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 :

(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)

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)

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)

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)

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.