CuSO4 - Copper Sulphate
KCIO3 -
NH4OH - Ammonium Hydroxide
K2CO3 - Potassium Carbonate
NA2SO4 - Sodium Sulphate
KC2H3O2 -
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∙ 11y agoKCIO3 is nothing. KClO3 (with a lowercase L) is potassium chlorate.
HCN is an acid; KClO3 is a salt.
69. 00 g of oxygen
To balance the chemical equation KCIO3 → KCI + O2, you need to make sure the number of atoms on both sides is equal. First, balance the potassium atoms by adding a coefficient of 1 in front of KCI. Next, balance the chlorine atoms by adding a coefficient of 1 in front of KCI. Finally, balance the oxygen atoms by adding a coefficient of 3 in front of O2. The balanced equation is KCIO3 → KCI + 3O2.
There is no such thing as KCIO3. That should be a lowercase L, not an I. (all two-letter element symbols use a lowercase for the second letter) That being said, KClO3 is Potassium Chlorate. K = Potassium Cl = Chlorine O = Oxygen 3 = number of Oxygen atoms in the molecule
No, potassium chlorate (KClO3) is a solid compound at room temperature and pressure. It can be decomposed to produce oxygen gas when heated.
K=39.100 Cl=35.457 O3=48.000 total=122.557 %K = 39.1x100/122.557 %Cl = 35.457x100/122.557 %O = 48.0x100/122.557
KCIO3-MNO2 cannot comes in contact with the rubber stopper otherwise, or a severe explosion may result.
There is no such thing as KCIO3. That should be a lowercase L, not an I. (all two-letter element symbols use a lowercase for the second letter) That being said, KClO3 is Potassium Chlorate. K = Potassium Cl = Chlorine O = Oxygen 3 = number of Oxygen atoms in the molecule
Balanced equation: 2KClO3(s) → 2KCl(s) + 3O2(g) Unbalanced reaction: KClO3(s) → KCl(s) + O2(g)
The compound KIO3 is potassium iodate, which is a salt of potassium and iodate ions. It is commonly used as a source of iodine for dietary supplementation and in some analytical chemistry applications.
The mixture of KClO3 and MnO2 can react vigorously and release oxygen gas under certain conditions. The oxygen gas produced can build up pressure inside the container, leading to a potential explosion. Rubber stoppers are not gas-impermeable and may not be able to contain the pressure, hence it is safer to use a stopper that is more appropriate for such reactions.