2KNO3 (s) ==heat==> 2KNO2(s) + O2(g)
potassium nitrate decomposes to potassium nitrite and oxygen.
NB Note the spelling for the product.
the balanced equation would be 2kno3 > 2kno2 +o2
2KBr+= 2k + Br2
2KOH + Ba(NO3)2 -----> 2KNO3 + Ba(OH)2
Silver nitrate + Potassium iodide ----> Silver iodide + Potassium nitrate AgNO3 + KI ----> AgI + KNO3
Potassium iodide + silver nitrate --> Silver iodide and potassium nitrate The chemical equation is: K+I- (aq) + Ag+[NO3]- (aq) --> AgI (s) + K+[NO3]- (aq)
Do you want that for Monopotassium phosphate, dipotassium phosphate, or tripotassium phosphate? --------------------------------- To clarify for the previous answerer, ionic compounds inherently don't use the mono-, di-, or tri- system used for molecular compounds. Instead, when a cation and an anion is supplied, the ionic compound assumes the number of cations and anions that will generate a neutral ionic compound. In this case, since K is 1+ and PO4 is 3-, the compound potassium phosphate always refers to K3PO4. Therefore: 3AgNO3 + K3PO4 -> 3KNO3 + Ag3PO4
Strontium Nitrate: Sr(NO3)2Potassium Phosphate: K3PO4
Potassium nitrate is too stable and so is silver for these two species to react. There is thus no balanced equation.
It is impossible to balance that equation.
The balanced equation is 2 KI + Pb(NO3)2 -> 2 KNO3 + PbI2.
Kn2 heat equal kn2+o2
Pb(NO3)2 + 2KCl ---> PbCl2 + 2KNO3
the equation for the decomposition of lead ii nitrate by heating is: 2Pb(NO3)2 - - - ->2PbO + 4NO2 + O2
Your balanced chemical equation for this double replacement reaction would be: Cu(NO3)2 + 2KOH ----> Cu(OH)2 + 2KNO3 Therefore, you would end up with copper II hydroxide and potassium nitrate.
2KOH + Ba(NO3)2 -----> 2KNO3 + Ba(OH)2
No reaction
Silver nitrate + Potassium iodide ----> Silver iodide + Potassium nitrate AgNO3 + KI ----> AgI + KNO3
Silver nitrate + Potassium iodide ----> Silver iodide + Potassium nitrate AgNO3 + KI ----> AgI + KNO3
Any chemical reaction, only the dissolution of potassium nitrate in water.