Advertisements
Advertisements
प्रश्न
Name three oxoacids of nitrogen. Write the disproportionation reaction of that oxoacid of nitrogen in which nitrogen is in +3 oxidation state.
Advertisements
उत्तर
The three oxyacids of nitrogen are:
(i) Nitric acid \[\ce{(HNO3)}\]
(ii) Nitrous acid \[\ce{(HNO2)}\]
(iii) Hyponitrous acid \[\ce{(H2N2O2)}\]
+3 oxidation state of nitrogen is observed in \[\ce{HNO2}\]. It undergoes disproportionation
\[\ce{\underset{+3}{3HNO2} -> \underset{+5}{HNO3} + \underset{+2}{2NO} + H2O}\]
+3 oxidation state changes to +5 and +2 oxidation states.
APPEARS IN
संबंधित प्रश्न
Why does NO2 dimerise?
Explain why Mn2+ ion is more stable than Mn3+? (Given : Mn→ Z=25)
Tendency to show –3 oxidation state decrease from Nitrogn (N) to Bismuth (Bi).
Which of the following statements is not correct for nitrogen?
Nitrogen is relatively inactive element because ____________.
Pick out the wrong statement.
Among the 15th group elements, as we move from nitrogen to bismuth, the pentavalency becomes less pronounced and trivalency becomes more pronounced due to:
In which one of the following oxides of nitrogen, one nitrogen atom is not directly linked to oxygen?
Which of the following oxides of nitrogen reacts with FeSO4 to form a dark brown compound?
Which oxide of nitrogen is obtained on heating ammonium nitrate at 250°C?
Which of the following can be used as anesthesia?
A deep brown gas is formed by mixing two colourless gases which are:
Assertion: \[\ce{HNO3}\] makes iron passive.
Reason: \[\ce{HNO3}\] forms a protective layer of ferric nitrate on the surface of iron.
On heating lead (II) nitrate gives a brown gas “A”. The gas “A” on cooling changes to colourless solid “B”. Solid “B” on heating with NO changes to a blue solid ‘C’. Identify ‘A’, ‘B’ and ‘C’ and also write reactions involved and draw the structures of ‘B’ and ‘C’.
HCl is added to following oxides. Which one would give H2O2
Which oxide of nitrogen is obtained on heating ammonium nitrate at 250°C?
Assertion: Nitrogen and oxygen are the main components in the atmosphere but these do not react to form oxides of nitrogen.
Reason: The reaction between nitrogen and oxygen requires high temperature.
