MAtch ListI with List II

Choose the correct options from the options given below:

A-II, B-IV, C-I, D-III

The correct answer is (4) A-II, B-IV, C-I, D-III.

Elementary Reactions

An elementary reaction is a chemical reaction that occurs in a single step. Elementary reactions have no intermediate steps and do not require energy of activation. This means that the reactants can collide and form products without any additional energy input.

For example, the reaction between hydrogen and bromine to form hydrogen bromide is an elementary reaction.

\(H_2 + Br_2 → 2HBr\)

This reaction occurs in a single step and does not require energy of activation. The reactants collide and form products directly.

Complex Reactions

A complex reaction is a chemical reaction that occurs in multiple steps. Complex reactions have intermediate steps and require energy of activation. This means that the reactants must first absorb energy in order to collide and form products.

For example, the reaction between methane and oxygen to form carbon dioxide and water is a complex reaction.

\(CH_4 + 2O_2 → CO_2 + 2H_2O\)

This reaction occurs in multiple steps and requires energy of activation. The reactants must first absorb energy from the environment in order to collide and form products.

Free Radical Combination

A free radical combination is a type of reaction in which two free radicals combine to form a product. Free radicals are atoms or molecules that have an unpaired electron.

For example, the reaction between two chlorine atoms to form chlorine gas is a free radical combination reaction.

\(\overset{•}{Cl} + \overset{•}{Cl} → Cl_2\)

This reaction is a fast reaction because the free radicals are already in a high energy state. The unpaired electrons on the free radicals make them very reactive and likely to collide and form a product.

Slow Reaction

A slow reaction is a chemical reaction that proceeds at a slow rate. Slow reactions are often characterized by a high energy of activation. This means that the reactants must first absorb energy in order to collide and form products.

For example, the reaction between iron and sulfur to form iron(II) sulfide is a slow reaction.

\(Fe + S → FeS\)

This reaction is a slow reaction because the reactants must first absorb energy from the environment in order to collide and form products.