what will happen to potassium chlorate when it undergoes heat?
828284
The first thing that happens is that it melts.  If you continue heating the molten salt, you will see bubbles appearing.  These are bubbles of oxygen:\n2 KClO3(l)   --->   3 O2(g)   +   2 KCl(l)\nThe main product left behind is potassium chloride, but I believe that you also get some potassium perchlorate (tetraoxochlorate(VII)), produced by disproportionation:\n4 KClO3(l)   --->   3 KClO4(l)   +   KCl(l)\n\nIt wouldn't surprise me if the reaction also produced very small amounts of oxides of chlorine, such as chlorine dioxide, ClO2.\n\nAllan Deeds.
50562
adding water to potassium already causes it to explode.  you are correct - the reaction releases hydrogen and forms an oxide of potassium, and the considerably exothermic nature of the reaction generates enough heat to ignite the hydrogen gas.  so, mixing water and potassium solid typically causes a big-time explosion - just like mixing water and sodium.\n\nas for the powdered magnesium in there - i suspect that the explosion would scatter it, and it might ignite - the ignition temperature for magnesium metal is 450 C - so you'd probably end up with white-hot burning magnesium shrapnel flying everywhere!\n\nso, if you're ever thinking about making a nasty bomb, sounds like a good way to do it.
796075
At 10°C, saturated solution of potassium chloride is more concentrated than potassium nitrate. At this temperature, potassium chloride completely dissolves while potassium nitrate would form some precipitates. At 60°C, it would be the same since both would completely dissolve at this temperature.
866705
To solve this question we need to know the specific heat of the resulting KI solution.  To make things easier, we can probably assume that the specific heat of the solution is the same as the specific heat of water (c = 4.184 J/g degree C).\n\nThe energy (Q) released when a given mass, m, cools a given number of degrees C, (delta T), with a known specific heat, c, is:\nQ = mc(delta T)\n\nWe know the mass of the water, we know its specific heat, we know how many degrees its temperature changed, now just plug in and get an answer,\nQ = (60 g)(4.184 J/g degree C)(14 degree C)\nQ = 3514.56 Joules\nQ = 3.51 kJ\n\nBut this amount of heat energy was due to 28.7 grams of KI dissolving, and we want to know the heat given off by 1 mole, so we need to convert 28.7 grams of KI into moles of KI using the molar mass (166 g/mol).\n28.7 g KI / 166 g/mol KI = .173 moles KI\n\nSo if 3.51 kJ of energy was absorbed when .173 moles of KI dissolved, if one mole of KI dissolves, 20.3 kJ would be absorbed....the answer which you were looking for.\n\nBy the way....\nthe "(triangle) H" you are referring to is the change in the enthalpy of the reaction.  The "triangle" is the Greek letter "Delta".  It is more common to see it written out as "delta" or "change in" if one cannot use the actual Greek alphabet in typing, as opposed to "triangle".  Δ
925364
Definitely not water, as those three metals will burn on contact with water (and potassium will explode.) Liquid CO2 might do, as it would cool the burning material extensively, possibly below the ignition point. The sand (SiO2) would be a smothering agent. I'm not sure about the carbon tet.\n\n5 NOV 06, 1522 hrs, GMT.
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
177751
The particles in the dish and salt will expand when heated, or condense when cooled.  In this case the mass after it cooled down should be smaller
968045
A common lab method to produce small amounts of oxygen is to decompose potassium chlorate.  A little manganese oxide will catalyze the reaction.  Just put the KClO3 in a test tube, add a little MnO2 and heat with a burner.  You can collect the O2 by water displacement.\n\n2KClO3  --> 2 KCl + 3O2
572926
FIRST OF ALL WHY THE SODIUM CHLORIDE IS HARM FULL TO HUMAN ??BUT THE ANSWER IS WRONG TEE Na Cl react with aluminum to produce hydrogen and sodium aluminum oxide. and a lot of heat. if the aluminum is in the powder form which will produce lot of heat and H2 which will cause a blast. do it your self proof the H2 with adding a balloon to the reacting bottle and let the balloon fly.
288242
The reaction should be written as follows,\n2 KClO3(s) --> 2 KCl(s) + 3 O2(g) H = -89.4 kJ\n\nYou either did not include the arrow or it is not displaying properly.\n\nPotassium Chlorate decomposes with heat to form Potassium Chloride and Oxygen gas, no where in this reaction is elemental Potassium involved.\n\nThe standard enthalpy of formation of any pure element in its natural state is zero. Oxygen is a diatomic molecule and thus, Oxygen gas (O2) has a enthalpy of formation of 0 kJ in this reaction, no matter how much of it you have, it is still zero.\n\nSince the Potassium Chloride is the only product left that has any non-zero enthalpy of formation, we know that the over all change in enthalpy is equal to the enthalpy of formation of KCl * the number of moles produced.\nIf the over all change in enthalpy is -89.4 kJ and 2 moles of KCl are produced, then the enthapy of formation of the KCl must be 44.7 kJ/mole less than the enthalpy of formation of the Potassium Chlorate.
872856
It will eventually melt at 2572C, and it will boil at 2850C.\n\nHeat does not cause it to react, typically.
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?
955815
In this compound (potassium chlorate),  the net charge is zero. The potassium ion has a charge of +1, and the chlorate ion (ClO3-) has a charge of -1.\nSo, the total negative charge is -1.
828596
It reacts when in contact with any acid material. When combined with an acid, it forms a salt.
127210
Hydrochloric acid will react with metals ABOVE Hyrogen in the activity series of metals to produce Hydrogen gas.\nThe metals will displace Hydrogen from the acid and make a metal salt (which is usually in solution).\n\nSo if we say that [A] is a generic metal above Hydrogen in the activity series that has a normal oxidation state of +1, then the reaction would be as follows,\n[A] (s) + HCl (aq) --> H2 (g) + [A]Cl (aq)
141648
It is formed by heat pressure
133194
This usually happens in solution, the Chlorine is a chloride ion.\n\nAgNO3(aq) + Cl-(aq) --> AgCl(s) + NO3-(aq)