Question

Identify the following redox reactions by type. Check all that apply. (a) Fe + H2SO4 → FeSO4 + H2 combination decomposition displacement disproportionation (b) S + 3F2 → SF6 combination decomposition displacement disproportionation (c) 2CuCl → Cu + CuCl2 combination decomposition displacement disproportionation (d) 2Ag + PtCl2 → 2AgCl + Pt combination decomposition displacement disproportionation

Answer 1

Answer :

(a) displacement reaction

(b) combination reaction

(c) disproportionation reaction

(d) displacement reaction

Explanation :

(a) The given balanced chemical reaction is,

$Fe+H_2SO_4\rightarrow FeSO_4+H_2$

This reaction is a single replacement reaction or displacement in which the the more reactive element (Fe) replace the less reactive element (H).

(b) The given balanced chemical reaction is,

$S+3F_2\rightarrow SF_6$

This reaction is a combination reaction in which the two reactants molecule combine to form a large molecule or single product.

(c) The given balanced chemical reaction is,

$2CuCl_2\rightarrow Cu+CuCl_2$

This reaction is a disproportionation reaction in which the chemical species gets oxidized and reduced simultaneously.  It is also considered as a redox reaction.

(d) The given balanced chemical reaction is,

$2Ag+PtCl_2\rightarrow 2AgCl+Pt$

This reaction is a single replacement reaction or displacement in which the the more reactive element (Ag) replace the less reactive element (Pt).