Advertisements
Advertisements
Question
Name three oxoacids of nitrogen. Write the disproportionation reaction of that oxoacid of nitrogen in which nitrogen is in +3 oxidation state.
Advertisements
Solution
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
RELATED QUESTIONS
Write balanced chemical equations for action of potassium permanganate on: Hydrogen
Pb(NO3)2 on heating gives a brown gas which undergoes dimerisation on cooling? Identify the gas
What is the covalence of nitrogen in N2O5?
Bond angle in `PH_(4)^(+)` is higher than that in PH3. Why?
How is nitrogen prepared in the laboratory? Write the chemical equations of the reactions involved.
Explain why NH3 is basic while BiH3 is only feebly basic.
The statement true for \[\ce{N^-_3}\] is ____________.
Nitrogen is relatively inactive element because ____________.
Among the 15th group elements, as we move from nitrogen to bismuth, the pentavalency becomes less pronounced and trivalency becomes more pronounced due to:
Which of the following oxides is neutral?
In which one of the following oxides of nitrogen, one nitrogen atom is not directly linked to oxygen?
Which of the following can be used as anesthesia?
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’.
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.
