What type of redox reactions are the following
i) 3Mg(s) + N2(s) → Mg3N2(s)
ii) KClO3(s) → 2KCl(s) + 3O2(s)
iii) Cr2O3(s) + 2Al(s) → Al2O3(s) + 2Cr(s)
Answers
Answer⤵️⤵️
Column I Column II Reason
A 3Mg(s)+N
2
(g)→Mg
3
N
2
(s) (iii) Combination A combination reaction is defined as a chemical reaction in
which two or more substances combine to form a single substance under suitable conditions.
B NaH(s)+H
2
O(l)→NaOH(aq)+H
2
(g) (i) Displacement Displacement reaction is a chemical reaction in which a more reactive element (NaH) displaces a less reactive element (H
2
O→H
2
) from its compound. Both metals and non-metals take part in displacement reactions.
C 3ClO
−
(aq)→2Cl
−
(aq)+ClO
3
−
(aq) (iv) Disproportionation Disproportionation reaction is a redox reaction in which a compound of intermediate oxidation state converts to two different compounds, one of higher and one of lower oxidation states as:
3
Cl
+1
O
−
(aq)→2
Cl
−
−1
(aq)+
Cl
+5
O
3
−
(aq)
D 2KClO
3
(s)→2KCl(s)+3O
2
(g) (ii) Decomposition A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more elements or new compounds.
(A)−(iii), (B)−(i), (C)−(iv), D−(ii)
Answer:
a=iii b=i c=iv d=ii ok follow me pls pls pls