Question

Write the balanced chemical equation for each of the following reactions between water and the non-metallic oxide to form an acid. $$ \begin{array}{l}{\text { a. } \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { b. } \mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { c. } \mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow}\end{array} $$

Short answer

The balanced equations are: \( \mathrm{CO}_{2}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3}(aq) \), \( \mathrm{SO}_{3}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(aq) \), \( \mathrm{N}_{2} \mathrm{O}_{5}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_3(aq) \).

Step-by-step solution

Identify Reactants and Products

Identify that the reactants are a non-metallic oxide and water. The products will be acids formed when these reactants combine.

Step 2a: Balance Equation for CO2 and H2O

Determine the product for the reaction between CO2 and H2O. The product is carbonic acid, H2CO3. Write and balance the equation: \[ \mathrm{CO}_{2}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3}(aq) \]

Step 2b: Balance Equation for SO3 and H2O

Determine the product for the reaction between SO3 and H2O. The product is sulfuric acid, H2SO4. Write and balance the equation: \[ \mathrm{SO}_{3}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(aq) \]

Step 2c: Balance Equation for N2O5 and H2O

Determine the product for the reaction between N2O5 and H2O. The product is nitric acid, HNO3. Write and balance the equation: \[ \mathrm{N}_{2} \mathrm{O}_{5}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_3(aq) \]

Key concepts

Chemical Reactions

Chemical reactions involve the transformation of one or more substances into new substances. In our exercise, the reactions involve a type of chemical reaction called a 'synthesis reaction', where two reactants combine to form a single product. Here, non-metallic oxides react with water to create acids. This is a common type of reaction in chemistry.

When balancing chemical reactions, it is essential to ensure that the number of atoms for each element is the same on both sides of the equation. This principle is known as the Law of Conservation of Mass. For instance, in the reaction between CO2 and H2O, we end up with H2CO3 (carbonic acid), maintaining the balance of atoms between reactants and products.

Acid Formation

Acid formation often occurs when non-metallic oxides react with water. The resulting compounds are usually acids, which are substances that release hydrogen ions (H+) in a solution.

For example, when CO2 (carbon dioxide) reacts with H2O (water), it forms H2CO3 (carbonic acid). Similarly, SO3 (sulfur trioxide) combines with H2O to produce H2SO4 (sulfuric acid), and N2O5 (dinitrogen pentoxide) reacts with H2O to produce HNO3 (nitric acid). These reactions are significant in both natural processes and industrial applications.
Understanding acid formation helps us grasp broader environmental concepts, such as acid rain, which is caused by non-metallic oxides like SO2 and nitrogen oxides dissolving in water droplets in the atmosphere.

Non-Metallic Oxides

Non-metallic oxides are compounds formed between non-metal elements and oxygen. They are typically acidic oxides and contribute to acid rain when dissolved in water. In our exercise, three non-metallic oxides are given: CO2 (carbon dioxide), SO3 (sulfur trioxide), and N2O5 (dinitrogen pentoxide).

When these oxides react with water, they form acids. For example:

• CO2 reacts with water to form carbonic acid (H2CO3).
• SO3 reacts with water to form sulfuric acid (H2SO4).
• N2O5 reacts with water to form nitric acid (HNO3).

This type of reaction is useful in various applications, including industrial chemistry and environmental science, to understand the implications of these oxides in the atmosphere and their role in pollution.