Q1 Na2CO3 +Fe2O3→A +CO2
Q2 AgNO3→heat W+X+O2
X+ H2O→HNO2+HNO3
W+HNO3→Y+NO+H2O
Y+Na2S2O3(excess)→Z+NaNO3
13AgNO3 ---(Heat)--> Ag + NO2 + O2
(Always remember tht Ag/Hg being smwhat less reactive wan't 2 pptate. out if they get a chance i.e. heated/decomposition)
NO2 disproportionates in water... NO2 + H2O ----> HONO + HNO3
In the 3rd reac.n, "N" is bein' reduced ,so Ag shud get oxidised..
Further AgNO3 reacts with Hypo 2 gve a white ppt. of Ag2S2O3 (simply ion exchange b/w Ag & Na) ...which on standing turns blacks due to decomposition into Ag2S & SO3
132 Possibilties of "N" reduction frm NO3- - NO or NO2...
But, Even if NO were 2b released, it wud have used up the O2 to get oxidised a little to NO2...as is the case when v test fr Nitrites...
11@ eure,
It should be Na FeO2 (Sodium ferrite)
This reacn is a part of Lowing process , used in the manufacture of NaOH
PLEASE CHECK AGAIN
24oops yes..u r rite...i checked ans to wrong ques...sorry for trouble...
btw can u explain the answer a bit more ???
11Fe2O3 is largely basic. The ignited form is difficult to dissolve in acids. However the freshly precipitated hydrous form dissolves in acids, giving the very pale violet [Fe (H2O) 6 ] 3+ ion, and in conc NaOH , forming [Fe (OH) 6] 3 - . This shows that the oxide is slightly amphoteric. Fusion with LiOH, NaO or Na2 CO3 gives Li FeO2 or NaFeO2.
Fe2O3 + Na2CO3 → 2 NaFeO2 + CO2
At one time, this was used in the obselete Lowig Process for manufacturing Caustic Soda.
Fe2O3 + Na2CO3 → 2 NaFeO2 + CO2
2 NaFeO2 +H2O → 2 NaOH + Fe 2O3
