Question

Which of the following represents the chemical equation involved in the preparation of \(\mathrm{H}_{2} \mathrm{O}_{2}\) from barium peroxide? (a) \(\mathrm{BaO}_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{BaSO}_{4}+\mathrm{H}_{2} \mathrm{O}_{2}+8 \mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{CH}_{3} \mathrm{CHOHCH}_{3}+\mathrm{O}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{COCH}_{3}+\mathrm{H}_{2} \mathrm{O}_{2}\) (c) \(\mathrm{BaO}_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{BaCO}_{3}+\mathrm{H}_{2} \mathrm{O}_{2}\) (d) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}+3 \mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow 3 \mathrm{BaSO}_{4}+2 \mathrm{H}_{3} \mathrm{PO}_{4}\)

Short answer

(a) \(\mathrm{BaO}_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}+\mathrm{H}_{2}\mathrm{SO}_{4} \rightarrow \mathrm{BaSO}_{4}+\mathrm{H}_{2} \mathrm{O}_{2}+8\mathrm{H}_{2} \mathrm{O}\) is the correct equation for the preparation of \(\mathrm{H}_{2} \mathrm{O}_{2}\) from Barium Peroxide.

Step-by-step solution

Understanding the Question

The task is to identify the chemical equation that shows the preparation of Hydrogen Peroxide (\(\mathrm{H}_{2} \mathrm{O}_{2}\)) from Barium Peroxide (\(\mathrm{BaO}_{2}\)). We need to look for an equation where these two substances interact and lead to the formation of Hydrogen Peroxide.

Examining Option (a)

This option shows the reaction between hydrated Barium Peroxide (\(\mathrm{BaO}_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\)) and Sulfuric Acid (\(\mathrm{H}_{2}\mathrm{SO}_{4}\)). The products are Barium Sulfate (\(\mathrm{BaSO}_{4}\)), Hydrogen Peroxide (\(\mathrm{H}_{2} \mathrm{O}_{2}\)), and water. This represents a typical reaction used to prepare Hydrogen Peroxide in laboratories.

Checking Option (b)

Option (b) represents the oxidation of isopropanol to acetone with the release of Hydrogen Peroxide. However, this is not a preparation of \(\mathrm{H}_{2} \mathrm{O}_{2}\) from Barium Peroxide.

Looking at Option (c)

Option (c) shows a reaction between Barium Peroxide, Carbon Dioxide, and water to form Barium Carbonate and Hydrogen Peroxide. While this reaction involves producing Hydrogen Peroxide, it is not a commonly used method for its preparation.

Analyzing Option (d)

Option (d) shows the reaction between Barium Phosphate and Sulfuric Acid to produce Barium Sulfate and Phosphoric Acid. This reaction does not produce Hydrogen Peroxide and is therefore not the correct answer.

Conclusion

After examining all options, option (a) is the correct chemical equation that represents the preparation of Hydrogen Peroxide from Barium Peroxide. It is a typical laboratory synthesis for \(\mathrm{H}_{2} \mathrm{O}_{2}\).

Key concepts

Barium Peroxide Reaction

Barium peroxide (\textbf{BaO\(_2\)}) is a white crystalline compound commonly used in the preparation of hydrogen peroxide (\textbf{H\(_2\)O\(_2\)}) due to its rich oxygen content. When barium peroxide reacts with sulfuric acid (\textbf{H\(_2\)SO\(_4\)}), hydrogen peroxide is produced along with barium sulfate (\textbf{BaSO\(_4\)}) as a by-product, which is insoluble and hence, easily separated through filtration.

The chemical equation representing this reaction is:
\[\begin{equation} \text{BaO}_2 \times 8\text{H}_2\text{O} + \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + \text{H}_2\text{O}_2 + 8\text{H}_2\text{O} \tag{a}\text{.} \[\] \text{\textbf{(Option a is the correct answer.)}} \[\] \text{The hydrated form of barium peroxide is used here, indicated by the} \times 8\text{H}_2\text{O}, \text{which reflects the presence of water molecules associated with the peroxide in its solid state.} \end{equation}\]
Understanding the stoichiometry of this chemical reaction is essential in calculating the expected yield of hydrogen peroxide in a laboratory setup.

Laboratory Synthesis of H2O2

Hydrogen peroxide is a versatile compound widely used in disinfection, bleaching, and as a mild antiseptic. The synthesis of hydrogen peroxide in a laboratory setting often involves the reaction between barium peroxide and sulfuric acid, which is a safe and convenient method.

Firstly, a suspension of barium peroxide is mixed with cold diluted sulfuric acid to prevent the decomposition of hydrogen peroxide. As the reaction proceeds under controlled conditions, the insoluble barium sulfate forms and precipitates out of the solution, leaving behind aqueous hydrogen peroxide. The resulting hydrogen peroxide can then be further purified and concentrated if needed. To enhance the understanding and performance of this synthesis, it is crucial to maintain a low temperature and use a diluted acid; these precautions help to mitigate any side reactions or decomposition of the desired product, hydrogen peroxide.

Chemical Equations in Chemistry

Chemical equations are symbolic representations of chemical reactions, showcasing the reactants and products along with their respective quantities. Writing and balancing chemical equations is a fundamental skill in chemistry that serves as the language through which chemists communicate reaction details.

For instance, the equation for the preparation of hydrogen peroxide from barium peroxide is balanced with respect to both mass and charge, meaning the number of atoms for each element, and the overall charge, are equal on both sides of the equation. Mastery of interpreting chemical equations not only helps in understanding reactions like the synthesis of H\(_2\)O\(_2\), but also in predicting reaction outcomes, calculating theoretical yields, and scaling up reactions for applications across various industries, including pharmaceuticals, environmental science, and materials engineering.