Question

\(\mathrm{II}_{2} \mathrm{O}_{2}\) does not liberate oxygen when it reacts with (1) \(\mathrm{NaOCl}\) (2) \(\mathrm{MnO}_{2} / \mathrm{H}^{+}\) (3) \(\mathrm{Cl}_{2}\) (4) \(\mathrm{C}_{6} \mathrm{H}_{6}\)

Short answer

(3) \( \mathrm{Cl}_{2} \)

Step-by-step solution

- Understand the Reactants and Products

To determine which option does not liberate oxygen when reacting with \( \mathrm{II}_{2} \mathrm{O}_{2} \), first recall the general behavior of \( \mathrm{II}_{2} \mathrm{O}_{2} \). This compound is an oxidizing agent, and therefore, reacts with materials that can be oxidized, potentially producing oxygen gas (\( O_2 \)).

- Analyze Each Reaction

Let's go through each option and check whether they typically produce oxygen gas when reacting with an oxidizing agent like \( \mathrm{II}_{2} \mathrm{O}_{2} \).

- Sodium Hypochlorite Reaction

Consider \( \mathrm{NaOCl} \) (sodium hypochlorite). This will react with \( \mathrm{II}_{2} \mathrm{O}_{2} \) to produce \( Cl_{2} \) and \( O_2 \). \(\mathrm{II}_{2} \mathrm{O}_{2} + 2 \mathrm{NaOCl} \rightarrow \mathrm{Cl}_{2} + \mathrm{O}_{2} + 2 \mathrm{Na}^{+}\)

- Manganese Dioxide and Acid Reaction

Consider \2.\( \mathrm{MnO}_{2} / \mathrm{H}^{+} \) (manganese dioxide with acid). When these react, manganese dioxide acts as an oxidizing agent and typically liberates oxygen: \(2 \mathrm{II}_{2} \mathrm{O}_{2} + 2 \mathrm{MnO}_{2} \rightarrow 2\mathrm{II}^{+}, \mathrm{O_2}, \mathrm{MnO_4^-} \)

- Chlorine Reaction

Consider \( \mathrm{Cl}_{2} \) (chlorine). Chlorine is a strong oxidizing agent and does not typically cause the liberation of oxygen when reacting with another oxidizing agent like \( \mathrm{II}_{2} \mathrm{O}_{2} \).

- Benzene Reaction

Consider \( \mathrm{C}_{6} \mathrm{H}_{6} \) (benzene). Benzene is an organic compound that can react with strong oxidizers. The interaction between benzene and \( \mathrm{II}_{2} \mathrm{O}_{2} \) will generally not result in the release of oxygen.

Key concepts

Oxidation Reactions

Oxidation reactions play a crucial role in chemistry. In these reactions, a substance loses electrons, typically making it more positive.
The substance that gains those electrons and promotes oxidation is known as the oxidizing agent.
In our exercise, \( \mathrm{II}_2 \mathrm{O}_2 \) acts as an oxidizing agent.
It drives reactions by accepting electrons from other substances. For example, when \( \mathrm{II}_2 \mathrm{O}_2 \) reacts with sodium hypochlorite \( ( \mathrm{NaOCl}) \), it produces chlorine \( ( \mathrm{Cl}_2) \) and oxygen gas \( (O_2) \).
This characteristic of oxidizing agents is vital in numerous chemical processes, from industrial manufacturing to metabolic pathways in living organisms.

Chemical Reactions

Chemical reactions are processes where substances (reactants) are transformed into new substances (products).
In our specific case, the reactions of \( \mathrm{II}_2 \mathrm{O}_2 \) with other substances were analyzed.
The nature of these reactions depends on whether oxygen is liberated during the process.
For instance, manganese dioxide with acid (\( \mathrm{MnO}_2 / \mathrm{H}^+ \)) results in the production of oxygen through an oxidation process.
However, the reaction involving chlorine \( \mathrm{Cl}_2 \) does not produce oxygen because chlorine itself is a strong oxidizing agent.
Similarly, benzene \( \mathrm{C}_6\mathrm{H}_6 \) when reacting with \( \mathrm{II}_2 \mathrm{O}_2 \), does not lead to oxygen liberation.
Understanding these characteristics helps in predicting the outcomes of various chemical reactions.

Oxygen Liberation

Oxygen liberation is a key indicator in oxidation reactions.
When an oxidizing agent reacts, it often releases oxygen as part of the chemical process.
In our exercise, identifying which reactions liberate oxygen is important.
Sodium hypochlorite \( \mathrm{NaOCl} \) and manganese dioxide with acid \( \mathrm{MnO}_2 / \mathrm{H}^+ \) both result in oxygen liberation when reacting with \( \mathrm{II}_2 \mathrm{O}_2 \).
This is evidenced by the appearance of \( O_2 \) gas in the chemical equations.
Conversely, chlorine \( \mathrm{Cl}_2 \) and benzene \( \mathrm{C}_6\mathrm{H}_6 \) do not cause oxygen to be released when they react with the oxidizing agent.
Understanding which conditions lead to oxygen liberation is essential for controlling and utilizing these reactions in various scientific and industrial applications.