Question

Indicate what type, or types, of reaction each of the following represents: (a) H2 O(g) + C(s) ⟶ CO(g) + H2 (g) (b) 2KClO3 (s) ⟶ 2KCl(s) + 3O2 (g) (c) Al(OH)3 (aq) + 3HCl(aq) ⟶ AlCl3 (aq) + 3H2 O(l) (d) Pb(NO3 )2 (aq) + H2SO4 (aq) ⟶ PbSO4 (s) + 2HNO3 (aq)

Answer 1

Answer :

(a) This reaction is a type of single displacement reaction.

(b) This reaction is a type of decomposition reaction.

(c) This reaction is a type of double displacement reaction.

(d) This reaction is a type of double displacement reaction.

Explanation :

(a) $H_2O(g)+C(s)\rightarrow CO(g)+H_2(g)$

This reaction is a type of single displacement reaction. It is a type of reaction in which the more reactive metal displaces the least reactive metal from its solution.

(b) $2KClO_3(s)\rightarrow 2KCl(s)+3O_2(g)$

This reaction is a type of decomposition reaction. It is a type of reaction in which a single larger compound decomposes to give two or more smaller molecules as a product.

(c) $Al(OH)_3(aq)+3HCl(aq)\rightarrow AlCl_3(aq)+3H_2O(l)$

This reaction is a type of double displacement reaction. It is a type of reaction in which the cation and the anion of the two reactant exchange their places to give two another compounds as a product.

(d) $Pb(NO_3)_2(aq)+H_2SO_4(aq)\rightarrow PbSO_4(s)+2HNO_3(aq)$

This reaction is a type of double displacement reaction. It is a type of reaction in which the cation and the anion of the two reactant exchange their places to give two another compounds as a product.