Silver(I) chromate --Δ--> Chromium(III) oxide + Silver + Oxygen
2Ag2CrO4 --Δ--> Cr2O3 + 4Ag + 2.5 O2
Silver(I) chromate = Ag2CrO4
2Ag2O -> 4Ag + O2
Two types: silver (Ag+) and chromate (CrO4-2) And within the formula (Ag2CrO4) there are two silver ions and one chromate ion for a total of three ions.
Ag2CrO4
how many moles are there in 56.0 grams of silver nitrate?
Silver Chromate Ag=Silver CrO4= Chromate(a polyatomic ion)
Silver(I) chromate = Ag2CrO4
Solid AgOH is not known. It may be in solution but when precipitated you get the oxide, Ag2O A likely decompoition wuld be 2AgOH -> Ag2O + H2O
Silver chromate is not soluble in water.
2Ag2O -> 4Ag + O2
The chromate ion (CrO4-2) has yellow colour so all the chromate compounds including silver chromate is yellow in colour.
Two types: silver (Ag+) and chromate (CrO4-2) And within the formula (Ag2CrO4) there are two silver ions and one chromate ion for a total of three ions.
No
Reddish orange
Ag2CrO4
how many moles are there in 56.0 grams of silver nitrate?
Silver chromate has a brown red colour