Question

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:

a. $2{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)\stackrel{∆}{\to }4\mathrm{Al}\left(\mathrm{s}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)$

b. ${\mathrm{Br}}_2\left(\mathrm{l}\right)+{\mathrm{BaI}}_2\left(\mathrm{s}\right)\to {\mathrm{BaBr}}_2\left(\mathrm{s}\right)+{\mathrm{I}}_2\left(\mathrm{s}\right)$

c. $2{\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{∆}{\to }4{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

d. ${\mathrm{BaCl}}_2\left(\mathrm{aq}\right)+{\mathrm{K}}_2{\mathrm{CO}}_3\left(\mathrm{aq}\right)\to {\mathrm{BaCO}}_3\left(\mathrm{s}\right)+\mathrm{KCl}\left(\mathrm{aq}\right)$

e.$\mathrm{Pb}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{PbO}}_2\left(\mathrm{s}\right)$

Short answer

(a) The reaction is decomposition reaction.

(b) The reaction is displacement reaction.

(c) The reaction is combustion reaction.

(d) The reaction is double displacement reaction.

(e) The reaction is combination reaction.

Step-by-step solution

Part (a) Step 1: Given Information

We are given the equation, and we must determine whether it is a combination, decomposition, single replacement, double replacement, or combustion process.

Part (a) Step 2: Explanation

Now, the given equation is $2{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)\to \mathrm{Al}\left(\mathrm{s}\right)+{30}_2\left(\mathrm{g}\right)$

which states the the reactant is breaking down into two products and the reaction in which reactants break down into two or more than two products are called decomposition reaction.

Hence, the given reaction is decomposition reaction.

Part (b) Step 1: Given Information

We are given the equation, and we must determine whether it is a combination, decomposition, single replacement, double replacement, or combustion process.

Part (b) Step 2: Explanation

Now, the given equation is ${\mathrm{Br}}_2\left(\mathrm{l}\right)+{\mathrm{Bal}}_2\left(\mathrm{s}\right)\to {\mathrm{BaBr}}_2\left(\mathrm{s}\right)+{\mathrm{I}}_2\left(\mathrm{s}\right)$

which states that Br is displacing I from its compound and the reaction in which a elements displaces an another element from its compound is called displacement reaction.

Hence, the given reaction is displacement reaction.

Part (c) Step 1: Given Information

We are given the equation, and we must determine whether it is a combination, decomposition, single replacement, double replacement, or combustion process.

Part (c) Step 2: Explanation

Now, the given equation is $2{\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)+{50}_2\left(\mathrm{g}\right)->4{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

which states that ${\mathrm{C}}_2{\mathrm{H}}_2$is oxidized by oxygen and release carbon dioxide and water and the reaction in which reactant in the presence of oxygen release carbon dioxide and water is called combustion reaction.

Hence, the given reaction is combustion reaction.

Part (d) Step 1: Given Information

We are given the equation, and we must determine whether it is a combination, decomposition, single replacement, double replacement, or combustion process.

Part (d) Step 2: Explanation

Now, the given equation is ${\mathrm{BaCl}}_2\left(\mathrm{aq}\right)+{\mathrm{K}}_2{\mathrm{CO}}_3\left(\mathrm{aq}\right)\to {\mathrm{BaCO}}_3\left(\mathrm{s}\right)+2\mathrm{KCl}\left(\mathrm{aq}\right)$

which states that Cl and ${\mathrm{CO}}_3$are displacing each other from their compounds and the reaction in which a elements displaces each other from its compound is called double displacement reaction.

Hence, the given reaction is double displacement reaction.

Part (e) Step 1: Given Information

We are given the equation, and we must determine whether it is a combination, decomposition, single replacement, double replacement, or combustion process.

Part (e) Step 2: Explanation

Now, the given equation is $\mathrm{Pb}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{PbO}}_2\left(\mathrm{s}\right)$

which states the the reactant combines together to form products and the reaction in which reactants combine together to give products are called combination reaction.

Hence, the given reaction is combination reaction.