Question:

Find the products formed if chlorine reacts with the cold and dilute sodium hydroxide solution. 
 

Updated On: Dec 8, 2023
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Solution and Explanation

When chlorine reacts with cold and dilute sodium hydroxide (\(NaOH\)) solution, the following products are formed: 

Sodium Hypochlorite (NaOCl): Chlorine (\(Cl_2\)) reacts with sodium hydroxide (\(NaOH\)) to produce sodium hypochlorite (\(NaOCl\)) as one of the primary products. The balanced chemical equation for this reaction is:
\(Cl_2 + 2NaOH → NaOCl + NaCl + H_2O \)

Sodium Chloride (NaCl): In addition to sodium hypochlorite, sodium chloride (\(NaCl\)) is also formed as a product. The balanced chemical equation shows the formation of sodium chloride:
\(Cl_2 + 2NaOH → NaOCl + NaCl + H_2O \)

Water (H2O): Water is produced as a byproduct of the reaction. The balanced chemical equation includes water as one of the products:
\(Cl_2 + 2NaOH → NaOCl + NaCl + H_2O\)

So, when chlorine reacts with a cold and dilute sodium hydroxide solution, the products formed are sodium hypochlorite (\(NaOCl\)), sodium chloride (\(NaCl\)), and water (\(H_2O\)). 
 

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Concepts Used:

Law of Chemical Equilibrium

Law of Chemical Equilibrium states that at a constant temperature, the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants each raised to a power equal to the corresponding stoichiometric coefficients as represented by the balanced chemical equation.

Let us consider a general reversible reaction;

A+B ↔ C+D

After some time, there is a reduction in reactants A and B and an accumulation of the products C and D. As a result, the rate of the forward reaction decreases and that of backward reaction increases. 

Eventually, the two reactions occur at the same rate and a state of equilibrium is attained. 

By applying the Law of Mass Action;

The rate of forward reaction;

Rf = Kf [A]a [B]b

The rate of backward reaction;

Rb = Kb [C]c [D]d

Where,

[A], [B], [C] and [D] are the concentrations of A, B, C and D at equilibrium respectively.

a, b, c, and d are the stoichiometric coefficients of A, B, C and D respectively.

Kf and Kb­ are the rate constants of forward and backward reactions.

However, at equilibrium,

Rate of forward reaction = Rate of backward reaction.

Kc is called the equilibrium constant expressed in terms of molar concentrations.

The above equation is known as the equation of Law of Chemical Equilibrium.