Peroxide and Superoxide Reactions: Videos & Practice Problems

Peroxides react with water to produce barium hydroxide and hydrogen peroxide, while superoxides yield potassium hydroxide, hydrogen peroxide, and oxygen gas. In acid reactions, peroxides generate hydrogen peroxide instead of water, and superoxides produce both hydrogen peroxide and oxygen. Balancing these reactions involves adjusting coefficients to maintain stoichiometry. Understanding these reactions is crucial for grasping the behavior of peroxides and superoxides in various chemical contexts.

Reaction with Water

When peroxides react with water, they behave similarly to oxides but yield hydrogen peroxide as an additional product. In the case of oxides, the reaction with water typically produces hydroxides, which are basic. However, peroxides introduce a more complex ion, resulting in the formation of both hydroxides and hydrogen peroxide.

For example, when barium peroxide reacts with liquid water, the products are barium hydroxide and hydrogen peroxide. The balanced chemical equation for this reaction can be represented as:

\[ \text{BaO}_2 + 2 \text{H}_2\text{O} \rightarrow \text{Ba(OH)}_2 + \text{H}_2\text{O}_2 \]

In the case of superoxides, the reaction with water produces potassium hydroxide, hydrogen peroxide, and oxygen gas. For instance, when potassium superoxide reacts with water, the balanced equation is:

\[ 2 \text{KO}_2 + 2 \text{H}_2\text{O} \rightarrow 2 \text{KOH} + \text{H}_2\text{O}_2 + \text{O}_2 \]

In summary, while the reactions of peroxides and superoxides with water follow a similar pattern to those of oxides, they yield additional products, specifically hydrogen peroxide and, in the case of superoxides, oxygen gas. Understanding these reactions is crucial for predicting the behavior of these compounds in various chemical contexts.

Peroxide and Superoxide Reactions Example

To complete and balance the chemical equation involving sodium peroxide, we start by identifying the components of sodium peroxide, which consists of sodium ions (Na⁺) and peroxide ions (O₂^2-). When sodium peroxide reacts with water (H₂O), it produces sodium hydroxide (NaOH) and hydrogen peroxide (H₂O₂). The unbalanced reaction can be represented as:

Na₂O₂ + H₂O → NaOH + H₂O₂

To balance this equation, we need to ensure that the number of each type of atom is the same on both sides. By placing a coefficient of 2 in front of NaOH and H₂O₂, we achieve the following balanced equation:

Na₂O₂ + 2 H₂O → 2 NaOH + H₂O₂

Now, let's verify the balance: on the left side, we have 2 sodium (Na), 4 hydrogen (H), and 4 oxygen (O) atoms. On the right side, we also have 2 sodium, 4 hydrogen, and 4 oxygen atoms. Thus, the equation is balanced, confirming that the final balanced equation is:

Na₂O₂ + 2 H₂O → 2 NaOH + H₂O₂

Write a balanced equation for the reaction of rubidium superoxide with water.

• A. 2 RbO₂(s) + 2 H₂O(l) → 2 RbOH(aq) + H₂O₂(aq) + O₂(g)
• B. 4 RbO(s) + 2 H₂O(l) → 4 RbOH(aq) + O₂(g)
• C. 2 RbO₂(s) + 2 H₂O(l) → 2 Rb(OH)₂(aq) + 2 H₂O(aq)
• D. 6 Rb₂O(s) + 4 H₂O(l) → 12 Rb(s) + 4 H₂O₂(aq) + O₂(g)

Answer: (A)

Reaction with Acids

In the context of chemical reactions involving peroxides and superoxides with acids, it is essential to understand the products formed during these interactions. When peroxides react with acids, they yield hydrogen peroxide instead of water. For instance, when sodium peroxide reacts with hydrochloric acid, the reaction can be represented as:

2 Na₂O₂ + 4 HCl → 4 NaCl + 2 H₂O₂

Here, sodium chloride (NaCl) is formed alongside hydrogen peroxide (H₂O₂), highlighting the unique behavior of peroxides in acid reactions.

On the other hand, superoxides, such as potassium superoxide, react with acids to produce both hydrogen peroxide and oxygen gas. For example, the reaction with nitric acid can be expressed as:

2 KO₂ + 4 HNO₃ → 2 KNO₃ + 2 H₂O₂ + O₂

In this case, potassium nitrate (KNO₃) is produced along with hydrogen peroxide and oxygen gas (O₂). The balancing of these reactions is crucial, as indicated by the coefficients used in the equations, ensuring that the number of atoms for each element is conserved on both sides of the reaction.

