Question

What is formed by reacting dry KOH with ozone? (a) \(\mathrm{K}_{2} \mathrm{O}\) (b) \(\mathrm{KO}_{2}\) (c) \(\mathrm{K}_{2} \mathrm{O}_{3}\) (d) none of these

Short answer

Dry KOH reacts with ozone to form  KO_2 (option b).

Step-by-step solution

Recognizing Reactants and Reaction Type

We begin by identifying the reactants: potassium hydroxide ( KOH) and ozone ( O_3). Since the reaction involves KOH in a dry state, it will lead to the formation of specific potassium oxides or peroxides when reacting with ozone, a strong oxidizing agent.

Analyzing Reaction Possibilities

Dry KOH typically reacts with ozone to form potassium superoxide (KO₂). In this context, the superoxide formation is more favorable due to the oxidizing nature of ozone, which tends to form compounds with higher oxidation states for the metal involved.

Writing the Reaction Equation

The balanced chemical equation for the reaction of dry KOH with ozone is: \[ ext{2 KOH + O}_3 ightarrow ext{2 KO}_2 ext{+ H}_2 ext{O} \]. This reflects the production of potassium superoxide and water as products.

Comparing Options with Reaction Product

We compare the products from the reaction (KO 2) with the provided options: - (a)  K_2O is incorrect because it forms under different conditions. - (b)  KO_2 is correct as it matches the outcome of forming a superoxide. - (c)  K_2O_3 doesn't chemically form under this reaction. - (d) 'none of these' is incorrect because KO 2 is indeed formed.

Key concepts

Chemical Reactions

Understanding chemical reactions is crucial when predicting the outcome of mixing different substances. Each reaction involves reactants and products: the reactants are the starting substances, and the products are the new substances formed. In the specific case of potassium hydroxide (KOH) reacting with ozone (O₃), we have a transformation resulting in new chemical compounds.

Identifying the nature of the reactants helps predict the type of reaction. KOH, a strong base, reacts with ozone, a potent oxidizer. This kind of interaction typically results in a specific type of oxidative reaction. In such a scenario, recognizing the conditions — here, KOH being dry — is important. These conditions lead to the formation of particular products, guiding us to understand why specific chemical reactions happen.

Oxidizing Agents

Oxidizing agents are substances that facilitate the oxidation of other substances by accepting electrons during a chemical reaction. Ozone (O₃) is a notable example of a strong oxidizing agent.

Ozone's role in chemical reactions is to change the oxidation state of the elements it interacts with. When ozone reacts with potassium hydroxide (KOH), it tends to form compounds where potassium is at higher oxidation states. This process is indicative of ozone's powerful oxidizing capacity. Thus, in the reaction with KOH, ozone efficiently promotes the formation of potassium superoxide (KO₂), rather than other products.

In general, understanding the strength and purpose of oxidizing agents like ozone allows chemists to predict the products of reactions efficiently. This is particularly valuable in synthetic chemistry, where the goal is often to produce specific outcomes from carefully chosen reactants.

Superoxide Formation

Superoxide formation is a fascinating process in chemistry, particularly when it involves reactive elements like potassium and strong oxidizing agents such as ozone. The superoxide ion (O₂⁻) is formed when oxygen receives an extra electron, leading to a state where it can participate in further chemical reactions.

In the context of forming potassium superoxide (KO₂), this process begins with the presence of dry KOH reacting with ozone. Ozone, being an effective oxidizer, not only facilitates the oxygen gaining an additional electron but also stabilizes the resulting potassium superoxide compound.

The chemical equation governing this reaction, 2 KOH + O₃ → 2 KO₂ + H₂O, beautifully illustrates such transformations. Potassium superoxide has unique properties and applications, including its role in removing carbon dioxide in closed environments, making its formation from such reactions highly valuable in both academic and practical chemical processes.