Question

Classify each chemical equation as a combination/synthesis, decomposition, single replacement , double replacement, or combustion
A. Pb(s) + Hg2SO4 (s) ---> PbSO4(s) +2 Hg(I)
B. NaCI(aq) + AgNO3(aq) --->AgCI(s) +NaNO3(aq)
C. 2H20(I)--->2H2(g) + 02(g)

Answer 1

We classify each of the reaction as follows:

A. Pb(s) + Hg2SO4 (s) ---> PbSO4(s) +2 Hg(I)
Single replacement reaction

B. NaCI(aq) + AgNO3(aq) --->AgCI(s) +NaNO3(aq)
Double replacement reaction

C. 2H20(I)--->2H2(g) + 02(g)
Decomposition reaction

Hope this answers the question. Have a nice day.

Answer 2

Answer: A is single displacement reaction, B is double displacement reaction and C is decomposition reaction.

Explanation:

Synthesis reaction is defined as the reaction where substances combine in their elemental state to form a single compound.

$A+B\rightarrow AB$

Decomposition reaction is defined as the reaction where a single substance breaks down into two or more simpler substances.

$AB\rightarrow A+B$

Single displacement reaction is defined as the reaction where more reactive element displaces a less reactive element from its chemical reaction.

$AB+C\rightarrow CB+A$

Element C is more reactive than element A.

Double displacement reaction is defined as the reaction where exchange of ions takes place.

$AB+CD\rightarrow AD+CB$

Combustion reaction is defined as the reaction where a hydrocarbon reacts with oxygen gas to produce carbon dioxide and water molecule.

$\text{hydrocarbon}+O_2\rightarrow CO_2+H_2O$

For the given options:

Option A:

$Pb(s)+Hg_2SO_4(s)\rightarrow PbSO_4(s)+2Hg(l)$

This is considered as a single displacement reaction because lead is more reactive than mercury.

Option B:

$NaCl(aq.)+ AgNO_3(aq.)\rightarrow AgCl(s)+NaNO_3(aq.)$

This is considered as a double displacement reaction.

Option C:

$2H2O(l)\rightarrow 2H_2(g)+O_2(g)$

This is considered as a decomposition reaction.

Hence, A is single displacement reaction, B is double displacement reaction and C is decomposition reaction.