Hydrogen
LIST-I contains compounds and LIST-II contains reactions
| List-I | List-II |
|---|---|
| (I) $\mathrm{H}_{2} \mathrm{O}_{2}$ |
(P) $\mathrm{Mg}\left(\mathrm{HCO}_{3}\right)_{2}+\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow$ |
| (II) $\mathrm{Mg}(\mathrm{OH})_{2}$ |
(Q) $\mathrm{BaO}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow$ |
| (III) $\mathrm{BaCl}_{2}$ |
(R) $\mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{MgCl}_{2} \rightarrow$ |
| (IV) $\mathrm{CaCO}_{3}$ |
(S) $\mathrm{BaO}_{2}+\mathrm{HCl} \rightarrow$ |
| (T) $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}+\mathrm{Ca}(\mathrm{OH})_{2} \rightarrow$ |
Match each compound in LIST-I with its formation reaction(s) in LIST-II, and choose the correct option
Explanation:
Hydrogen peroxide (H2O2) can act as both an oxidizing agent and a reducing agent, depending on the reactants and the conditions of the reaction. Let's illustrate both properties using chemical equations involving first row transition metal ions.
Hydrogen peroxide as an oxidizing agent:
In an alkaline solution, hydrogen peroxide can oxidize manganese(II) ions (Mn2+) to manganese dioxide (MnO2). The balanced chemical equation for this reaction is:
$2\text{Mn}^{2+} + \text{H}_2\text{O}_2 + 4\text{OH}^- \rightarrow 2\text{MnO}_2 + 4\text{H}_2\text{O}$
In this reaction, H2O2 is reduced to water (H2O), while Mn2+ is oxidized to MnO2.
Hydrogen peroxide as a reducing agent:
Conversely, in an alkaline solution, hydrogen peroxide can reduce chromium(VI) ions (CrO42-) to chromium(III) ions (Cr3+). The balanced chemical equation for this reaction is:
$2\text{CrO}_4^{2-} + 3\text{H}_2\text{O}_2 + 2\text{OH}^- \rightarrow 2\text{Cr}^{3+} + 3\text{O}_2 + 5\text{H}_2\text{O}$
In this reaction, H2O2 is oxidized to oxygen (O2), while CrO42- is reduced to Cr3+.
Through these equations, it is clear that hydrogen peroxide can exhibit both oxidizing and reducing properties in alkaline solutions, depending on the nature of the transition metal ion it interacts with. These dual roles make H2O2 a versatile reagent in various chemical processes.
Hydrogen peroxide acts as an oxidising as well as a reducing agent.
Hydrogen peroxide is a better oxidising agent than water.
Explanation:
The absorption of hydrogen by palladium is commonly known as "occlusion".
Let's dive a bit deeper into this concept:
Palladium has a unique ability to absorb large quantities of hydrogen gas. When hydrogen gas comes into contact with palladium, the hydrogen molecules dissociate into individual hydrogen atoms. These atoms are then absorbed into the interstitial spaces between the palladium atoms in its crystal lattice. This process of hydrogen absorption is not merely a physical process but also involves some chemical interactions at the atomic level.
The term "occlusion" refers to this specific phenomenon. The absorbed hydrogen can be released again upon heating or by applying a vacuum, making palladium-hydrogen systems very useful in various applications, such as hydrogen storage, purification, and sensors.
To understand this interaction more quantitatively, consider the solubility of hydrogen in palladium which can be described by the Sieverts' law:
$ C_H = K \cdot \sqrt{P_H} $
Where:
- $C_H$ is the concentration of hydrogen in palladium.
- $K$ is the Sieverts' constant.
- $P_H$ is the partial pressure of hydrogen gas.
This relationship shows that the concentration of absorbed hydrogen is proportional to the square root of the hydrogen gas pressure.