 g·cm−3 \nMelting point 336.53 K\n(63.38 °C, 146.08 °F) \nBoiling point 1032 K\n(759 °C, 1398 °F) \nCritical point ( K, {{{mpa}}} MPa \nCrystal structure cubic body centered \nOxidation states 1\n(strongly basic oxide) \nElectronegativity 0.82 (Pauling scale) \nIonization energies\n(more) 1st: 418.8 kJ·mol−1 \n2nd: 3052 kJ·mol−1 \n3rd: 4420 kJ·mol−1 \nAtomic radius 220 pm \nAtomic radius (calc.) 243 pm \nCovalent radius 196 pm \nVan der Waals radius 275 pm \nMiscellaneous \nMagnetic ordering  ? \nThermal conductivity (300 K) 102.5 W·m−1·K−1 \nThermal expansion (25 °C) 83.3 µm·m−1·K−1 \nSpeed of sound (thin rod) (20 °C) 2000 m/s \nShear modulus 1.3 GPa \nBulk modulus 3.1 GPa \nMohs hardness 0.4 \nBrinell hardness 0.363 MPa \nCAS registry number 7440-09-7 \nSelected isotopes \nMain article: Isotopes of potassium iso NA half-life DM DE (MeV) DP \n39K 93.26% K is stable with 20 neutrons \n40K 0.012% 1.277×109 y β- 1.311 40Ca \nε 1.505 40Ar \nβ+ 1.505 40Ar \n41K 6.73% K is stable with 22 neutrons \n \nReferences \nPotassium (IPA: /pə(ʊ)ˈtasiəm/) is a chemical element. It has the symbol K (Latin: kalium) and atomic number 19. The name "potassium" comes from the word "potash", as potassium was first isolated from potash. Potassium is a soft silvery-white metallic alkali metal that occurs naturally bound to other elements in seawater and many minerals. It oxidizes rapidly in air and is very reactive, especially towards water. In many respects, potassium and sodium are chemically similar, although organisms in general, and animal cells in particular, treat them very differently.\n\nContents [hide]\n1 Notable characteristics \n2 Applications \n3 History \n4 Occurrence \n5 Isotopes \n6 Precautions \n7 Potassium in nutrition and medicine \n8 See also \n9 References \n10 External links \n \n\n\n[edit] Notable characteristics\n \nThe flame testWith a density less than that of water, potassium is the second least dense metal after lithium. It is a soft, low-melting solid that can easily be cut with a knife. Freshly cut potassium is silvery in appearance, but in air it begins to tarnish toward gray visibly and immediately. Potassium must be protected from air for storage to prevent disintegration of the metal from oxide and hydroxide corrosion. Often samples are maintained under an inert medium such as kerosene.\n\nSimilar to other alkali metals, but more so than lithium and sodium, potassium reacts violently with water producing hydrogen. The reaction is sufficiently exothermic that the evolved hydrogen gas ignites.\n\nK + H2O → ½ H2 + KOH \nBecause potassium reacts quickly with even traces of water, and its reaction products are nonvolatile, it is sometimes used alone, or as NaK (an alloy with sodium which is liquid at room temperature) to dry solvents prior to distillation. In this role, it serves as a potent desiccant.\n\nPotassium is an essential element for all living organisms.\n\nPotassium and its compounds emit a violet color in a flame. This fact is the basis of the flame test for the presence of potassium in a sample.\n\nPotassium compounds generally have excellent water solubility, due to the high hydration energy of the K+ ion. Potassium ion is colorless in water.\n\nPotassium may be detected by taste because it triggers all the types of tastebuds, according to concentration. Dilute solutions of potassium ion taste sweet (allowing moderate concentrations in milk and juices), while higher concentrations become increasingly bitter/alkaline,
784949
Additional information is needed.  The mixture could contain one atom of Potassium and the rest Sodium or the reverse.\n\nThe total mass of the sample does not tell you anything about the relative mix.
159817
temperature of fire was 900°F to 1200°F\n\nMost volatiles ignite at temperatures ranging from 1000º - 1400º F.\n\ncombusted in the fourth and final state at temperatures in excess of 935°F.
944951
Flame tests show the color of the metal (the positive ion). The negative ion is usually nitrate (NO3) or sulfate (SO4) which are colorless.
167726
potassium can form many compounds. such as KCN KCl KOH et cetera.
972593
Flame tests are "OK" when you are dealing with a reasonably pure solution.  If there are more than one cation present, such as sodium and potassium, then the resultant color in the flame will not be so determinant.  Also, if you are color blind flame tests suck.
235729
No.\nPotash is potassium ash.i.e. what happens when you burn potassium.\nSoda ash is sodium ash - burnt sodium.\n(both are very reactive)\nThey were known long before the metals even existed (freely)\nThey were used to make glass along with lime (CaCo3)\nAround 1800-1810 Sir Humphrey Davy melted all these mineral ashes and ran an electric current through them with a brand new invention-the battery. In the process he discovered many \nnew elements like K and Na.
777381
Levels of potassium within the cells is much higher than the extra cellular tissues. A burn victim has a lot of tissue damage. When this tissue becomes damaged, the cells have been lysed and spill this additional potassium into the blood stream. The kidneys will pick up on this increase in extra cellular potassium (because that is what they are able to monitor) and will actively pump this potassium out of their body trying to bring them back to homeostasis. Hope this helps. Thanks.
729619
Acetate will burn really well if is divided up so that air can get to it.  It is flammable enough that movie film, when stored in large quantities,like in a movie studio vault, is considered a special fire hazard.
919726
Sodium and Potassium are correct.  They are extremely reactive with water, forming Hydroxides and releasing Hydrogen gas, which is usually ignited from the exothermic heat of the reaction.\n\n2 Na + 2 H2O -> 2 NaOH + H2\n\n2 K + 2H2O -> 2 KOH + H2
874059
I think that isolating potassium is the wrong approach.  Potassium metal reacts with atmospheric water to form KOH and hydrogen gas.  If you accidentally get water on the metal the reaction is so vigourous that the metal will catch fire, which will be dangerous.  \n\nTry a different approach.  Dissolve KCl in water and add a molar equivalence of Silver iodide, AgI, also dissolved in water..  AgCl is nearly insoluble in water (~0.9 mg/L at 10C)  and will precipitate out, leaving KI in solution.  Filter out the AgCl and evaporate the water, leaving solid KI.  \n\nThe two biggest problems starting with KNO3 are:  It will be nearly impossible to salt out the nitrate because of its high solubility in salt form, and two, many nitrate salts, particularlyof metals, are highly explosive and dangerous.  KCl is cheap and plentiful, so why not just buy some?