Overall, understanding these reactions is vital for grasping the behavior of peroxides and superoxides in acidic environments, as they demonstrate distinct pathways and products that differ from typical acid-base reactions.

Peroxide and Superoxide Reactions Example

In the reaction between cesium superoxide and sulfuric acid, the products formed are cesium sulfate, hydrogen peroxide, and oxygen gas. The balanced chemical equation for this reaction can be represented as follows:

When balancing the equation, we start by identifying the reactants and products:

Reactants: Cesium superoxide (CsO₂) and Sulfuric acid (H₂SO₄)

Products: Cesium sulfate (Cs₂SO₄), Hydrogen peroxide (H₂O₂), and Oxygen gas (O₂)

The balanced equation is:

2 CsO₂ + H₂SO₄ → Cs₂SO₄ + H₂O₂ + O₂

In this equation, we ensure that the number of each type of atom is equal on both sides. We have:

• 2 cesium (Cs) atoms on both sides
• 1 sulfate (SO₄) group on both sides
• 2 hydrogen (H) atoms on both sides
• 4 oxygen (O) atoms on the reactant side (2 from CsO₂ and 2 from H₂SO₄) and 4 oxygen atoms on the product side (2 from H₂O₂ and 2 from O₂)

This balanced equation illustrates the stoichiometry of the reaction, ensuring that mass is conserved throughout the process.

Write a balanced equation for the reaction of barium peroxide with hydrochloric acid.

• A. BaO(s) + 2 HCl(aq) → BaCl₂(aq) + H₂O(aq)
• B. 2 Ba₂O(s) + 2 HCl(aq) → 2 Ba₂Cl(aq) + H₂O₂(aq)
• C. Ba₂O₂(s) + 2 HCl(aq) → 2 BaCl(aq) + H₂O₂(aq)
• D. BaO₂(s) + 2 HCl(aq) → BaCl₂(aq) + H₂O₂(aq)

Answer: (D)

Here’s what students ask on this topic:

What are the products of the reaction between barium peroxide and water?

When barium peroxide (BaO₂) reacts with water (H₂O), it produces barium hydroxide (Ba(OH)₂) and hydrogen peroxide (H₂O₂). The balanced chemical equation for this reaction is:

${\mathrm{BaO}}_2+2H_2{O}_1\to {\mathrm{Ba}}_1{\mathrm{(OH)}}_2+H_2{O}_2$

How do superoxides react with water?

Superoxides react with water to produce hydroxide (OH^-), hydrogen peroxide (H₂O₂), and oxygen gas (O₂). For example, potassium superoxide (KO₂) reacts with water as follows:

$2{\mathrm{KO}}_2+2H_2{O}_1\to 2{\mathrm{KOH}}_1+H_2{O}_2+O_2$

What are the products of the reaction between sodium peroxide and hydrochloric acid?

When sodium peroxide (Na₂O₂) reacts with hydrochloric acid (HCl), it produces sodium chloride (NaCl) and hydrogen peroxide (H₂O₂). The balanced chemical equation for this reaction is:

$1{\mathrm{Na}}_2{O}_2+2{\mathrm{HCl}}_1\to 2{\mathrm{NaCl}}_1+H_2{O}_2$

What are the products of the reaction between potassium superoxide and nitric acid?

When potassium superoxide (KO₂) reacts with nitric acid (HNO₃), it produces potassium nitrate (KNO₃), hydrogen peroxide (H₂O₂), and oxygen gas (O₂). The balanced chemical equation for this reaction is:

$2{\mathrm{KO}}_2+2{\mathrm{HNO}}_3\to 2{\mathrm{KNO}}_3+H_2{O}_2+O_2$

How do peroxides and superoxides differ in their reactions with acids?

Peroxides and superoxides differ in their reactions with acids in the following ways:

1. Peroxides react with acids to produce a salt and hydrogen peroxide (H₂O₂). For example, sodium peroxide (Na₂O₂) reacts with hydrochloric acid (HCl) to form sodium chloride (NaCl) and hydrogen peroxide:

$1{\mathrm{Na}}_2{O}_2+2{\mathrm{HCl}}_1\to 2{\mathrm{NaCl}}_1+H_2{O}_2$

2. Superoxides react with acids to produce a salt, hydrogen peroxide, and oxygen gas (O₂). For example, potassium superoxide (KO₂) reacts with nitric acid (HNO₃) to form potassium nitrate (KNO₃), hydrogen peroxide, and oxygen gas:

$2{\mathrm{KO}}_2+2{\mathrm{HNO}}_3\to 2{\mathrm{KNO}}_3+H_2{O}_2+O_2$